DEPARTMENT OF THE INTERIOR

BULLETIN

OP THH

UNITED STATES

GEOLOGICAL SURVEY

No. 55

WASHINGTON

GOVERNMENT PRINTING OFFICE 

1889

UNITED'STATES-GEOLOGICAL SUEVEY

J. W. POAVELL, DIRECTOR

REPORT OF WORK DONE

IN THK

DIVISION OF CHEMISTRY AND PHYSICS

MAINLY DURING THE

YEA.R 1886-'87

FEANK WIGGLESWOETH CLAEKE, CHIEF CHEMIST

WASHINGTON"

GOVERNMENT PRINTING OFFICE 

1889

179469

CONTENTS.

SCIENTIFIC PAPERS.

Page. 

Letter of transmittal........................................................ 9

Studies in the mica groups. By F. W. Clarke ...... ......................... 12

The analysis and composition of tourmaline. By R. B. Riggs................. 19

Notes on certain rare copper minerals from Utah. By W. F. Hillebraud and 

H. S. Washington......................................................... 38

Mineralogical notes. By W. F. Hillebraud........................ ........... 48

Analyses of some natural borates and borosilicates. By J. Edward Whitfield.. 56 

On the Johnson County, Ark., and Alien County, Ky., meteorites. By J. Edward Whitfield............................................................ 63

Scorodite from the Yellowstone Park. By J.Edward Whitfield............... 65

Flow of solids, or behavior of solids under high pressure. By William Hallock. 67

MISCELLANEOUS ANALYSES.

Feldspar from the Hoosac Tunnel............................................ 79

Two feldspars from Greylock Mountain, Massachusetts ....................... 79

Three feldspars from Delaware ...... ........................................ 79

Triassic sandstone from Maryland ........................................... 80

Limestone from the Auglaize River, Ohio ...................... .............. 80

Twelve rocks from the Menomonee River .................................... 81

Rocks from Pigeon Point, Minnesota........... .............................. 81

Two rocks from Montana.................................................... 83

Fifteen rocks from California................................................. 84

Ores of iron and manganese ................................................. 85

Coals ....................................................................... 87

Iron and steel...................^........................................... 87

Kitre from Utah............................................................. 88

Salt from Warsaw, N. Y...................................................... 89

Two clays from Owen's Lake, California ..................................... 89

Clay,'sand, etc., from Martha's Vineyard .................................... 89

Water from Paris, Me ....................................................... 91

Waters from Savannah, Ga .................................................. 91

Artesian wells in Georgia and Alabama...................................... 91

Water from Arkansas........................................................ 92

Water from a spring near Fort Wingate, N. Mex ............!................ 92

Water from Owen's Lake, California......................................... 93

5

ILLUSTRATIONS.

Papc.

Plate I. Diagram of apparatus used in work on high pressure................ 70

FiG. 1. Crystalline form of olivenite ...- .--...--------...-..----......--- . 39

2. Crystalline form of chalcophyllite ................................... 43

3. Crystalline form of clinoclasite...................................... 43

4. Crystalline form of clinoclasite...................................... 43

5. Crystalline form of clinoclasite...................................... 44

6. Crystalline form of brochautite.. ........................ ............ 4(i

7. Crystalline form of brochantite ..................................... 40

8. Crystalline form of brochautite ...................................... 46

9. Samarskite......................................................... 48

10. Cyrtolite ........................................................... 52

11. Cyrtolite........................................................... 52

12. Crystalline form of colemanite ...................................... 57

13. Crystalline form of colemanite ...... ................................ 57

14. Diagram of apparatus used iu work on high pressures.:.............. 70

15. Diagram of apparatus used in work on high pressures ................ 70

16. Diagram showing experiment......... ........................... 71

LETTER OF-TRANSMITTAL.

DEPARTMENT OF THE INTERIOR, 

UNITED STATES GEOLOGICAL SURVEY,

Washington, D. 0., January 1,1888.

SIR : This bulletin, like its predecessors Nos. 9, 27, and 42 represents some of the more important work done in the Division of Chemistry and Physics during one fiscal year. It does not by any means 

cover all the work completed in the laboratories, but only those portions which were considered far enough advanced for publication. 

Several other researches are very nearly finished, and will duly appear 

either as independent bulletins or in the next annual bulletin of the 

division.

In one investigation we are indebted to Mr. H. S. Washington, of 

New Haven, for his kind co-operation. His name appears with Dr. 

Hillebrand's, as joint author of a paper herewith presented.

F. W. CLARKE,

Chief Chemist. 

Hon. J. W. POWELL,

Director U. S. Geological Survey.

9 

SCIENTIFIC PAPERS.

11

WORK DONE IN THE DIVISION OF CHEMISTEY AND

PHYSICS IN 1836-87. .

STUDIES IN THE MICA GROUP.

BY F. W. CLAKKE.

I. MUSCOVITE FROM ALEXANDER COUNTY, N. 0.

This mica occurs in overlapping, crystalline plates, implanted edgewise in pockets at the well-known locality for emerald and hiddeniteat 

Stony Point. The plates are several centimeters in diameter, w}th 

sharply defined crystalline boundaries; and in the specimens before me 

they are associated with crystallized dolomite, pyrite, and rutile. All 

of these minerals are more or less dusted over with a dark-green chloritic coating, which, together with some ferruginous staining, gives the 

mica a somewhat bronzy appearance. An analysis made on carefully 

purified material gave the following results:

Ignition :................................................... 5. 46

Si02 ....................................................... 45.40

TiOz ....................................................... 1.10

A1203 .-.................................................... 33.66

Fe203 ......--....-..-...........---.....-.- --...---....--. 2.36

MgO ...................................................... 1.86

CaO....................................................... none

Li2O....................................................... trace

Na20 ...................................................... 1.41

KsO....................................................... 8.33

F.......................................................... .69

100. 27 

Less oxygen ............................................... .29

99.98

This, except for the presence of titanium, is the composition of an 

ordinary muscovite. Possibly the titanium may be due to minute inclusions of rutile, but none such were detected. It is more probably 

present as a replacement either of silica or of alumina.

One of the smaller plates of this mica was examined microscopically 

by Mr. J. S. Diller, who has kindly furnished the subjoined notes:

The group of muscovite scales shows well-defined crystallographic outlines, most 

prominent among which are the clinopinacoid and the unit prism, although a small 

clinodiagonal prism is also common. Parallel with the latter there are indistinct

13
14 WASHINGTON LABORATORY. [BULL. 55.

cleavage lines, which in the basal plane make an angle of 31° -with the edge between 

the basal plane and the clinopinacoid. The angle of the optic axes, measured in oil 

in a plane perpendicular to the plane of symmetry, is 35°.

The muscovite is partially coated by a greenish dnst, which in its arrangement 

follows crystallographic lines, giving to the scales a streaked appearance. It appears most abundantly upon the prismatic edges, but to a considerable extent also 

upon the clinopinacoid, and in traces on the clinodiagonal. Thin laminae of dust 

occur between the folise of the muscovite, to which they impart a yellowish tinge in 

reflected light. This dust appears to be weakly doubly refracting, but its structureless character and want of definite optical properties render its determination a matter of difficulty.

With some trouble I collected a little of this chloritic dust, 0.3165 

gramme iu all, and made a partial analysis of it, as follows:

Ignition .......................................... 20.50

Si03 .......... .................................... 31.16

A12O3 ............................................. 8.06

FeaOs............................................. 35.86 = 32.28FeO.

MgO............................................... 5.43

101.01

The iron is undoubtedly present chiefly, but not wholly, in the ferrous 

state; and the aininina is ascribable to traces of admixed mica. Still, 

with all its defects, the analysis clearly defines the mineral as a member of the obscure hisingerite group, which has rarely been noted in 

this country. Its association with pyrite is similar to some of its occurrences abroad, and here, as observed elsewhere, it may originate in 

the alteration of that species. I hope to give it a fuller examination 

sometime with a larger supply of material. For the specimens so far 

studied I am indebted to the kindness of Mr. Wm. Earl Hidden.

II. LEPIDOMELANE FROM BALTIMORE, MD.

This mineral, the characteristic black mica of the Jones Falls pegmatite, was sent me for analysis by Dr. Gr. H. Williams, of the Johns 

Hopkins University. The specimen submitted was in broad, brilliant 

foliations, black by reflected light, but dark smoky green by transmitted light. According to Dr. Williams it is very nearly uniaxial. 

In the following analysis the direct estimation of water and the determination of ferrous iron were made by Mr. E. B. Eiggs:

H2O ........................................................ 4.48

SiOa........................................................ 35.78

A1203 ....................................................... 16.39

Fe203 ....................................................... 14.55

FeO ........................................................ 11.02

MnO ....................................................... 1.08

CaO........................................................ none

MgO ....................................................... 8.67

K3 0 ........................................................ 7.76

NaaO ....................................................... .56

TiOs.-.-,..,,--.. ,-,...................................... none

100.29
CLARKE.] STUDIES IN THE MICA GROUP. 15

Beckoning the water with the alkalies, the analysis gives approximately the formula B'6R// 3R///4Si 5O22 . The mineral, therefore, is slightly 

too basic for an ordinary orthosilicate, and it seems to occupy an intermediate position, as do its ratios, between annite and the Litchfield 

lepidomelane.

III. LEPIDOMELANE FROM LITCHFIELD, ME.

In a previous paper upon the minerals of Litchfield 1 1 gave an analysis of this mica, together with some data as to its occurrence. It is 

scattered abundantly through the elseolite syenite of the locality, in 

black brilliant plates or scales, which are transparent only in very thin 

laminae, and then transmit light of a dark green color. It is one of the 

least transparent micas I have ever seen. According to Mr. Diller, 

who kindly made a microscopic examination of the mineral, it is so 

nearly uniaxial, that a measurement of its optic axial angle is impracticable. Some specimens show evidence of two micas, one being blacker 

and more brittle than the other, so that a new analysis was made upon 

very carefully selected material. Only the more transparent and elastic folise were chosen, and the results are given below :°

H<,0 ................................................. 4.67

Si03 . ................................................ 32.35

A1203 .. ..........-..^.... ............................ 17.47

FeO.. ............................................... 13.11

MnO ................................................ 1.02

CaO. ................................................ .89

MgO ................................................ none

NasO ................................................ .70

K20 ................................................. 6.40

TiOa ................................................. none

100.83

THE DETERMINATIONS FOR IRON IN THE FERROUS STATE AND FOR WATER.

The ferrous iron and water determinations were made by Mr. Biggs. 

Titanium was carefully sought for by two methods in three separate 

tests, but only a doubtful trace was discovered. The formula of the 

mica, reckoning water with the alkalies, is very nearly B'6R//2B/ "6Si5O24.

This mica, on account of its low percentage of silica and its basic 

nature, has peculiar interest. Among published analyses of micas I 

find only two which approach it in these particulars, namely the micas 

from Brevig and Miask, described by C. Bammelsberg.2 These gave respectively 32.97 and 32.49 per cent, of silica, but they also contained, 

the first 2.42 and the second 4.03 of titanic oxide. This constituent, as

'Bull. U. S. Geological Survey, No. 42, p. 35. 

2 Ge'oJ. Gesell, Zeitschr., vol. 31, 676-691.
16 WASHINGTON LABORATORY. [BULL. 55.

has been stated, is lacking in the Litchfield mineral. JSotably all three 

of these low silica micas are from localities of elseolite syenite, although 

Kaininelsberg says nothing of the actual associations of the specimens 

discussed by him. The question at once arises, to be settled by future 

investigation, whether micas of this peculiar character are representative of elseolitic rocks, and whether there is any genetic relation between them and eleolite. I hope that observations upon this poiut 

may soon be multiplied.

Some mouths ago I published some analyses of the Eockport micas, 

which were made by Mr. Eiggs in this laboratory. 1 One of these, the 

so-called annite, seems to have a serial relation with the analogous 

micas from Baltimore and Litchfield, which may be expressed in formulae, These, stated in empirical form,are as follows:

Rockport...................................... ....R'6R"4R'"2Si 502o

Baltimore .........................................R/6R"3R"/48i602.2

Litchfield.........................................R/6R^R"/6Sifi024

Here we have E' and silicon constant, while a gain of E///2O2 corresponds in each step to a loss of one atom of E". If now we assume 

that E'^Oz represents really two of the recognized univalent groups 

 A1=O, we shall find that all three of the micas, reduce to the true 

orthosilicate type, containing the nucleus E'"2 (SiO4 )5 , which appears to be 

characteristic of many iron micas and of the phlogopite group. We 

thus have, uniting all the monoxide bases, the following general formulae :'

Rockport..................................... R/, 4R"/a(SiO4 )6

Baltimore.....................................R'12 (A10)2R'//2 (Si04 )5

Litchfield............................ .........R/ io(AlO)4R'"2 (SiO4)5

In short, the three micas are built upon the same fundamental plan, 

and exhibit a new and highly suggestive order of variation.

IV. IRON-BIOTITE FROM AUBURN, ME.

Among the minerals occurring at the well-known lepidolite locality at 

Auburn a brilliant black biotite is common. Some time since, in looking over a collection of the Auburn material in the possession of Mr. 

N. H, Perry, of South Paris, I observed that certain broad foliar of this 

mica were bordered by a grayish distinct margin, about 5mm wide, which 

was made up of micaceous scales. Inasmuch as the lepidolite of the 

locality forms similar borders upon the muscovite, I thought that this 

bordering might have interest, and Mr. Perry kindly placed his best 

specimen at my disposal. Analyses of both the biotite and the margin 

were made, but unfortunately the amount of the latter available was 

too small for complete investigation. In the study of the border, therefore, ferrous iron and water had to be neglected, and that analysis is

'Bqll. U. S. Geological Survey, NO. 42, p. 22.
CLARKK.] STUDIES IN THE, MICA GROUP. 17

so far incomplete. The results are given below, with determinations of 

water and ferrous iron in the biotite made by Mr. Biggs:

HaO.. ...........

SiO2 ............

A1203 ...........

FesO, ...........

Fpf)

MnO ............

MgO... ......... O

CaO ............

Na,0. .......... .

K9O.. ...........

F ...............

Less oxygen.... .

Biotite.

4. 64

34. 67

30.09

2.42

16.14

.85

1.98

none

1.67

7.55

 .28

100. 29 

.12

100. 17

Margin.

nndet.

56.44

16. 01 ,

| 15. 91

nndet.

.97

none.

1.92

6.15

.71

Upon microscopic examination by Mr. Diller the mica was found to 

be "almost completely uniaxial,for when it was rotated between crossed 

nicols the displacement of the black cross was scarcely perceptible." 

He also found that the same mica, with a slight change of color from 

brown to greenish brown, continued into the border, where it was intimately mingled with grains and fibers of quartz. The latter admixture 

accounts in part for the high percentage of silica in the margin, although 

it seems probable that there may be also some degradation, from the 

original orthosilicate toward a inetasilicate type. At all events the 

specimens are in nowise analogous to those which show lepidolite borders upon muscovite.

In its ratios this Auburn mica is not simple. Approximately, reducing all monoxides to the univalent type, its formula may be written 

R'n(AlO)3Al2(SiO4 }5; with R/11 =E4K2Feg j4 . It seems to be a compound 

intermediate between the Litchfield and Baltimore micas, with R"' 

nearly all aluminum.

V. IRON-MICA FROM THE VICINITY OF PIKE'S PEAK.

This specimen, which was kindly given me by Mr. C. S. Bement, was 

a section from a large prismatic crystal in his collection. It was a 

bronzy black mica, resembling phlogopite externally, but remarkably 

altered at the center. The entire core of the crystal was made up of a 

soft, rotten material, evidently derived from, the original mica, and surrounded by a broad black margin of the latter. Streaks of rusty alteration products reached into the margin in every direction, so that no 

Bull. 55 2
18 WASHINGTON LABORATORY. [BULL. 55.

absolutely unchanged material could be obtained for analysis. According to Mr. Diller, the angle of the optic axes is too small for measurement.

Analyses were made of both margin and center, the former being as 

little altered, the latter as much altered, as could be selected.

Again I am indebted to Mr. Riggs for determinations of water and 

ferrous iron:

H2 0. ..............

SiO3 ..............

A1203 -. ............

PW>3 .............

FeO-. .............

MnO. .............

CaO ..............

MgO. .............

NaaO. ....... ......

KBO. ..............

F .................

Margin.

4.54

34.21

16.53

- 20. 15

14.17

01

.48

1.34

1.43

6.50

.08

100. 34 

.03

100. 31

Center.

Ignition 7. 82

34. 63

17.95

31.25

3.01

.34

.81

1.08

8Q

1 Qfi

.54

100. 28 

.23

' , 100. 05

These figures show the order of alteration so well, that comment upon 

them is unnecessary. The original mica probably was very near Lewis's 

siderophyllite, but it is hardly worth while to discuss the ratios.
THE .ANALYSIS AND COMPOSITION OF TOURMALINE.

BY R. B. RlGGS.

Apart from the work by Rammelsberg 1 very little has been done 

towards solving the question of the composition and constitution of 

tourmaline. Its apparent complexity and the difficulties attending the 

determination of certain constituents have doubtless turned many aside, 

possibly also the impression that with Rammelsberg's investigations the 

matter was settled. While Eammelsberg's work was comprehensive, 

and was possibly good for the times, his analyses are so seriously 

faulty in certain important respects as to justify a new investigation. 

Though the direct estimation of both water aud boric acid would seem 

to be of the highest importance before any satisfactory conclusions 

could be reached with reference to the constitution of tourmaline, we 

find that, having failed in one single attempt to determine the water 

directly, he takes the loss on ignitiocu, deducts therefrom an amount 

equal to the amount of silicon tetrafluoride, representing the fluorine 

found in the mineral, and calls the rest water. He takes it for granted 

that the fluorine is driven off (quantitatively. While this supposition 

is questionable, it is not the main ground of Objection. In the revision2 

of his earlier work Rammelsberg conies to the conclusion that the 

iron contained in tourmaline is all there in the ferrous condition, yet 

he wholly ignores the fact of its possible oxidation on ignition, especially 

an ignition such as would be necessary to expel the fluorine.'

In a few cases boric acid was determined directly, but by a method 

(Stromeyer's) which has ever been counted as one of the most unsatisfactory. In the majority of analyses boric acid was estimated by difference. B\it if the results called water are incorrect and low, as they 

surely are, the boric acid ought to be correspondingly high, or the 

analysis must be faulty in other respects.

The direct estimation of water being possible, and a satisfactory 

method for determining boric acid having lately been devised by Dr. F. 

A. Gooch,3 new tourmaline analyses seemed desirable. ^

i Pogg. Arm., vol. 80, p. 449; vol. 81, 1 p.; vol. 139, pp. 379, 547.

2 Pogg. Ann., vol. 139, p. 379.

3 Bull. U. S. Geological Survey, No. 4'<i, pp. 64-72.

19
20 WASHINGTON LABORATORY. [HULL. 55.

Through the kindness of many persons, abundant and varied material has been at my disposal.

. METHODS OP ANALYSIS.

A few words on the methods of analysis may not be out of place 

here, that the character of the work may be the better judged.

Water. The water was directly determined by igniting a mixture of 

the mineral and carbonate of soda in a Gooch tubulated crucible, the 

sodium carbonate being used to hold back any fluorine that might 

otherwise be driven off. The carbonate of soda was first fused, and 

then, in order to insure perfect dryness, the mixture of the mineral and 

this reagent was again dried in an air bath at 105° C. for two or three 

hours. This estimation, as well as all the other more important ones, 

was made in duplicate.

Boric acid. When the tourmaline contained fluorine, the same mate-' 

rial was used for determining both the boric acid and the fluorine, the 

filtrate from the mixed carbonate and fluoride precipitates being used 

for the estimation of the boric acid. The calcium borate (cf. line 7, 

page 16) which may be formed is so readily soluble in hot water that 

no difficulty is experienced in bringing it quantitatively into the filtrate. 

After evaporating this filtrate to a conveniently small volume, it is 

brought into the retort and acidified with nitric acid. The boric acid 

is then volatilized as methyl borate, according to the Gooch method, 

and weighed as borate of lime. It is scarcely necessary to say that 

throughout this treatment nitric acid should be used as the neutralizing reagent, and that, if care be taken in its use, in no case does the 

amount of salt which is to be brought into the retort become inconveniently great. Where no fluorine is present the soda fusion may be 

digested with water at once, the solution containing the sodium borate 

filtered off, neutralized, and treated as above indicated. One might 

save himself even this filtration but for the fact that in using the whole 

fusion a quantity of bases would thus be brought into the retort, which, 

even at the low heat required by the distillation, would give up their 

nitric acid, thereby rendering the determination in its after stages more 

difficult, and possibly less exact.

Fluorine. The fluorine was estimated by the Berzeliau method. 

Though it is far from a good method, care and experience enable one to 

obtain fairly trustworthy determinations. The tendency is towards too 

. high results, because of the difficulty of freeing the calcium fluoride 

from last traces of alumina and silica, and a better method-will probably show even less fluorine to be present in tourmaline than the insignificant quantity now found.

Ferrous oxide. Tourmalines, particularly the lithia and iron varieties, are decomposed by acids with extreme difficulty. This fact, together with the fact.that the iron in tourmaline (possibly from some
KIGGS.] ANALYSIS AND COMPOSITION OF TOURMALINE, 21

inherent organic reason, such as the high and unstable degree of oxidation of the boric acid) oxidizes with unusual ease, has made the deterininati'on of the condition of this constituent most troublesome. On 

account of its refractory nature, usually not more than 0.2 gramme of the 

finely ground mineral was taken for this determination. Several methods of decomposition were tried without any satisfactory results other 

than to lead to the conviction that the presence of ferrous iron in large 

amounts was doubtful until the digestion of the mineral with hydrofluoric acid in a sealed platinum crucible over the direct flame was resortedto, with fairly conclusive results.

(1) The mineral was digested with hydrofluoric and sulphuric acids 

in a sealed platinum crucible immersed in boiling water from oue to 

seven days, a treatment which decomposes most minerals in the course 

of a few hours. In a few cases complete decomposition seemed to have 

been effected; in the greater number, however, it was at the best very 

incomplete. In no case was more than 1 per cent, of ferrous oxide 

found, though between thirty and forty experiments were made, and 

some of the tourmalines analyzed contain as high as 11 per cent, of iron. 

These determinations were made in a deep heavy platinum crucible of 

about 60CC capacity. This crucible has a flaring mouth, into which fits 

a platinum head securely held in place by a gallows screw clamp. 

Though the joints are ground, a rubber washer is inserted between the 

cap and the lips of the crucible to insure a tight fit. Before sealing 

the crucible a little carbonate of ammonia is thrown in to expel the air. 

During the period of digestion the crucible is kept completely immersed 

in water, so that it is difficult to comprehend how the outside air can 

play any part in the oxidation of the iron. I am accordingly tempted 

to think that we have here to deal with a very slow reduction of the 

highly oxidized condition of the boric acid, at the expense of which there 

is a corresponding oxidation of the iron. That this change goes on 

slowly, if at all, is evident from the possibility of effecting a decomposition unaccompanied by it.

 -(2) From 0.2 to 0.5 grammes of the mineral were heated with sulphuric 

acid 4 parts acid to 1 of water in sealed glass tubes, from oue to four 

days, at temperatures varying from 150° C. to 250° C. Although the 

tubes were frequently taken out of the bath and shaken, decomposition 

in none of the fifteen attempts was more than partial. As even the best 

acid contains organic matter, sometimes in considerable quantities, a 

high heat, i. e., above 200° C., is likely to be attended by a reduction of 

the acid, thus vitiating the results.

(3) The mineral was also fused with.bisulphate and bifluoride of potassium, respectively, in an atmosphere of carbon dioxide. Though decomposition was usually effected in a couple of hours, the iron was invariably all oxidized. A reduction of the sulphuric acid may be the 

cause of the results when bisulphate of potassium was used. No such 

explanation avails in the case of the bifluoride fusion.
22 WASHINGTON LABORATORY. [BULL. 55.

(4) Convinced, by the summations of some of the analyses and by 

comparing the loss on ignition with the corresponding direct water determinations, that the iron in tourmaline must be there, in large part.at 

least, in the ferrous condition, I finally heated the mineral with hydrofluoric and sulphuric acids in the closed platinum crucible over the direct flame, thus digesting at a moderately high temperature and a correspondingly high pressure, and at the same time securing a constant 

agitation of the powdered mineral. In these determinations a thin lead 

washer replaced the rubber. Half an hour with these conditions usually 

sufficed to effect complete decomposition. The crucible was cooled in 

an atmosphere of carbon dioxide and the iron was determined in the 

usual way with a potassium permanganate solution. Fair results were 

obtained, such as to indicate that the iron in tourmaline is there chiefly 

in the ferrous condition5 the conclusion which Eammelsberg reached 

as the result of Mitscherlich's experiments1 , confirmed by a few determinations of his own.

Alkalies. Several vain attempts were made to decompose the tourmaline with hydrofluoric and sulphuric acids. As showing the refractory nature of the mineral, the following is a case in point: One gramme 

of the pale greeii Auburn variety, after being ignited, was evaporated 

to dryness 'with about 20ce of hydrofluoric acid five times and left an 

insoluble residue of 0.473 gramme. The Lawrence Smith method was 

finally adopted, and with -highly satisfactory results. The only precautions necessary are that the mineral be finely powdered, and .that 

the mixture with ammonium chloride and calcium carbonate be intimate, which latter condition is only to be secured by grinding the 

several ingredients together. When these conditions are all that they 

should be, there is no trouble in bringing about complete decomposition in the course of an hour's gentle ignition. After the alkalies have 

been leached out with water, the residue should of course be treated 

with acid to test the completeness of the disintegration. In the case of 

the tourmalines, with their low silica percentages, the solution is usually 

complete if the decomposition has been perfect. After the alkalies 

have been freed from the other bases by the usual well-known methods, 

although the greater part of the boric acid will have been driven off by 

the repeated evaporations, more or less of it remains. This residual 

amount is removed by two or three evaporations with methyl alco.- 

hol. The separation of lithia from the other alkalies was made by the 

Gooch method,2 by boiling the mixed chlorides in amyl alcohol, and 

further separations were effected in the usual way.

Silica. On the strength of the belief that tourmaline sometimes contains fluorine in considerable amounts, the silica was at first estimated by precipitating it with carbonate of ammonia. Where the 

bases thrown down by this reagent are so in excess of the silica as 

they are in tourmaline, its precipitation is fairly easy and quantitative.

1 Jour. Prakt. Chemie, vol. 86, p. 1. 2 Bull. U. S. Geol. Survey, No. 42.
MOOB.] ANALYSTS AND COMPOSITION OF TOURMALINE. 23

Nevertheless, where this method was used, of duplicate determinations 

the higher is taken in the summation. Save where the silica is greatly 

in excess of the-bases thrown down by ammonium carbonate, the addition of zinc compounds, as is commonly recommended, is wholly unnecessary. In fact, even in dealing with such minerals as the 

lepidolites, which contain about 50 per cent, of silica and only 30 per 

cent, of alumina, the addition of zinc compounds gives no better results 

than are obtained by simple evaporation with carbonate of ammonia, 

the evaporation being repeated several times.

As soon as it became evident that the amount of fluorine, if present 

at all, was so small that its influence in carrying off silica could be 

neglected, the ordinary method of separation was employed. In all 

cases silica was corrected by evaporation with hydrofluoric acid.

Alumina. The only point worthy of mention in this connection is the 

necessity of testing the alumina for the silica which it frequently contains. This is usually done by fusing the ignited product with potassium bisulphate. Where it amounts to as much as it does in tourmaline, 

generally exceeding four-tenths gramme, a carbonate of soda fusion 

works more satisfactorily; it can be continued longer and at a higher 

temperature, This fusion is readily converted into a sulphate fusion, 

and the desired separation is thus accomplished. Several fusions are 

sometimes necessary to bring the bases into solution. As regards other 

determinations nothing in particular need be said.

ANALYSES.

Analyses have been made of material from the following localities: 

Auburn, Eumford, and Paris, Me.; Calhao, province of Minas 

Geraes. Brazil; De Kalb, Gouverneur, and Pierrepont, N. Y.; Hamburgh, N. J.; Orford, N. H.; Monroe and Haddam, Conn.; Stony Point, 

N. C.; and Nantic Gulf, Baffin Land, well representing the variations 

in physical properties and chemical composition which characterize 

the different varieties of tourmaline.

For the sake of compactness the results of these analyses have been 

grouped. The tourmalines from Maine and those from Brazil are thrown 

together according to localities, though, barring the iron varieties, they 

should be classed together on the basis of their composition, on which 

basis those from other localities are roughly grouped.

Maine. These tourmalines occur in veins of albitic granite, the chief 

constituents of which are quartz, albite, and muscovite, with lepidolite 

and beryl -as important accessories. At Eumford spodumene is abundant.

Auburn. A. Colorless to very pale green crystals, some of which 

were tinged faintly pink and blue, infusible. Sp. gr., 3.07. B. Light 

green, fragile crystals, infusible. C. Dark green, massive tourmaline;
24 WASHINGTON LABORATORY. [BULL. 55.

fuses with difficulty. D. Massive black tourmaline, easily fusible. Sp. 

gp., 3.19.

A. B. C. . D.

/ 

Si02 ...38.14

A12O3 ... 39.60 1

Fe2O3 ... .30 I 

FeO.... 1.38 (

TiO-2 .. .uonej

P2O5 .. .trace

MnO... 1.38

CaO.... .43

MgO.. .trace

Li20 ... 1.34

Na2O... 2.36

K2 0.... .27

H2 0,... 4.16

B203 .-.. 10.25

F...... .62

100.23

Less O .26

i. n.

.... 38.00 37.85

37.73]

49 1 > 41.37-41.48 -^ > 

3.88 f

nonej

trace

.51

.49

.04

1.34

2.16

.62

4.06- 4.26 4.18

10.15-10.34 10.55

..... .72 .62

100.39

.26

I. II. I. II.

.... 37.SO 36.26 .... 36.18

36.681

42.37-42.54 -15 144.05-44.73 

7.07 f

nonej

trace

.72

' .17

.16

1.05

. 2.88

.44

4.16- 4.20 4.05 4.00- 4.11

9.94 9.83-10.04

.72 .71 .... .80

 100.28

.30

'

34.99

33.96 1

none \ 

14.23 f

nonej

trace

.06

.15

1.01

trace

2.01

.34

3.62

9.63

none

100.00

i. 'ii.

.... 34.87

49.76-49.79

3.56- 3.68

9.44- 9.82

90.97 100.13 99.98

The material for the above analyses was received from Mr. N. H. 

Perry, of South Paris, Me.

Rumford, Black Mountain. A. Massive, rose-colored, infusible. G., 

2.997.

B. Massive, dark green ; fuses with difficulty.

Paris, Mount Mica. Massive, black, powder blue-black, easily fusible.

SiOa ............... 38.07

A1203 .............. 42.24

Fe2O3 .............. .....

FeO............... .26

B.

MnO ........

CaO.........

MgO ........

Li2O...... ...

Na20 ........

K20 ........

H2O.........

B3O3 ........

F ...........

....... .35

....... .56

....... .07

....... 1.59

....... 2.18

....... .44

...... 4.26

...... 9.99

....... .28

4.25- 4.28 

9. 85--10.13

100.29 

Less oxygen ....... .12

36. 53

38. 10

none

6.43

trace

.32

.34

none

.95

2.86

.38

3.52

10. 22

.16

99.81

.07

..... 36.42

3. 44- 3. 60

10. 03-10. 41

35. 03

34.44

1.18

12.10

trace

.08

.24

1.81

.07

2.03

.25

3. 69

9.02

none

99.89

Paris.

i. n.

34.99-35.06

3. 63- 3.75 

8.92- 9.12

100.17 99.74
MODS.] ANALYSIS AND COMPOSITION OF TOURMALINE. 25

For the Bumford material I am indebted to Mr. E. M. Bailey, of 

Andover, Me. The Paris tourmalines was kindly furnished me out of 

the National Museum collection.

In connection with the Maine tourmalines the following interesting 

alteration products were studied:

A. An alteration from the light green Auburn (B) variety.

B. Flesh-colored alteration product from the Bum ford locality.

C. An alteration from the Hebrou rubellite.

A. B. C.

Si02 ............................................... ...... 53.03 43.90

Als03 ....................................-.......'. ...... 31.67 38.71

PeaOs-............................................. ...... .51 .58

FeO............................................... ...... ...... .25

MnO .............................................. ....... trace .04

CaO............................................... ...... trace .41

MgO .............................................. ...... trace .05

LisO............................................... 2.86 .20 ......

Na«0 .............................................. 2.16 .54 1.05

K20 ............................................... 9.64 9.44 10.92

H2O ............................................... ...... 4.80 4.25

B2 0:i............................................... trace trace trace

F.................................................. ...... trace? none

100.25 100.16

While the light green Auburn tourmalines were mostly translucent 

crystals, a few were found which, having become partially opaque, had 

assumed a micaceous structure. With scant material only the above 

partial analysis was possible. The results indicate a change in the direction of lepidolite.

The Bumford alteration was examined microscopically by Mr. J. S. 

Diller, who observed as follows:

Under the microscope it is seen to be composed of two minerals most thoroughly 

intermingled in nearly equal proportions. One of these minerals is micaceous in 

structure, with strong double refraction like damourite, which it closely resembles 

in general appearance. The other mineral is clear, colorless, and apparently monoclinic, with a rather low index of refraction and moderately intense double refraction.

While the Hebron rubellite alteration retains its crystalline form, its 

material is altered into a softer mineral of an opaque, talcose appearance. The analysis shows the change to be towards damourite, 1 and not 

towards lepidolite as has been supposed.

Brazil. Calhao, province of Minus Geraes. The association of these 

tourmalines I was unable to find out. From their composition, however, it is probable that it does not differ greatly from that of the Maine 

varieties. The specimensa nalyzed were supplied by Mr. G. F. Kunz.

A. The pink, almost colorless, center of crystals having a green 

border, infusible. Sp. gr., 3.028.

B. Pale green, like the border of A, infusible.

C. Olive green, fusible in very thin splinters.

1 F. W. Clarke, U. S. Geological Survey, Bulletin No. 42, p. 15.
26 WASHINGTON LABORATORY. [BOLL. 55.

D. Black, in splinters a smoky blue green, fuses easily. Sp. gr., 3.20. 

A. B. c. D.

Si02 . . .

A12 03 .-

FesOsFeO ...

PA---

MuO ...

CaO...

MgO ..

Li 2 0....

NosO ...

K2 0 ....

H2O....

B2 03 ...

F. ......

Lesaoxy

i. ii. 

....37.19 ..... 37.12

....42.431

....none L2 94.43 08

.... .52j

.... .79

.... .57

.... 1.73

.... 2 24

.... .23

... 3.90 3.86- 3.93

...10.06 9.96-10.16

99. 66 1 

gen.....

i. ii. 

37.39 ..... 37.31

39.65"! 

2; 29 | 42- 30-42. 38

trace J 

1.47 

.49 . 

none 

1.71 

2. 42 

.25 

3. 63 3. 60- 3. 66 

10.29 10.10-10.49 

.32 ..... .41

.00. 06 

.13

/ 

36.91 

38. 13 

.31 

3.19 

.11 

2.22 

.38 

.04 

1.61 

2.70 

.28 

3.64 

9.87 

.14

99.53 

.06

i. n. 

34.63 

32. 70 

.31 

13.69 

none 

.12 

.33 

2.13 

.08 

2.11 

.24 

3.49 

9.85-9.88 9.63 

.... .17 .06

99. 5'J 

.02

. " v

I. 11. 

34.50

3. 42-3. 56 

9. 55-9. 70 

.... .10

99.93 99.47 99.50

De Kail, St. Lawrence County, K. Y. Colorless to light brown translucent crystals in calcite, with quartz and titanic oxide inclusions, easily 

fusible. Sp. gr., 3.085.

Gouverneur, St. Lawrence County, N. Y. Brown, associated with calcite, easily fusible.

Hamburgh, '8. J. Large, cinnamon brown crystals, associated with 

calcite, quartz, and colorless mica, with many small, shiny, black scales 

of titanic oxide, easily fusible.

De Kalb. Gouverneur. 'Hamburgh.

II.

Fe2O3 .............

FeO..............

TiO, .............

P«0ft ... ......

MnO. ............

CaO .............

MgO ... .. ...

SrO. .............

BaO .............

Li2O .............

Na2O. .............

K2 0. .............

H.2O.. ............

B3 0 3 . ............

F. ...............

Less oxygen.. ....

.52

.12

nudet.

none

3.70

14.53

trace

none

trace

1.39

.18

3. 56 3. 55- 3. 57

10. 58 10. 46-10. 70

.50

100. 83

.21

f 

37.39

27.79

.10

.64

1.19

none

none

2.78

14.09

trace

none

trace

1.72

.16

3.83

10.73

trace?

i. ii.

37. 33-37. 45

3. 77- 3. 89

10. 63-10. 83

I. II.

100. 42

100. 62

35.25

28.49

none

.86

.65

trace

none

5.09

14.58

trace

none

trace

.94

.18

3.10

10.45

.78

100.37

.33

100.04

3.02-3.18
RIGG8.] ANALYSIS AND COMPOSITION OF TOURMALINE. 27

For the De Kalb and Hamburgh tourmaline I am indebted to Mr. G. 

F. Kunz. The Gouverneur material was from the National Museum 

collection.

From the large amount of titanic oxide found in the Gouverneur specimen it was feared that it might be there as an impurity. On examining a section microscopically Mr. Diller found it, on the contrary, to 

be quite free from inclusions of any kind. Specimens from other Gouverneur localities, viz, from the town of Gouverneur itself and from 

Eeese's farm, 7 miles north of the town, were also found to contain the 

oxide in large amounts. *

Orford, N. H. Dark brown crystals, in chloritic schist, easily fusible.

Monroe, Conn. Dark brown crystals, in chloritic schist, easily fusible.

Orford.

 A 

I,

Mouroo.

II. I, II,

SiO2 .................. 36.66

AliOs-......._...... 32.84

FeaOs................. none

FeO .................. 2.50

Ti08 .................. .23

PaOs.................. none

MuO.................. trace

CaO.................. 1.35

MgO.................. 10.35.

SrO .................. trace

BaO.................. none

Li20.................. trace

Na«O ................. 2.42

KaO .................. .22

H2O ...........-"....-. 3.78 3.77- 3.79

B203 .................. 10.07 9.86-10.28

F..................... trace?

100.42

36.41

31.27

none

3.80

1.61

trace

trace

.98

9.47

trace

none

none

2.68

.21

3.79

9.65

none

3. 76-3. 82

9. 57-9. 73

99.87

The Orford material was received from Prof. C. H. Hitchcock. The 

Monroe specimens came from the National Museum collection. The 

schistose gangue, in which the tourmalines from Orford and Monroe 

are imbedded, is of particular interest, and was studied microscopically 

as well as chemically, in the hope that it might throw light on the 

genetic relations of magnesian tourmaline. The microscopic work, 

which was of special importance, was kindly undertaken by Mr. J. S. 

Diller..
28 WASHINGTON LABORATORY.

Chemical analysis.

[BULL. 55.

Constituents.

Si02 ..............

A1203 .............

CaO ..............

MgO. .............

Na20...... .........

K30.... ...........

Orford.

27.18

33.10

.19

28.09

undet.

11. 75

100. 31

Monroe.

43.30

27.44

1.96

19.22

1.47

.60

7.45

101. 44

While Mr. Diller found the Orford matrix to be essentially chlorite, 

in agreement with the results of chemical analysis, the gangue rock 

of the Moiiroe tourmaline turned out to be particularly interesting.

Of this Mr. Diller says:

This light gray glittering rock is composed chiefly of biotite, chlorite, and alightcolored mineral which may possibly be zoisite. The biotite is very dark and apparently uniaxial and negative with all the other physical properties of the species. 

The chlorite is much paler than the biotite and of a greenish color. It is distinctly 

biaxial, with a small optic angle and positive. The relation of the chlorite to the 

biotite is readily seen in the thin sections, where it evidently is derived from the 

latter by a process of alteration. An interesting feature is that in the immediate 

vicinity of the imbedded tourmaline the biotite is all changed to chlorite, and is 

arranged with its folia approximately perpendicular to the crystallographic planes 

of the tourmaline, against which it impinges. The chlorite completely envelops 

the tourmaline, and the other portions of the hand specimen are made up chiefly of 

biotite aud the zoisitic mineral with a small proportion of chlorite. This variation in 

the mineralogical composition of the hand specimens readily explains the discrepancy that at first appeared to exist betw.eeu the results of chemical analysis and my 

observations.

o

That the analysis represents a portion of the rock rich in chlorite 

and poor in biotite, the high magnesia and low alkalies plainly show. 

The relation existing between the biotite, the chlorite, and the tourmaline in this Monroe matrix is of importance, indicating, as suggested, 

the transition to be from the mica through the chlorite to the tourmaline.

Pierrepont, St. Lawrence County, U. Y. Perfect black crystals? 

highly modified, associated with calcite,; fuses easily. Sp. gr., 3.08.

Nantic Gulf, Cumberland, Baffin Laud. Large black crystal, easily 

fusible. Sp. gr., 3.095.

Stony Point, Alexander County, 1ST. C. Perfect, medium-sized, black 

crystals, from the hiddeuite mine, with implanted crystals of quartz. 

The associated minerals are chiefly quartz, muscovite, apatite, rutile, 

beryl, and spodumene; fuses easily. Sp. gr.3 3.13.
RIGGS.J ANALYSIS AND COMPOSITION OF TOURMALINE. 29

Haddam, Conn. Black crystals in quartz and feldspar, powder blue 

black, easily fusible.

1

SiOa...

Ala03 -

Fe203 .-

FeO...

TiO2 ...

P205 ...

MnO ..

CaO...

MgO .. 

SrO....

BaO...

Li20...

N%O..

K20...

H.O...

B203 .. 

P

Les&O.

Pierrepont.

, - v 

I. II.

35. 61

25.29

.44

8.19

.55

trace

trace

3.31

11.07 

none

?

trace

1.51

.20

3. 34 3. 30- 3. 37

10. 15 10. Op-10. 31 

.27

99.93 

.11

Nantio Gulf.

I. II.

35.34

30.49

none

8.22

.40

none

trace

2.32

7.76 

trace

. ?

trace

1.76

.15

. 3. HO 3. 5:?- 3. 67

10. 45 10. 30-10. 60 

none

100. 49

Ston

35.56

33.38

none

8.49

.55

?

.04

.53

5.44 

none

none

trace

2.16

.24

3. 63

10.40 

none

100. 42

y Point. Haddam.

I. II. I. II.

34. 95

31. 11

.50

11.87

.57

trace

.09 .81"

4.45 

none

uone

trace

. 2.22

.24

3. 57- 3. 69 3. 62 3. 58- 3. 66

9.92 9.74-10.10 

none

100. 35

99.82

Mr. W. E. Hidden very kindly furnished the Stony Point material. 

For the other specimens I am a debtor to the National Museum.collection. The gravity determinations of the Pierrepont, Stony Point, and 

Nantic Gulf tourmalines were kindly made by Dr. William Halleck.

From the above analyses it is at once apparent that we have three 

types to deal with, lithia, iron, and magnesian tourmalines, respectively, 

with an indefinite number of intermediate products.

For comparison's sake I have tabulated these results, arranging them 

so as best to show how these types graduate from one into the other, 

beginning with the lithia tourmaline and passing thence through the 

iron varieties to those of the purest magnesian type. To render it a 

complete table of tourmaline analyses, so far as such analyses are worth 

considering, the results of Eammelsberg's extensive work are added, 

given in the order and grouping found in his revision of the subject.1 

Also an analysis of an interesting chrome-tourmaline from the Ural, 

by A. Cossa and A. Arzruni;2 the only one of a small number of scattering analyses which seemed to have any value from an analytic standpoint.

1 Ramm. Handb. cl. Miu. Chem., 1875, 538-544 ; Pogg., Ixxx, 449, Ixxxi, 1.

2 Zeit. Kryst. uud Min., vol. 7, 1,
30 WASHINGTON LABORATOEY. [BULL. 55.

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R1GGS.] ANALYSIS AND COMPOSITION OF TOURMALINE. 31

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-i- COf-Hr-tirtcxjiOOSOOC^COOt-OOOOt^Ot^C^lt^^HCOCOCOf CsO-JCiOltO 

w * « * ; ; j ;«5 :

fv? J^ *-» ^_ ^ O5 OO_ CO_ b- OS O C3 O5 O> O5 C> OS -< O O <N rM »H I O OS OS GS_ O CO O

.;...,'..;; ;i! I . g ^ .- ^ ..* . 

i "El 7J i : ! j ='S -S ^ : 3 S § I I : J i S -g B||5 : «-§1-gas^|^-gH||s:a^ g a

^ Su ^3"S'S 1»S2o45<2'^i>,a'clSt-, > grt2 : 3

«^SSoSS-d r^3^cf-&§M b*?S'0 'ara«'S a can.-«cj B ^>^ t2^o r:! ^'"^"" !3 "^ t* c3 a''^'j:l ^^H N ^

rHNcOTj!iritd(>cocS'O-^<NcoT*oec5f^o6c»oi-<c4co^in r-ieaai'Vui
o 0

PHOH

CD 

fu

o 100

;

Localities. i2

 ' 00 

i CO

co oo in

rH L IO

; ;

 

CO 00 t~ 

CO CO I>

: 

i-l O CO 

OC 00 O5

r>l CD o

CO CO Til

O CO tod 06 a

CO CO CO

3? CO 

0 O

0 O)

I. Brazil.................. 2. Chesterfield............ 3. Paris ..................

<3

00

5S 2s

06

tC.1 

i

q s

(? C>

O 

o"; o

m 

CO

CD

COo

in

co- i
JUOUB.] ANALYSIS AND COMPOSITION OF TOURMALINE. 33

Bammelsberg concludes that all tourmalines can be referred to mixtures of the following silicate types: E'6SiO5 , B"3SiO5 , and B///2SiO5 , 

in which E'=H, K, Ha, and Li; R"=Mg, Fe, Ca, and Mil, and E'" = 

Al and B, making boric acid the equivalent of alumina. Be groups 

them in two classes:

I. Magnesian-irou tourmaline, represented by the rather complicated 

formula

and 

II. Lithia tourmaline, represented by

f E'G Si05 ) s E"3Si05 » . ft/// _ B . o A1 111 \ 8 E'"2Si05 f + u { 8 E'"2Si05 J e e ^ " ^ ' 6 Al '

with the following special formuke: E/2E//2Al4B2Si402o for the more 

purely inaguesiau varieties; B^oB'^Al^BcSi^Ofio for the purer iron varieties, and for the lithia tourmaline E'eAli-^SigC^, and other complications i'or those lithia varieties containing iron. The results may 

warrant these deductions; of that we have nothing to say. The important question concerns the chemical constitution of tourmaline. 

Attention has already been called to the weak points in Barnmelsberg's 

analyses; but for the sake of emphasis I refer again to his method of 

determining the water percentages and what depends on it. He assumes that1 the fluorine is driven off quantitatively on ignition, carrying 

with it silicon as the tetra fluoride. This assumption is questionable. A 

half hour's blasting would seem to be sufficient to drive off' the water, 

but it was repeatedly observed that where the tourmaline contained 

fluorine, further blasting, after the water was presumably all off, was 

invariably accompanied by a small loss of but a few hundredths per 

cent. This after loss is probably fluorine in some of its compounds 

with silica, as experiments made it clear that boric acid is not expelled 

by any amount of blasting. While making this correction for fluorine 

the oxidation of the iron is wholly ignored. With this in mind I have 

given loss on ignition in connection both with my own analyses and 

with those by Eammelsberg. Comparing this loss with the direct determinations of water, at the same time noting the amounts of iron 

contained in the respective tourmaline, one is forced to conclude that 

the oxidation of the iron plays an important role here in diminishing 

the loss on ignition by the amount required to convert it into ferric 

oxide. If we were to make the more justifiable correction for the oxidation of the iron, setting aside the fluorine correction, we would have 

more concordant results to deal with results, moreover, which agree 

closely with the direct determinations of water but if the percentages 

representing water are low, those of boric acid, when it is estimated by 

Bull. 55 3
34 WASHINGTON LABORATORY. [BULL. 55.

difference, ought to be correspondingly high, and so they are in a few 

cases. In the greater number of analyses, however, they are unaccountably low, unless we suppose, as I am inclined to do, that the silica 

determinations run high, representing, in some cases, besides the actual silica, more than 1 per cent, of impurities. If all this be true, in 

working out his ratios Eammelsberg found in water and boric acid 

two variables instead of the two constants that they probably are.

It is scarcely necessary to say that certain constituents found in tourmalines are not essential, but have been thrust upon them by their 

associates. The idea that a tourmaline must contain fluorine was long 

ago exploded. Indeed, it had its birth not in facts but in Eammelsberg's assumption that tourmaline contained no water and that the loss 

on ignition was due wholly to fluorine.

Studying those constituents, which are the essentials, in the light of 

their molecular or atomic ratios, we find some very interesting relations. 

The ratios of certain elements are constants in all varieties of tourmaline. Si:B:H:O = l:£:§: 5.2. All the other constituents are variable within rather indefinite limits, and considered individually are 

confusing. If, however, the bases, including hydrogen, be reduced to a 

common, uuivalent basis and be consolidated, the results fall into line 

with the above ratios. This reduction may be made in either one of 

two ways and with almost equally good results. It will be noticed that 

the oxygen ratio is invariably in excess of the amount necessary to the 

silicon and boron, even though we assume both the SiO4 (as we certainly must) and BO2 groups. This small residual is to be disposed 

of. It can be done by assuming the presence of either the A1=O or 

the O=H group. Both hypotheses have been made use of in the following table. E(1) is the univalent equivalent of the bases with the 

oxygen excess incorporated in an A1=O group; E(2) the uuivaleut 

equivalent of the bases on the basis of an assumed 0-H group, The

table is given in full that the extent of the variations, from what seein 

to be simple ratios, may in no wise be concealed, as often happens, in 

giving averages. The hydrogen ratio, though already included in E, 

is given by itself, being one of the constants. For much the same 

reason the alkali ratios are also given, although with them the values 

vary according to the type of the tourmaline. This at least would 

appear to be true for the iron and lithia varieties.

Si : B : RO : K(») : O : H : Alk 

Rumford A ........

Brazil A...........

Auburn A .........

Brazil B...... .....

Auburn B .........

Brazil C ...........

RumfovclB ........

Auburn C .........

1

1

1

1

1

1

1

1

.46

.47

.46

.47

.48

.45

.48

.46

4.48

4.45

4.4*3

4.50

4.48

4.42

4.44

4.50

5.01

5.12

4.83

4.92

4.80

4.93

4.95

4.99

5.18

5.26

5.10

5.17

5.11

5.15

5.20

5.20

.74

.70

.72

.66

.71

.66

.64

.74

.28

.31

.28

.31

.30

.32

.30

.28
UIGGB.] ANALYSIS AND COMPOSITION OF TOURMALINE. 35

Paris.......

Anburn D .. 

Brazil D ....

Had darn. 

Natitic Gnlf 

Stony Point

Pierrepont.. 

Moiiroe..... 

Orford ..... 

Gouverueur 

Hamburgh . 

De Kalb....

Si

1

1

1

1

1 

1

1

1

1

1

1

1

1 :

1 :

: B

.45

.48

.48

.50

.51

.51

.51

.46

.48

.50

.51

.50

.48

; A

: RC) :

4.47

4.50

4.50

4.51

4.52

4.19

4.52

4.43

4.48

4.51

4.50

4. 51

: 4.47

: & .

R(2 )

5.09

5.01

5.02

5.00

5. 00

5.01

4.77

4.89

4.99

4.73

5.08

5.08

: 4. 96

: 5

: 0 :

5.21

5. 21

5.21

5.24

5.25

5.41

5.13

5.12

5.20

5.10

5.30

5. 29

: 5.20

: 5£ :

H :

.70

.70

.68

.69

.68

.68

.63

.69

.68

.68

.59

.66

: .67

: *

Alk

.12

.12

.13

.12

.12

.10

.09

.15

.13

.10

.06

.08

Except in two or three cases the ratios of Si: B : R(1) : O approximate closely 1: £ : £ : 5, the oxygen, in excess of the amount exactly 

represented by the ratio (5), having been absorbed in an A1=O group. 

These ratios give as a general tourmaline formula the simple boroorthosilicate R8BO22SiO4 . The R9 includes the constant H R3 , (Li, Na, 

K) varying between the limits Rj and R2, (Ca, Mg), varying from R0 to 

R3 , Ee varying from R0 to R$, and (Al, A1=O) varying from R4 to R7 . 

On the other hand the ratio Si: B : R(2) : O are about as 1: £: 10 : 5.20, 

which would give-the equally simple general formula R10 BO22SiO4 ,wheii 

R]0 includes the above constant and variables, excepting that OH replaces the A1=O group, and Al accordingly varies between the limits 

Ra and R8 . If we expand, in order to bring out the hydroxyl ratio, we 

have 12SiO4 , 6BO2 , EMHs(OH)3 =Si: B : R : O=l: $:' 5: 5.25. Between 

these two views there are no means at hand of deciding. Could we 

find that the water is not all driven off at the same temperature, or something of the kind, that knowledge would favor the latter assumption.

Experiments to this end are desirable; but whichever postulate we 

make, the following special formulae may be taken as represeutiug typical compounds of the three varieties :

I. Lithia tourmaline 12 SiO2 , 3 B2O3 , 4 H2O, 8 A1aO3 , 2 (NaLi)2O.

II. Iron tourmaline 12 SiO2 , 3 B2O;) , 4 H2O, 7 A1 2O:) , 4 FeO, Xa2 0. 

III. Magnesian tourmaline 12SiO2 ,3B2O3 ,4H2O,5 Al2O3 ,£&MgO,$Na2O.

Calculated. 

B203 . .. -......

Si03 ...... ....

AlaO3 . ........

FeO....:.....

MgO .........

Li 2O .........

Na2O .........

H8O.. ........

I.

.. 11.00

.. 37.70

... 42.75

. . . 1. 57

... 3.21

3. 77

100. 00

II.

10.18

34.89

34.59

13.95

2.90

3 49

100. 00

III.

10.90

37. 38

26. 49

19 31

2.18

3.74

100. 00
36 WASHINGTON LABOEATORYC [BULL. 55.

On comparing the theoretical composition of the above types with 

the results of analysis, they will be found to agree as closely as could 

be expected, at least in the values of the constants. The boric acid 

found invariably falls short of the theory. This is to be expected. 

The analyses do not represent ideal compounds, absolutely free from 

impurities, and the case would be very exceptional in which the impurity tended to raise and not to lower the percentage of boric acid.

In some of the above formulas the group BO2 has been assumed because the oxygen ratio demanded it. As has already been suggested, 

the ease with which the iron oxidizes, and the mysterious manner in 

which this change takes place, under conditions where we would suppose it impossible, perhaps point toward a higher degree of oxidation 

than the more common B2O3. As the result of a slow molecular rearrangement, the one is oxidize'd at the expense of the other. Such a 

change is, I believe, not without its analogies. Certain borates, where 

the assumption of an even higher oxide is thought necessary, on being 

heated, give borates of a lower order.

Notes. The question of color is one of some consequence, particularly 

when the varying colors of the lithia tourmalines are concerned. For, 

while the color of the iron and inaguesian varieties depends on the 

amount of iron present, and ranges from the colorless De Kalb through 

all the shades of brown to the Pierrepont black, the lithia tourmalines, 

containing more or less manganese, give us the red, green, and blue, 

as well as colorless varieties; the shades of color not depending on 

the absolute amount of manganese present, but rather on the ratios existing between that element and iron. When the ratios of Mn : Fe = 

1: 1 we have the colorless, pinkish, or very pale green tourmaline. An 

excess of manganese produces the red varieties. If, on the other hand, 

the iron be in excess, the result is the various shades of green and blue. 

When a section of tourmaline shows a red center bordered by green, 

the two colors are usually separated by a narrow belt of nearly colorless material, in which the iron and the manganese are presumably in 

equilibrium.

As regards fusibility; the lithia tourmalines which are free from 

both iron and magnesia are infusible. The presence of either or both 

of these elements brings with it a degree of fusibility increasing with 

their increase, till we find that the. purest tourmalines, both iron and 

rnagnesian, fuse with great ease. , The titanic oxide associated with the Hamburgh and De Kalb tourmalines attracted special attention because of its form. Having been examined chemically it was kindly studied microscopically by Mr. J. S. 

Diller, who observed as follows :

The small iron black scales with a rather brilliant metallic luster are cleavable into 

very thin foli;e, the thinnest of which, under the microscope, are perfectly opaque. 

In reflected light these lamellae show three systems of cleavage planes, traces of which,
KIGGS,] ANALYSIS AND COMPOSITION OP TOURMALINE. 37

upon the plane of foliation, intersect at an angle of 60°. The cleavage planes make 

a large angle with the plane of foliation, and it is evident that this mineral, is rhombohedral in crystallization. It is infusible on very thin edges, and does not become 

magnetic when heated. By this means it is distinguished from hematite and;lmeuite. 

From its physical properties alone I should conclude that it is a member of the ilmeuite 

series rich in oxide of titanium. As analysis shows it to be essentially titanic oxide, 

it becomes of special interest. In the first place it is the extreme member of the 

ilmenite series, and in the second place it is a new form of titanic oxide, which is 

thus shown to be tetramorphic. 
NOTES ON CERTAIN RARE COPPER MINERALS FROM UTAH.'

BY W. F. HlLLEBRAND AND H. S. WASHINGTON.

Some time since analyses and partial descriptions of several rare 

copper minerals from tbe American Eagle Mine, Tintic district, Utah, 

were published2 by one of us. These minerals had been found by Mr. 

Eichard Pearce in ore shipments from that mine to the Boston and 

Colorado Smelting Works, near Denver, Colo. Later, in shipments 

from the neighboring Mammoth Mine, in the same district, Mr. Pearce 

discovered a second series of minerals of similar character, most of the 

species, however, being distinct from those of the former, occurrence. 

In recent papers 3 he has given the results of his examinations and 

enumerated the following species: Bnargite, olivenite, conichalcite, 

cliuoclasite, brochantite, pharmacosiderite, tyrolite (U), eriuite, chalcophyllite, malachite, azurite, and one or two others of doubtful identity, 

of most of which " enargite is the mother mineral."

In order that this interesting series, in part new to America, might 

receive fuller study than he was able to devote to it, Mr. Pearce, with 

the assistance of Mr. Whitman Cross, selected a set of specimens for 

examination in the laboratory of the Geological Survey at Washington. 

The chemical work of this paper was there carried out by one of us,4 

while the crystallographical and optical study was undertaken by the 

other, 5 at New Haven, under the guidance of Prof. E. S. Dana. The 

results of our work, both chemical and physical, failed to meet some of 

the hopes induced by a first view of the material at disposal, although 

this was the best that could be found. They are of sufficient interest, 

however, to make public, especially in view of the meager state of our 

knowledge regarding a majority of the species herein mentioned.

1 Eead before the Colorado Scientific Society January 2,1888, and published in the 

Am. Journ. Sci., 3d series, vol. 35, 18rt8, p. 298.

2 Proc. Colorado Sci. Soc., vol 1, p. 112, and Bull. U. S. Geol. Survey, No. 20, p. 83. 

3 Proc. Colorado Sci Soc., vol. 2, pp. 134, 150. 

4 \V. F. Hillebraud. 

6 H. S. Washington. 

38
AND 

WASHINGTON.]

OLIVENITE.

This mineral occurred well crystallized. Its habit is tabular, parallel 

to a (100), and the crystals are, as usual, very simple, as shown in the 

figure. The planes & (010) and v (101) as a rule 

are either absent or very small. Measurements 

were made for the purpose of obtaining a more 

exact axial ratio than we have at present, the old 

values of Phillips dating back to 1823.

Upon examination and measurement with a 

Fuess horizontal goniometer, it was found that 

e/\6 (Oil A Oil) was the only angle sufficiently 

accurate for the purpose, a and m being a little TIG. i. crystalline form of 

rough and uneven. The angle mentioned fur- oiivcmto. 

liished a good value for c, but to obtain the value for « use had to be 

made of a specimen of oliveuite from the American Eagle Mine. 1 This 

oliveuite was acicular in habit, the prism m (110) predominating. From 

these crystals good measurements were obtained of m/\ m'" (110/\ 110), 

and a satisfactory axial ratio was deduced. . The measured angles are 

as follows :

e/\t, Oil A Oil = 67° 51' 

m/\m"', 110 A 110 = 86° 26'

From these angles we obtain the following axial ratio: 

a: b: c = 0.93961: 1 : 0.672606

The measurements above differ considerably from the fundamental 

angles of Phillips, which are

e/\6, Oil A Oil = 690 i(y 

and

m A w'", 110 A HO = 87° 30',

giving the axial ratio

a : I : c = 0.9573 : 1 : 0.6894.

Measurements were made with the view of determining whether the 

species is really orthorhombic or not. The following are the angles 

obtained :

a/\e, 100 A011 =89° 4', d/\e, 100X011 = 89059' 

a/\6,

It is seen that the front angles are in each case a trifle less than the 

rear angles; but not much reliance can be placed on these results, owing to the poor surface of both a (100) and ^(100).

1 No. 5684 in the Yalo collection.
40 WASHINGTON LABORATORY. |Bum55.

Under the microscope the tabular crystals showed parallel extinction 

and a slight pleochroism, the vibrations || c being pale olive green, while 

those || lj were of a brownish yellow, with the absorption b>c.

The mineral was not analyzed, because of the small quantity available, and because its identity was otherwise clearly established.

ERINITE.

Erinite occurs as a dark green crystalline lining of cavities, associated 

with and generally upon enargite, azurite, barite, or clinoclasite. Crystals of olivenite are frequently scattered over its surface, which shows 

often a somewhat satiny sheen due to minute crystal facets. Hardness 

4.5, sp. gr. undetermined. Because of its intimate association with 

azurite and olivenite it was very difficult to obtain pure material for 

analysis. Sample I contained 3.90 per cent, of insoluble matter, not 

included in the analysis. Sample II was composed of a small lot of 

vitreous crusts, the only ones of the kind observed, which had been 

collected before shipment of the specimens, and were thought to be 

erinite by Mr. Pearce, whose partial analyses of material similar to 

sample I are added for comparison under III.

i. IT. in. .

Hillebrand. Pearce.

CuO.......................... 57.67' 57.51 56.56 57.43

ZnO.......................... 1.06 0.59

CaO........................... 0.32 0.51 0.43

MgO........................... trace trace

As2 05 ......................... 33.53 31.91 32.07 32.54

PaO6 .......................... 0.10

H2O .......................... 7.22 9.15 6.86 7.67

Fe203 -........................ 0.14 0.20 0.85

S03 ........................... trace.

100.04 99.87 96.77 97.64

Analyses I and II, and presumably those of'Pearce, show the composition of air-dried powder. Sample I lost 0.67 per cent. H2O over 

sulphuric acid and a total of 0.78 per cent, at 100° C. At 280° C. the 

total loss was 1.14 per cent., leaving 6.08 per cent, firmly combined. 

Sample II lost 2.06 per cent, over sulphuric acid and a total of 3.22 per 

cent, at 280° 0., leaving 5.93 per cent, firmly combined. The molecular 

ratios, including all the water, are:

CuO (CaO,ZnO). As206 (Pa05 ). H2 0.

I...................... 5.08 : 1.00 : 2.74

II..................... 5.34 : 1.00 : 3.66

III (mean) ............ 5.13 : 1.00 : 2.87

If the weakly combined water be excluded from both I and II, the 

ratio is brought considerably nearer to that derived from Turner's ap1 Mean of 57.61 and 57.74.
IIII.LRBRAM) AND ' rrvl?nT rm-p A 1 

WASHINGTON.] TYKOLllJi,. 4 L

proxiniative analysis, 1 i. e., 5 :1: 2. It is uncertain whether Turner's 

sample was air-dried or heated to 100° C.

TYROLITE (?).

Kegarding the identity of this species some doubt exists, as the analytical results obtained do not agree with those given by von Kobell 2 

and Church.3 In general appearance it seems to resemble tyrolite. It 

occurs in thin scales on quartz, but more often in radiating scaly 

masses, somewhat like the pyrophyllite from Graves Mountain, Georgia. 

It has a bright apple-green color, sometimes with a tinge of blue; a 

somewhat pearly luster; a hardness of 2.5 (1.5 to 2 for tyrolite in the 

text books), and perfect cleavage. Under the microscope it showed 

little or no pleochroism, and extinction parallel and perpendicular to 

the radial line, In convergent light the cleavage flake showed the 

ordinary biaxial figure with the dispersion p >v. Its double refraction 

is negative, the acute bisectrix being perpendicular to the cleavage face 

and coinciding with the crystallographic c. The obtuse bisectrix lies 

parallel to the radial direction of the crystal,'but whether it corresponds with a or B can not be determined. It was unfortunate that a 

crystallographic investigation was impossible, as our knowledge of 

tyrolite in this respect is of the most meager description.

On heating it flies into fine fragments, which by gentle tapping of 

the tube collect into spongy masses. The mineral melts in the flame of 

a Bunseii burner. The sp. gr. of sample I (containing 2.25 per cent, of 

insoluble gangue) was 3.27 at 20£° C. From sample II, which was the 

purest and best crystallized to be found, 1.25 per cent, of gangue has 

been deducted.

i. n.

Hillebrand.

	Mean. 

CuO....... 45.20 45.23 45:22 46.38 42.60

ZnO....... ...... 0.04 0.04 trace 0.97 (Fe2O3 ,

CaO....... 6.86 6.82 6.84 6.69 9.10

MgO ...... 0.05 ........ 0.05 0.04 ........

A820B .--~. 28.84 28.73 28.78 26.22 27.87

PaGe-...--. trace ........ trace trace ........

H2 0 ....... 17.26 ........ 17.26 17.57 16.23

S03 ........ (?) (?) (?) 2.27 2.45

98.21 98.19 99.17 99.22

SO3 was unfortunately not tested for in I. It may, however, reasonably be assumed to be present in about the same amount as in II, and

1 Eclinb. Jotirn. Sci., vol. 9,1S28, p. 95, and Phil. Mag., vol. 4,1828, p. 154.

2 Pogg. Ann., vol. 18;p. 253.

3 Jonrn. Chein. Soc., 2d series, vol. 11, p. 108.
42 WASHINGTON LABORATORY. [BULL. 55.

if it be considered to be present as gypsum (CaS04 , 2H2O) the following molecular ratios are obtained:

CuO(CaO). As206 . H20.

I................... 5.00 : 0.94 : 6.80, or 11 : 2.07 : 14.96

II................... 5.00 : 0.84 : 6.81, or 11 : 1.85 : 14.98

III................... 5.00 : 0.90 : 6.29, or 11 : 1.98 : 13.84

It appears herefrom that the As2O5 is somewhat less and the H2O much 

less than required to satisfy the formula 5CuO, As2O5 , 9H2O, derived 

from vou Kobell's (1. c.) analysis, on the supposition that the CaCO3 found 

by him, and later by Frerizel 1 and church (1. c.), is not an essential 

cous'.ituent of tyrolite.

It is improbable that more than a very small quantity of chalcophyllite, if any, was mixed with the material analyzed under I and II, although 

both appeared on some of the specimens marked tyrolite received from 

Mr. Pearce, and are not always easily distinguished. In any mixture of 

tyrolite and chalcophyllite the water found must exceed its percentage 

in the former mineral. This is here not the case, whence it is to be inferred either that the present mineral is not tyrolite or that the older 

analyses do not represent its true composition.

A large portion of the water is very loosely combined. Of that in 

analysis I, 4.69 per cent, escaped at 100° C., the most of it over sulphuric 

acid; and in analysis II, 4.15 per cent, was removed by sulphuric acid, 

and, further, 0.91 per cent, escaped at 100° C., making a total of S.OGper 

cent. These amounts, subtracted from the total percentage found, leave 

12.57 and 12.51 per cent., respectively, or about five molecules (assuming 

five molecules CuO(CaO)). At 280° <J. the loss on sample II was 10.34 

per cent., in which is presumably included the water of the gypsum supposed to be present, leaving three molecules firmly combined.

Church (1. c.) likewise noticed a great Toss of water in vacuo and at 

100° C., but assumed that it was hygroscopic water included between 

the plates of the mineral. The second of his analyses, with data for calculating the centesimal composition, is as follows:

CuO.......................... 50.06

AsaO6 ......................... 29.29

H20 .......................... [8.73]

CaC03 ........................ 11.92

100. 00

Substance..................... 0.4585

HoOin vacuo ................. 0.024

H3 0 at 100°................... 0.011

CaCO3 ........................ 0.0505

CuO .......................... 0.212

Mg2P2 07 ...................... 0.205

Whence he deduces the formula 50uO, As2O5 , 4H2O. Assuming that 

Mg2P2O7 is an error for Mg2 As2O7, or for As2S3 , in which latter form it 

appears that arsenic was usually estimated by him in minerals of a similar character, it is impossible to deduce th,e above given percentage for 

As2O5. But considering the latter correct, and including the water lost 

in vacuo and at 100°, the composition is:

1 Naumann-Zirkel, Elemente der Mineralogie, p. 540.
IMI.I.KHKAXn AND 

WASHINGTON.] CHALCOPHILL1TE. 43

CuO..........:............................................. 46.24

Asa06 ....................................................... 27.05

H20 ......................................:.........-........ 15.70

CaCOa...................................................... 11.01

100. 00

which furnishes the molecular ratio CuO: As2O5 : H2O as 5.00:1.01: 7.43; 

not greatly differing from those derived from analyses I and II, above.

CHALOOPHYLLITE.

This mineral occurs in the form of small hexagonal plates arranged 

in rosettes, differing from the radial arrangement of the supposed tyrolite. It showed the same bright apple-green color, pearly luster, and 

perfect basal cleavage. An optical examination showed it to be uniaxial, with negative double refraction.

These crystals showed several planes replacing the edges, and measurements were made of them as far as possible. The angles did not 

agree very closely, owing to the imperfection of all the surfaces, but 

they were sufficiently exact to prove the presence of r (lOll, R), e 

(0112, -£ E), and two other rhornbohedrons new to the species, having 

the symbols w (1016,-iE) and d (0113,4- B).

The figure shows the habit of the crystals; 

but with d absent, this plane being only observed in one instance. The very rough angles 

obtained are given below: FIG. 2.-cry8taiiino form of

clialcophyllite. 

Observed. Calculated.

cAr, 0001 A 1011 = 71° 27' 71° 16'

CAW, 0001 A0016 = 26° 10' 26° 10' 20"

CA e, 0001 A 0112 = 56° 51' 55° 51' 10"

cAd, 0001 A0113 = 41° 50' 44°30'30';

The above angles are the means of several measurements, which vary 

among themselves from one to three degrees. The fair agreement in 

the first two results therefore is merely accidental, and no value can.be 

attached to these measurements, which are inserted because the measurements of this species are extremely few.

The mineral was not analyzed, for want of sufficient material. On 

heating it decrepitated as violently as the last-mentioned mineral, and 

in the flame of the burner fused, though not with the same-readiness.

CLINOCLASITE.

The clinoclasite occurs in two distinct habits one distinctly crystallized and the other in barrel-shaped or globular 

forms. It is of a dark bluish green color, almost 

black by reflected light, 

bright green by trans- __ 

mitted light. Streak and ,,, ,,,.. -

0 PIG. 4. Crystalline form of

powder bluish green. Sp. ciinociasite. 

gr. at 19° C. 4.38 (4.36 Pearce). Hardness, 2.5 to 3.

FIG. 3. Crystalline form of 

clinoclasite. .
44 . WASHINGTON LABORATORY. [BULL. 55.

At first sight these crystals seemed to be very promising and likely 

to afford good measurements for the species. But on further examination they did not come up to our expectations, c (001) and « (302) being 

the only two faces giving even fairly good measurements, m (110). 

r (101), t (111), andj? (113), the other planes observed, were all dull or 

rounded, and only capable of giving angles accurate enough to identify the forms. Of the planes above, t and^> are new to the species. 

Most of the crystals were apparently made up of two or more individuals in nearly parallel position, but inclined slightly in the zone c/b. 

A measurement in one case gave the angle 

4° 10', but as it is not the result of twinning, 

this angle of course is not constant, and only 

shows the very slight inclination of the indiFIG. 5.-CryBtaiiine form of vidual crystals. A consequence of this method

ciinuciasite. Of growth will be described later. 

The crystals were all simple, the form in Fig. 3, or a combination of 

that with r being the most usual. Occasionally the lower half of in is 

replaced by £, as shown in Fig. 4, giving the angle 13° 20' (calculated 

13° 17') for m/\ t. The new plane p (Il3) was observed in several crystals and is shown in Fig. 5. 

The following angles were obtained for it:

Observed. Calculated.

c A#, 001 A I13=61° 6' 61° 26' 30"

«Ai>i 302 A ll3=50° 14' 51° 19' 10"

1 , 113 A 113=82° 85° 48'

The angles are merely approximate, but sufficient to establish the 

form. The crystals are for the most part elongated in the direction of 

the b axis, with a length of from 2 to 3 millimeters, and show easy

cleavage parallel to c.

The other type of clinoclasite is interesting as showing the consequence of the nearly parallel growth of the crystals mentioned above. 

In some of the specimens the crystals are grouped about the I axis, with 

c exposed. They are inclined a trifle in the zone c/b and also in the 

zone a/b, thus rounding off the group in two directions, but decidedly 

more in the latter zone, forming, with the elongation in the direction of 

&, distinctly barrel-shaped forms. Occasionally the curvature in the 

zone c/b is carried still further, producing globular forms. In all cases 

c forms the outer surface arid the crystals are closely crowded together, 

producing a bright and coarsely rough surface.

The material analyzed consisted of the globular masses mentioned 

above, and was probably not as pure as the crystals and barrel-shaped 

forms. A trifling amount of insoluble matter (0.05 per cent.) has been 

deducted. For comparison, Mr. Pearce's partial analyses are also 

quoted.
HILLKHKANI) AND 

WASHINGTON.] M1X1TE. 45

CuO....

ZnO....

AssOs-...

p.2 o5 -...

11,0 .....

Fe303 ....

8iOs .....

a 

.... 62,34

.... 0.06

.... 29.59

.... 0.05

.... 7.73

.... 0.12

. . . . 0. 06

I. 

Hillebrand.

. b 

62. 54

0.04

29.60

0.05*

7.72

0.12

0.06*

Mean.

62. 44 

0.05

29.59 

0.05 

7.72 

0.12 

0.06

II.

Pearee.

. a b 

61.68 61.22

Theoretical 

composition.

62. 65

29.36 28.85 30.25

7.31 7.27 7.10

99.95 100.13 100.03 98.35 97.34 100.00

* Assumed the same as in a.

These results reveal nothing worthy of remark, except that the water, 

as in most earlier analyses, is found uniformly higher than that required 

by the formula 60uO, As2O5 , 3H2U, or Cu3 [AsO4f+3Cu [OH]2.

MIXITE (?),

On some specimens of ore, but apparently not in close association 

with the other minerals mentioned, was a mineral occurring in delicate 

tufts of silky needles of a whitish to pale greenish color, as described 

by Mr. Pearee.1

It was impossible to procure enough of the needles free from an underlying non-crystallized greenish coating of cavities for a satisfactory 

analysis. A good deal of the latter was necessarily included in the 

sample tested, but qualitative tests showed that both needles and coatings contained the same constituents. It is hardly to be doubted that 

both have the same centesimal composition.

CuO...................43.89

ZnO.................. 2.79

CaO.-................ 0.26

Bi 2 0..,-.................11.14

As2 06 .................27.78

PiO5 .................. 0.06

H2O ...................11.04

SiO,.................. 0.36

I.

Hillebrand.

... .-A-,

6

43.88

2.62

0.26

11.22

28.79

11.04

0.48

Fe2 03 . 0.97

Mean.

43.89 

2.70 

0.26

11.18

28.79t 

0.06

11.04 

0.42 

0.97

II.

Pearee.

50.50

3.19

27.50

12.55

98.29 99.31 93.74 

t The higher value was undoubtedly nearer the truth than the lower.

That an error as to the CuO occurs in Pearce's analysis is beyond 

question. The above results agree fairly well with Schrauf's analysis 

of mixite,2 which contained 43.21 CuO, 13.07 Bi 3O3 , 30.45 As2O5 , and 

11.07 B2O, besides a little CaO and FeU; but the form of this mineral 

was given by Schrauf differs from that of the present one, and its colors 

given as emerald to bluish green. Schrauf's number for the specific

'Proc. Colorado Sci. Soc., vol. 2, p. 151, under the title "New Mineral." 

3 Zeit. f. Kryst., vol. 4, p. 277.
46 WASHINGTON LABORATORY. (BULL. 55.

gravity (2.66) is unquestionably much too low. That of the material 

now analyzed was 3.79 at 23£° C. When treated with dilute nitric acid 

it becomes at once covered with the brilliant white coating of bismuth 

arseniate, so characteristic of mixite. The latter mineral is stated to 

belong to the inonoclinic or the triclinic system, while the observations 

of Mr. Whitman Cross would indicate that the present one can belong 

to neither of those systems. He says: 1 k 'The needles are very slender, 

with a length of more than lmm in some cases, by a thickness of. less 

than 0.05mm. They are deeply striated vertically, and the crystal system could not be determined, although the extinction in polarized light 

makes reference to the tetragonal, the hexagonal, or the rhombic system necessary. The index of refraction is high. Pleochroism distinct, 

the colors observed being for the thicker crystals, a (and b) sea green, 

c sky blue."

PHARMACOSIDERITE.

For want of sufficient material no analyses were made.

BROCHANTITE.

This hydrous sulphate of copper occurs in two distinct 

types in the specimens examined. The first, or ordinary 

brochantite, is of a prismatic habit, as is shown in Fig. 6. 

The crystals are dark green and transparent, but do not 

give good measurements, owing to the imperfection of the 

surface. The cleavage parallel to b (010) is perfect. The 

measured angle of m /\ b (110 A 010)=51° 46' is only approximate, and differs considerably from Miller, who 

gives 52° 5', and Schrauf, who gives 52°. 

The second type is like Waringtouite from Cornwall, described by

Maskelyne.2 This variety was suspected by

Mr. Pearce (loc. cit., p. 135). It is of a light

green color, and has a curved double-wedgeshaped habit. The forms observed are-shown

in Figs. 7 and 8. The crystals were poor for

measuring, all the planes, with the exception

of b, being curved to a great degree. The crystals were none of them 

more than two or three millimeters long, with the 

relative proportions of the figures. They were 

implanted by b. m, in Fig. 8, was identified with 

certainty; the angle for b/\m being 52° approxirnatety. The plane lettered ft was very much 

curved in all cases, and its symbol, consequently, 

is not known with exactness. It corresponds in 

its angles, very roughly, it is true, to the 7c, 12.1. 4

FIG. 6. Crystalline form of 

brochanlite.

FIG. 7. Crystalline form of 

brochantite.

FIG. 8. Crystalline form of 

brochantite.

1 Proc. Colorado Sci. Soc., vol. 2, p. 153.

2 Cheui.News, vol. 10, p. 263, 1864, and Phil. Mag., ser. 4, vol. 29. p. 475,
HILl.EnUAND WASHINGTON.] AND TJPnr'W A TMTTTF A.1 BKOCHANTITE. 4<

of Schrauf, some of the angles obtained from these crystals and the 

corresponding ones of Schrauf's Waringtonite being given here:

Washington. Schrauf. 

& A fc, 010 A 12.1.4 = 80°-82° 86° 43' 

TOA&, HO A 12.1.4 = 45° 43° 11' 

. fc A fc', 12.1.4 A 12.1.4 = 75°-80°

In most of the crystals of this type & \vas undulating parallel to c.

Want of material forbade an analysis of this mineral, but blow-pipe 

tests and the crystallographic examination establish its identity beyond 

doubt.
MINERALOGICAL NOTES.i

By W. F. HlLLEBBAND.

Although the results of analysis of the herein-mentioned minerals, 

unsupported as they are, with one exception, by any crystallographic evidence, lead to complete identification of the species only in one case, they 

are deemed of sufficient importance to place on record, together with 

such information regarding their physical properties as could be gathered from the material at hand, which was in some cases rather scanty.

A few years ago in granitic debris on Devil's Head Mountain, 

Douglas County, Colo., in the Pike's Peak region, Mr. W. B. Smith 

found a number of minerals which appeared worthy of examination. 

.Two of these, allanite and gadolinite, have already been analyzed by 

Mr. L. G. Eakius.2 The following analyses, I-VI, represent the composition of the others, of which all but No. Ill were made in the laboratory of the U. S. Geological Survey, in Denver, over two years ago.

1. SAMARSKITE ? .

The mineral first to be mentioned occurred in fragments of all sizes 

up to that of a chestnut, without any evidence of crystal form except 

on a small portion of one piece, where a structure resembling that shown 

in Fig. 9 was apparent. The color was pitch black, with brilliant vitreous luster, but pale brown in thin splinters; streak 

dirty brown. The pieces were very brittle, and 

when heated flew into fine, sharp fragments. Fracture subconchoidal. These characteristics agree very, 

closely with those given by J. Lawrence Smith 3 

for the purest North Carolina samarskite, but the 

density is much greater, being 6.18 at 22° C. for I, 

Fio.9.-IsLnawkite (?). as rai£nt be expected from the percentage of Ta2O5, 

which is much higher than that as yet found in any 

recognized samarskite. Hardness, 5.5 to 6. Slight solubility in HC1 

was shown on prolonged boiling, and a somewhat greater in H2SO4. 

Before the blow-pipe a splinter became dull, but did not fuse. Analysis 

I shows the composition.

A single piece of but a few grammes weight, while in its general behavior and appearance resembling those just described, presented two 

points of difference. The streak was salmon colored, and the rather 

thin piece was bounded on two opposed sides by flat surfaces, which

1 Eead in part before the Colorado Scientific Society, March 5, 1888. 

3 Proc. Colorado Sci. Soc., vol. 2, p. 32.

3 Am. Jour. Sci., 3d series, vol. 13, 1877, p. 359; Ann. Chini., vol. 12, 1877, p. 253; 

Original Researches in Mineralogy and Chemistry, p. 197. 

48
Hll/LEBKAND.J MINERALOGICAL NOTES. 49

might possibly be the result of cleavage. These observed differences 

led to analysis II. The density at 25° C. was 6.12, and the hardness 5.5. 

As the analysis reveals a remarkable agreement in composition with 

the first-described specimens, there is no reason to suspect the presence 

of distinct species.

Analysis III gives the composition of the specimen shown in Fig. 9, 

which it was thought might be an altered state of the ah,ove-described 

mineral. It was evidently in an advanced stage of alteration, being 

very easily broken, and so much stained (brown) that scarcely any evidence of its original color and luster could be observed, though what 

little of these features remained indicated agreement with those above 

mentioned. As some water escaped at 100° C., and still more for each 

further slight increase in temperature, air-dried material was taken for 

the analysis. This shows in most respects so close an agreement with 

I and II, that the assumption of original identity with the brilliant black 

mineral does not seem far-fetched. The chief differences lie in the much 

lower percentage of Ta205 in III, and the presence of U03 instead of U02. 

The density at 16° C. was 5.45.

Analyses of samarskile.

Ta206 .......

Cb206 . ......

W03 ........

SnOs........

ZrO2 ........

UOZ . .......

Th02 . .......

Ce203 ......

(Di, La)2O3 .. 

Er203 .......

Y203 .:....-.

Fe203 .......

FeO.........

MnO. .......

ZnO ...... ..

PbO...... ..

CaO.. ......

MgO ........

KaO. ........

(Na,Li)sO.. 

HsO. ........

Fl ...... ....

T.

27. 03

27. 77

2.25

0. 95

*2. 29

4.02

3.64

0.54

1.80 

tlO.71

t6.41

8.77

o v>

0.78

0.05

0.72

0 07

0.17

0.24

1.58

?

100. 31

II.

28.11

26.16

2.08

1.09

*2.60

4.22

3.60

0.49

2.12

no. 70

t5.96

8.72

0.35

0.75

0.07

0.80

0.33

0. 13

0.17 

1.30

f

99. 75

III.

19.34

27.56

5.51

0.82

3. 10 (with TiO2 )

6. 20 (UO3 )

3.19

0.41

1.44

t9.82

15.64

8.90

0. 39 (or 0.74 UO2 )

Jo. 77

1.07

1.61

0.11

J 0. 3(5 

3. 94

?

100. 18

"Probably containing some TiOj.

t Calculated from the molecular weight of the mixed oxides of this group on the 

unsupported assumption that only Er3O3 and Y2O3 were present. The molecular 

weight in the case of I was 304.9 ; iu that of II, 307.7. 

Bull. 55 4
50 WASHINGTON LABORATORY. [BULL. 55.

The method of analysis followed was, with certain modifications, that 

devised by J. Lawrence Smith.1 Two instead of five grammes of material were taken for greater convenience in manipulation.

A few remarks in regard to certain points in the course of analysis 

may prove of service to those having similar analyses to make. By the 

method of Smith the constituents of the mineral are divided at once 

into two portions, those soluble in HF1 and those insoluble. The former 

portion includes Ta, Cb, Sn, W, U (if present as TJO3), Fe,2 Ti, Zr in 

part, Zn, Mn, Mg, K, and Na, while the latter contains the earths of the 

cerium and yttrium groups, Th, U (if present as UO2), part of the Zr 

when other earths are present, a small part of the Fe, and the Pb and 

Ca.

It was found, after converting the insoluble fluorides into sulphates 

and dissolving in water,, that a white insoluble residue remained, which, 

according to Smith in the case of samarskite, should be Cb2O5 and 

Ta2O5 . Neither of these could be found in it, however, the whole being 

lead sulphate. After filtering, the remainder of the lead was thrown 

down by H2S. The uranium then having been oxidized by nitric acid, 

the earths (except ZrO2 and some CaO) were thrown down by oxalic 

acid (not ammonium oxalate) in excess. The use of oxalic acid was 

rendered necessary by the observed solubility of the earths of the 

yttrium group in ammonium oxalate. These when freed from bases of 

the cerium group were not precipitated by this reagent, or, more properly, the precipitate at first formed dissolved completely in excess of the 

precipitant on very gentle warming and was not again precipitated on 

cooling. This behavior indicates the presence of erbium in quantity, 

which may influence the yttrium present, for the latter by itself is stated 

to be only partially soluble in concentrated boiling ammonium oxalate 

and to be again thrown out on cooling. It should be remarked, however, that the solubility above mentioned was very much greater than

when to a hot solution of erbium and yttrium sulphates, 3 prepared 

according to the data furnished by the above analyses, ammonium oxalate was added in excess.

The filtrate from the insoluble fluorides was evaporated to dryness, 

dissolved in water and a few drops of HF1, and the tin was thrown 

down by H2S, as done by Marignac.4 The filtrate was then evaporated 

with large excess of H2SO4, heated till all HF1 was certainly removed j

'Am. Chem. Journ., vol. 5, pp. 44, 73; Chern. News, vol. 48, pp. 13, 29; Original 

Researches in Mineralogy and Chemistry, p. 350.

3 Treatment with HF1 at once reveals whether the iron is present as admixed 

hematite or limonite (as in analysis III, where it remained suspended in the liquid iu 

an extremely fine state of division), or is chemically combined with the acids of the 

mineral. In the first case it resists the solvent action of HF1 for some time after the 

tantalates and columbates are thoroughly decomposed.

3 From T. Schuchhardt. Though marked chew, pure, it is not at all probable that 

they were so.

4 Ann. Ch. Phys., 4th series, vol. 13, p. 5.
HILLKBBAHD.] MINERALOGICAL NOTES. 51

then, without driving off the excess of H2SO4 , diluted and boiled (stirring corrstantly to prevent bumping) in a very large platinum dish for 

ten or fifteen minutes. The precipitate collected on a filter was then 

dissolved in HF1, the filtrate evaporated with excess of H2SO4 and 

treated in every way as above described till after the third precipitation by boiling. The combined filtrates were then evaporated, most of 

the H2 SO4 was driven off, the residue taken up with water and boiled 

for some time. The remainder of the metallic acids, except some TiO2 

if present, is now entirely precipitated, but to free altogether from ZrO2 , 

Fe2O3 , and from most of the TiO2 the precipitate was again dissolved 

in HF1, the filtrate was evaporated with H2SO4 , the excess of the latter 

partly driven off, and the acids were again thrown down by boiling.

This process is somewhat tedious, but seemed to possess the advantage of entirely separating Ta, Cb, and W from Fe and Zr and in great 

measure from Ti, unless the latter is present in quantity. The point to 

be observed is that the first precipitations shall- be made in strongly 

acid solutions, the latter in solutions less strong. The procedure of 

Smith driving off nearly all H2SO4 at first and then boiling with 

HC1 is objectionable; the metallic acids become strongly caked during 

removal of the H 2SO4 and retain much iron, which no amount of boiling 

with HC1 can remove. The further treatment of the combined filtrates 

requires no special mention. .

For the separation of WO3 the ignited and weighed oxides were 

fused with ;N"a2CO3 and S and separated as recommended by .Rose. The 

method, however, leaves much to be desired, for a considerable quantity 

of the R2O5 acids goes into solution with the W. Cb2 ()s, and Ta2O5 were 

separated by Marignac's method.

FeO was estimated by titration with KMnO4 after solution of the 

very finely powdered mineral in H2SO4 by heating for two or three 

days in sealed tubes, a blank experiment being made with H2SO4 alone 

in another tube. The excess of KMnO4 above that required for the 

conversion of all uranium (when assumed present as UO2 ) to UO3 was 

considered to be equivalent to the FeO. The accuracy of the determination is of course not affected by the fact that uranous salts reduce 

ferric salts in solution.

Fluorine could not be found quantitatively, but from the slightly acid 

reaction of the water evolved on heating the mineral, its presence is rendered probable.

From the two first analyses it is impossible to identify the mineral 

with any known species beyond doubt, although it appears to be more 

nearly allied to samarskite than to any other. The presence of the iron 

as Fe2O3 distinguishes it from most other tantalates and columbates 

containing much iron. That the greater part of the iron exists in the 

ferric condition is certain, for if the uranium existed as UO3 instead of 

UO2, as assumed, the amount of KMn04 required to oxidize 4.02 per 

cent, of UO2 (anal. I) would indicate but 2.13 per cent, of FeO.
52 WASHINGTON LABORATORY. [BULL. 55.

2. AN ILL-DEFINED ZIRCONIUM MINERAL.

» With the mineral just described occurred peculiar growths, from an 

inch to an inch and three-quarters in length, of a pale brown color, and 

having the forms shown in Figs. 10 and 11, of which analyses IV-VI represent the composition. Evidences of crystal faces were 

observed on the upper terminations of some specimens. It 

seemed not at all probable from its appearance that the substance was homogeneous, and a thin section showed plainly a 

mixture of two or more minerals. One of these is probably 

limonite, and the action of HF1 supports this view; for, 

while the powder as a whole was instantly decomposed, brown 

oxide of iron remained for some time suspended in the liquid. 

The specimen represented by analysis VI differed much in 

appearance in places from the others, fractured surfaces being coarsely 

granular, and showing clear reddish grains of some size which could 

easily be detached. The sp. grs. were 3.70 (IV), 3.60 

(V), 3.64 (VI). The analyses give the composition of 

air-dried material, for it was found that at 100° C. and 

with each further increase in temperature water was 

lost. They are only of value as showing the composition 

of these characteristic forms, which are mixtures of 

riG.n.-crytoiite(?). perjj apS cyrtolite, or some allied alteration product of 

zircon, with limonite and a phosphate.

Analyses.

Fm.lO. Cyrtolite (?).

Ta3 05 ..... 

SnOs......

Zr02 ......

Si02 ......

Th02 ......

Ce2 03 ..... 

(Di,La)203 . 

Er2 03 ..... 

Y203 ......

Fe203 .....

MnO......

CaO. ......

MgO ......

K2 0.......

Na3O......

H2 0. ......

pao« ......

Fl. ........

IV.

)

47 QQ

20.06

1.16

0.06 

0.19 

4.77 

2 27

5.53 

0.47

1 net

0.13

0.20

0.46

12.87

1.64

0 25

100. 04

V.

f 0.71 

J 0.03

L47. 81

20 fi4

> 1.20

4.76

2.48

5.97 

0.57

1.93

0.11

0.10

0.50

12.00

1.75

0.42

100. 98

VI.

Ul.OO

1Q 21

0.60

4.55 

3.13

4.86 

0.33

2.15

0.17

0.42

12 <I7

0 93

0.42

100.74
HILT,EBRAND.] MINERALOGICAL NOTES. 53

3. WHITE. BERYL.

The crystals analyzed were from a specimen in the National Museum 

found in a tin mine near Wiuslow, Me. The beryl is of interest on 

account of its color, which is white, with a faint greenish hue under 

certain conditions of light. Mr. J. S. Diller examined the crystals and 

reported as follows:

The white beryl which you gave me to examine is full of gas and liquid inclusions, 

most probably air and water, to which the light color of the beryl is due. Besides 

these it contains a considerable amount of fine ferritic dust, but on the whole is about 

as pure as minerals usually are. The beryl itself is fresh, and has suffered but little, 

if any, alteration.

The sp. gr. at 27°C. was 2.707.

VII.

Si02 ................ 65.21

Ti02 ................ trace

A12O3 ............... 18.50

Fe2 03 ............... *0.33

 BeO ................ U3.03

MgO................ 0.09

K2 0 ?

Cs30)

Na2 0 ...........

LijO ............

H2 0 ...........

PaOfi. ...........

....... 0.14

....... 0.87

....... 0.16

....... tl.80

....... none

100.13 

* FeO, if present, not estimated.

tBeO and A12O3 separated in the manner described by Peufield. (Am. Jour. Sci. 

[3], xxxii, 114). 

t After drying at 110° C.

4. A SULPHIDE OF COPPER, SILVER, AND ZINC.

Mr. Richard Pearce gives an analysis1 of a mineral from the Gagnon 

Mine, Butte, Mont., which he describes as massive,-and in appearance 

much like bornite, with density 4.95 and hardness 3.5 to 4. A specimen received from Mr. Pearce, and analyzed at his request, had a 

density of 5.407 at 20° 0. It was rather brittle, but flattened out in 

part under the pestle. From analysis VIII 0.12 per cent, of gangue 

has been deducted. Pearce's analysis is given under IX.

Cu. ..............

Ag...... .........

Pb...... .........

Zn.. .............

Fe ....... .......

S ................

VIII.

40.24

21.80

1.46

12.83

1 Qft

20.88

99.19

IX (Pearce.)

 41.10

24.66

9.80

2.09

20.51

1.02

99. 18

'Proc. Colorado Soi. Soo., vol. 2, p. 70.
54 WASHINGTON LABORATORY. [HULL. 55.

The general formula deduced from both analyses is US, with the 

different constituents apparently in varying proportions. It is impossible from the specimens examined to decide whether the mineral is 

new or only a mixture.

»

5. AN ARGENTIFEROUS ARSENIDE OF NICKEL AND COBALT.

From Mr. W, George Waring, through Mr. Whitman Cross, a mineral 

from the Eose Mine, Grant County, K Mex., was received, which 

has the composition given under X. It is said to occur also in the 

Black Hawk Mine, in the same county. It has a steel-gray color, and 

the particles abraded by a sharp blow of the hammer " take fire, and 

the pathway of each particle thus ignited as it falls to the ground is 

marked very distinctly by a trail of dense, white smoke," according to 

Waring. In a closed tube a heavy sublimate of arsenic is formed on 

very moderate heating. The gangue of the mineral is mainly carbonate 

of lime and iron with quartz. The carbonates may be extracted with 

HOI, when the arsenide is left entirely unaffected and showing evidences 

of crystalline structure (" pyritohedral," Waring). The sp. gr., after 

correcting for 4.80 per cent, of quartz, was 6.644 at 20° C.

As...............

S ................

Ag..... ...........

Cn. ..............

Ph.... ...........

Fe...... .........

X.

74.04

0.13

4.78

0.04

0.03

0.44

Ni )

Co i " "

CaO ..............

MgO ..............

X.

*19.52

' 0.09

0.05

99.12

* The separation of Ni and Co miscarried. According to a blow-pipe analysis by 

Waring the proportion of Ni to Co is as 3 to 1.

The atomic ratio of Ni, Co, Ag, Fe to As is much above 1: 2.5, showing either that the substance is a mixture of two minerals with the 

general formulas BAs3 and BAs3 , or of arsenic with one of the formula 

BAs2. i

6. A BASIC CUPRIC SULPHATE.

Two soft lumps of ore of a light green color, (rubbing off on the fingers) from the Antler mine, Yucca Station, on the Atlantic and Pacific 

Railroad, in Mohave County, Ariz., gave the following composition, 

after deducting 8 and 6 per cent, respectively of gaugue, which latter 

consisted mainly of quartz and a brownish foliaceous mineral. Sp. gr. 

at 16° C., 3.93, after correcting for gangue, the density of which was 

assumed to be 2.6.
IITLLEBKANT).] ,MINERALOGICAL NOTES. 55

CuO... .....................

ZnO. ............ ............

CaO.. ......................

S03 ........................

H30.. ......................

XI.

68.19

0.29

0.05

20.46

11.11

100. 10

XII.

67.64

0.04

. 0.04

21 4Q

10.76

99. 97

The molecular ratios are:

RO SOS H20

I................... 10.00 : 2.98 : 7.19

II ................... 10§.00 : 3.15 : 7.01

which lead to the formula 3CuSO4 -f 7Cu[OH]2, for which theory requires 68.45 CuO, 20.69 SO3,10.86 H2O. If in time this should prove 

to be a well-defined species, which conclusion the absence of crystalline form and want of very close agreement in the analyses do not warrant at present, the name antlerite, from the mine in which it occurs, 

is suggested as appropriate.
ANALYSES OF NATURAL BORATES AND BOROSILICATES.

BY J. EDWARD WHITFIELD.

Most of tbe published analyses of natural borates have the boric 

acid determined either by difference or by some of the methods which 

have been shown to be inaccurate, and they are therefore subject to 

question as to the exact ratios and formulas. A method for the direct 

estimation of boric acid having been devised in this laboratory by Dr. 

F. A. Gooch, 1 it was thought advisable to repeat the analyses of a few 

of the borates, and verify, if possible, the given formulas or correct 

errors caused by defective analytical methods. With this object in 

view, the following analyses were undertaken.

The methods employed differ in many cases from those used by other 

analysts in the already published accounts of these minerals. In the 

estimation of the ferrous iron, the method employed was to decompose 

the finely ground mineral with hydrofluoric and hydrochloric acids in an 

atmosphere of carbonic acid, and heating to a temperature of about 

100° C. in a tightly sealed platinum vessel, devised and used expressly 

for such determinations, and when thoroughly decomposed which is 

generally thecase after standing twelve hours, with occasional shaking 

to titrate with permanganate of potassium. This method is undoubtedly 

superior to that employed by Eammelsberg and Tschermak in their 

analyses.

The direct estimation of the water was made, after drying the mineral at 104° 0., with the apparatus devised by Dr. Gooch,* by which 

the error caused by calculating the water from ignition and ignoring 

the oxidation of the ferrous iron is eliminated.

The silica in every case has been corrected by evaporation with hydrofluoric and sulphuric acids, and the residue added to the precipitate 

of iron and alurninia.

COLEMANITE, FROM DEATH VALLEY, CALIFORNIA.

Of this mineral there was put at my disposal two specimens very 

different in appearance. One, designated as A, was a large, transparent crystal of the ordinary type, to all appearances perfectly clear and 

free from impurities.

1 Bulletin U. S. Geological Survey, No. 42, p. 647.

2 Am. Chern. Jour., vol. 2, 1880, p. 247. 

56
WHITFIELD.l NATURAL BORATES AND SILICATES. 57

By analysis the following results were obtained, and I insert for 

comparison the analysis by Mr. J. T. Evans1 and the theoretical composition calculated from the formulas given below:

H20 =

B,03 =

CaO =

MgO =

A.

21.87

50. ~9>

27.31

.10

J. T. Evans. 

= 21.835 = 

= 50.990 = 

= 27.175 =

Theory. 

21.9 

50.9 

27.2

99.98 100.000 100.0

The molecular ratios from analysis A are CaO : B2O3 : H2O 2: 3 : 5, 

resulting in the simple formula 2CaO, 3B2O3 , 5H2O, the calculated composition of which does not differ much from the results of the analysis. 

Mr. Evans calculated the same formula from his analysis, in which the 

boric acid was determined by difference.

The second specimen, B, was from the same locality, but was in the

form of a deposit, implanted on gangue, and consisted of small blade-like 

crystals, almost white, but in some lights appearing of a greenish cast. 

By duplicate analyses the following results were obtained:

B.

H2O............................................ 22.66

B203 -........................................... 49.56

CaO............................................ 27.36

MgO............................................ .25

SiO2 ............................................ .44

100.27

22.70

49.62

27.40

.26

.47

100.45

These results prove the mineral to be the same as variety A, but 

containing very slight impurities. The difference in the general appearance of the two specimens suggested a crystallographic examination of variety B; and, through the kindness of Prof. E. S. Dana, the 

following description was furnished by Mr. H. S. Washington, of New 

Haven:

The white transparent crystals, of about 2 to 5mm in length, occur implanted on a 

light porous gaugue, either in parallel 

position or in rosette-like aggregations, 

overlapping one another like shingles on 

a roof. They have in several places implanted on them small, white opaque, 

spheroidal masses, presumably of priceite. 

The habit of the crystals is remarkable, 

being unlike almost all the forms of colemaiute previously described. Prof. A. W. 

Jackson3 gives one figure resembling these 

forms, though more complex. They look 

at first sight like two rhomboheclrse of calV

,v

Fig. 12. Crystalline 

form of eolernanite.

FIG. 13. Crystalline 

form of colemauito. cite; the combination of prism and orthodome giving the mineral a decidedly rhombohedral aspect, as shown in Figs. 12,13.

'Proc. Cal. Acad. Sci., No. 1; Nenes. Jahr., 1886, 1-1-37. 

2 Bull. Cal. Acad., No. 4, pp. 358-374, plates.
58 WASHINGTON LABOEATORY. [BULL. 55.

. None of the crystals examined admitted of good measurements, the faces being 

broken, rough, or curved. They were accurate enough, however, for determining 

the symbols. The plane W 501 was curved very conspicuously and regularly, the 

face having, near a 100, the position approximately represented by the symbol 501. 

Tnis habit was very constant, the prism m 110 and orthodome W 301 being the only 

planes observed, with the exception of b 010, produced by the perfect cleavage, and 

a small and very uncertain plane observed in one or two cases replacing the edge 

W 301 /m' 110.

PEICEITE, FROM CURRY COUNTY, OREGON.

The specimen examined was white and chalky, and proved to be very 

pure material. An analysis gave the following composition, and I copy 

the results of an analysis by Silliman 1 and another by Mr. Thomas 

Price 2 for comparison:

Whitfield. Silliman.

H8 0..................... 19.42 18.29

B2 03 ..................... 48.44 49.00

CaO..................... 32.15 31.83

NaCl,.Fe203 , A1203 ....... ........ .96

100.01 100.08 100.00

The ratios from my figures are CaO: B2O3 : H2O -19: 23: 36, which do 

not-conform to any simple formula. In both the earlier analyses the 

boric acid was determined by difference, and there is a discrepancy between them of about 2 per cent.

PANDERMITE, FROM THE ISLAND OF PANDERMA, IN THE BLACK SEA.

The material was hard and compact, somewhat resembling marble.

BW>...................................................... 19.40

B203 ...................................................... 48.63

CaO...................................................... 32.16

100.19

From these figures it will be seen that the priceite and the pandermite are in composition identical, the diiference being wholly in the 

physical appearance of the material. The priceite is soft and friable, 

while the pandermite is compact. From the results obtained it is apparent that they are the same mineral.3 

ULEXITE, FROM RHODES' MARSH, ESMERALDA COUNTY, NEVADA.

The material for analysis was taken from one of the nodules found 

in this locality, which on being broken exposed the fine, silky fibers 

characteristic of the mineral.

'Am. Jour. Sci., ser. 3, vol. 6, pp. 128-130. 

3 Aiu. Jour. Sci., ser. 3, vol. 5, pp. 287-290. 

3 Dana, Syst. Min., app. m 97.
WHITFIKLD.] NATURAL BORATES AND SILICATES. 59

An analysis gave the following figures:

Pound. Calculated.

SiOB -........................................ 0.04 .......

01............ ................................ 2.38 .......

B2O3 .......................................... 43.20 45.34

SOs........ ....:. ............................. 0.28 .......

CaO.~...................-I-.......-...... 14.52 15.04

Na^O......................................... 10.20 8.83

KaO.-..-....................... .............. 0.44 . .......

H20...... ................................... 29.46 30.79

100.5 : 100.00 

Deduct O = CL............... ................ .53

99.99

The molecular ratios from these figures are Na2O : CaO : B2O3 : H2O 

=16 : 26 : 62:163, which conform to no simple formula, If, however, 

we correct for impurities by throwing out the SiO2 , the K2O, as KC1, 

the remaining Cl as NaCl, and the SO3 as gypsum (CaSO4 , 2H2O) we 

can calculate the composition given above, from which we deduce the 

formula NaCaB5 09, 6H2O, which lies between the two formulas given 

by Eamuielsberg.1

LUDWiaiTE, FROM MORAWITZA, BANAT, HUNGARY.

The material consisted of fine, radiating, silky fibers, almost perfectly 

black, but showing a tinge of violet when freshly broken, very tough 

when hammered, but easily cut, associated with quite pure magnetite.

Analysis gave 

B.2 03 ....................................................... 12.04

FeaOs-..................................................... 37.93

FeO.......................... ............................. 15.78

MgO.................. .................................... 30.57

MnO.................. .................................... 0.16

.............................. ....................... 3.62

100.10

The ratios are B2O3 : Fe2O3 : FeO : MgO : H2O = 17 : 24: 24: 76: 20. 

Taking all the protoxides, together with the water, as basic, we have 

B2O3 : Fe2O3 : BO = 3 : 4:20. G. Tschermak 2 obtained for boric acid, 

by Marignac's and by Stromeyer's methods, 16.09 per cent, and 15.06 

per cent, respectively, but gives no water; and from his results deduces 

the formula 3MgO, B2O3 + FeO, Fe2O3 . If he sought for water by ignition, the oxidation of ferrous iron might easily have led to error.

DATOLITE.

The material investigated was the well-known mineral from Bergen 

Hill, New Jersey, and consisted of crystals about 5mm in diameter, trans1 Pogg. Ann., vol. 97, p. 301. 2 Tsch. Min. Mitth., 1874, p. 09.
60 WASHINGTON LABORATORY. [BULL. 55;

lucent, white, or of a pale greenish color. I have been unable to find 

any published analyses of the mineral from this locality, although it 

has been known for so long a time. 

By analysis I obtained 

Si02 ............................ ............................ 35.74

FeO............................ ...-........-.:..-.......... .31

CaO........................................ ................ 35.14

B203 ........................................................ 22.60

H3O........:......................... ...................... 6.14

99.93

The small amount of iron is undoubtedly present as an impurity; 

leaving this out, the molecular ratios are SiO3 : CaO.: B2O3 : H2O=60: 

63: 32 : 34, giving the formula

B2O3, H2O, 2CaO, 2SiO3 , or H Oa SiO3 BO2 . 

DANBURITE,'FROM RUSSELL, ST. LAWRENCE COUNTY, NEW YORK.

This mineral has been fully described by Profs. George J. rush 

and Edward S. Dana,2 although from the description given by them-of 

the color of their specimen I imagine they had material differing somewhat from mine. The mineral analyzed by me was reddish yellow to 

pink in color, brilliant m luster, and associated with quartz, pyroxene, 

and calcite.

In the analysis referred to 3 the boric acid was determined by Stro. 

myer's method. The figures obtained by my analysis are given in the 

first column; the second is the analysis made by Mr. W. J. Comstock 

for Professor Brush.

SiO2 .............

B203 .............

CaO ... ...... ....

Fe2 03+Al203 .....

1.

49.70

25.80

23. M

1.02 

.20

99.98

2.

48.23

26.93

23.24

.47 

.63

.99.50

The comparison of the two analyses shows the material difference to 

be in the amount of impurities.

AXINITE.

Two specimens of this mineral from different localities were analyzed. 

The first, from Cornwall, England, was of selected crystals of a dark, 

clove-brown color, translucent, and implanted on quartz. The second

2 Am. Jour. Sci., pt. 3, vol. 20, 1880, .pp. 111-118. 3 Loc. cit.
WHITF1ELD.] NATURAL BORATES AND SILICATES. 61

was the axinite from Bourg d'Oisans, Dauphiny, France. This specimen was 6f a beautiful pearl-gray color, and in some of the smaller 

crystals almost colorless and quite transparent. The third analysis in 

the series is one of the Dauphiny axinite, by Eammelsberg, and is copied 

from his description of the mineral1 for comparison.

Si03 . .........

A1203 . ........

Fe203 ........

FeO... .......

CaO... .......

MnO... ......

MgO .........

KaO ..........

B3 03 ..........

HsO.. ........

1

Cornwall.

42.10

17..40

3.06

5.84

20.53

4.63

0.06

4.64

1.80

100. 66

2

Bourg d'Oisans.

41.53

17.90

3. 90

4.02

21.66

3.79

0.74

4.62

2.16

100. 32

3*

Bourg d'Oisnns. 

Itamuielsborg.

43.46

16. 33

2.80

6.78

20.19

2. 62

1.73

.11

5.61

1.45

101. 08

The ratios from the results of analysis No. 2 are: SiO2 : Al2O3 +Fe2O3 : 

(FeO + MnO) + (CaO + MgO) : B203 : H2O=69 : 20 : 51 : 6 : 12, or 10 : 3 

: 8 : 1 : 2 giving

B2O3 . 3 . B2'"O3 . 8R"O . 2H2O . 10SiO2 , or BR3'"R4"H2 (SiO4 )5O. 

This expression will allow of the graphic formula :

In these analyses the value of R4 is approximately three atoms of calcium and one atom of iron and manganese taken together. It is therefore probable that axinite is an isomorphous mixture of two species, 

having R=Ca3Fe and Ca3Mn respectively. If we reckon all the R as 

calcium, we shall have the following theoretical composition :

A1203 

Si02 . H20. 

CaO . B203 .

20.9

41.1

2.5 

30.7

4.8

100.0

1 Zeit. d. geol. Gesellsch. xxi, 689.
62 ^ WASHINGTON LABORATORY. (BOLL. 55.

These results, while differing from those deduced by Bainmelsberg 

from his formula, agree very well with all the results of analysis No. 2.

Although the Stromeyer and the Marignac methods of estimating 

boric acid have been shown to be unreliable, and the determination of 

any constituent of a mineral by difference is unsatisfactory, nevertheless, 

on comparing the results of the various analyses, it will be seen that the 

directly determined percentages of boric acid do not differ greatly from 

the older values.

My sincere thanks are due to Mr. H. S. Washington for kindly furnishing the description of the unusual variety of colemauite.
METEORITES FROM JOHNSON COUNTY, ARKANSAS, AND ALLEN 

COUNTY, KENTUCKY.

BY J. EDWARD WHITFIELD.

1. METEORITE FROM JOHNSON COUNTY, ARK.

^ A fragment of this meteorite was received by Prof. F. W. Clarke 

from the former owner, Mr. J. C. Betten, of Eureka Springs, Ark. 

This fragment weighed a little more than thirty-five grammes; the exposed surfaces were oxidized, the oxide of iron extending into the 

numerous cracks; in some cases almost through the specimen. The 

trace of chlorine found by analysis will account in some degree for this 

oxidation.

The following analysis gives the composition of the iron. The loss 

is due to the partial oxidation of the iron:

Pe...................... v ................................. 91.87

Ni.................... ...*.............e--.-.................. 6.60

Co............. .............................................. trace

S.......................................................... 0.05

CombinedC ............................................... 0.15

P......................................^................... 0.41

Mn........................................ _............. trace

Cl......................................................... trace

Insoluble in HC1........................................... 0.34

99.42

Specific gravity ..................................... 7.837

This meteorite has since passed into the hands of Mr. G. F. Kunz, 

who has fully described it1, and from his description I copy the main 

points of interest.

This meteorite is of unusual interest on account of the observance of 

its fall, which occurred about three o'clock on the afternoon of March 

27, 1886. It struck the ground about 75 yards from the house of Mr. 

Christopher C. Shandy, six miles east of Cabin Creek, Johnson County, 

Ark. It measures 44cm by 39cm, and weighs 48,732 kilos (107£ pounds). 

A high ridge 12.5cm high at the highest point runs through the center; 

one-half the mass is not over 7.5cm thick, part of it is only 5cm, and 

around the edge it is only 2.5cm or less.

Mr. Kuuz gives two figures, which show how very dissimilar the two 

sides are; the upper side is ridged and deeply dented, while the lower

1 Am. Jour. Science for June, 1887.

63
64 WASHINGTON LABORATORY. [BULL. 55.

side is flat, and covered with shallow but very large pittings. The 

upper side is remarkable for sirira showing the flow and burning, and 

all running from the center toward the edge, identical with those in 

the Eowton, Nedagolia, and Mazapil irons, but on a larger scale.

On the upper side ten nodules of troilite are exposed, measuring from 

33mm jn diameter to 55mm long and 25mm wide; on the lower side there 

are twelve nodules, the largest measuring 19mm by 39mm. On the upper 

side these nodules are coated in spots with a black crust similar to that 

found on the mass, but on the lower side the crust extends completely 

around the side of the nodules, showing the fusion very plainly. The 

troilite is very bright, and in some cases where the nodules were broken 

they were found to be iridescent. This is one of the octahedral irons 

showing the Widmanstattian figures beautifully on etching, and is one 

of the Caillite group of Stanislas Meunier and of the Mittlere Lamellen of Brezina.

2. A METEORITE FROM ALLEN COUNTY, KY.

This meteorite was found about the middle of June, 1867, by Mr. 

James H. More, while hoeing tobacco, near Scottsville, Alien County, 

Ky. In shape it resembles a wedge, the thickness at base being 14cni , 

width 18cm, and length 16em ; the mass, as found, weighing a little more 

than 10 kilos, and having the characteristic pitted surface. A section 

shows nodules of troilite varying in diameter from barely visible points 

to about 12mmo. The markings on an etched surface are exceedingly 

fine, and require the aid of a lens to distinguish them. There appear 

to be two sets of figures, one of long, very fine lines, representing octahedral cleavage, the other series being smaller, more crowded, and 

barely perceptible. An analysis gave the following composition:

Fe............................... .......................... 94.32

Ni.......................................................... 5.01

Co.............................................. ............ trace

S........................................................... 0.34

P..................................................... ...... 0.16

Total C.. ................................................... 0.12

99.95 

Specific gravity.............'................................ 7.848

This iron, as regards markings and general appearance of section, 

resembles the Scriba and Salt Eiver meteorites more nearly than any 

others represented in the National Museum collection; but as no complete analyses of these two irons are at hand, the chemical comparison 

can not well be made. The percentage of iron appears rather high, 

but duplicate determinations gave corresponding figures.

The material for analysis was received by Prof. P. W. Clarke from 

Messrs. Wa.rd and Howell, of Eochester, K Y., the present owners of 

the meteorite, to whom we are indebted for the privilege of descrip-, 

tion.
SCORODITE FROM THE YELLOWSTONE PARK.

BY J. EDWARD WHITFIELD.

Among a number of deposits and incrustations, submitted for analysis 

by Mr. Arnold Hague, of the U. S. Geological Survey, was a specimen 

from the Joseph's Coat spring, on Broad creek, east of the Grand CaSou. 

This specimen had a coating of a pale greenish color, the mass consisting of alternate layers of light red or brown and white. At first it was 

supposed that the green color was due to the organic coloring matter 

so prevalent in the basins of springs iu the Park, but on examination 

it proved to be a compound containing arsenic and iron. Following are 

the figures obtained by analysis, on material separated as well as possible from the silica and earthy matter that always accompanies the 

deposits from the. springs:

SiO8 ........................................................ 4.35

Fe203 ..............:........................................ 33.29

As205 ........ ..........................'.................... 46.48

HS 0........................................................ 15.50

SOs-........... ... ................................. .84

100.46

The analysis shows the presence of some lilica and sulphuric acid, but 

mainly agreeing with the composition of scorodite. Eecalculating, leaving out impurities, we obtain the following figures, which agree closely 

with the theoretical composition of the mineral:

Calculated. 

Fe2 03 ............................'.................. 34.94 34.7

A82 05 ............ ................................. 48.79 49.8

H9O ............................................... 16.27 15.5

100.00 100.0

There are other localities in the Park where scorodite is being deposited. At the Constant Geyser, in Norris basin, the water is thrown out 

two or three times a minute to a height of from ten to twenty feet. 

Around the vents the greenish tints are perceptible in the incrustations, 

but only on the surface, for on breaking the sinter the cross section 

shows the thin layers of alternate scorodite and silica; but here the 

scorodite has been altered to liraonite, and the Inyers are of a brownish 

color the nearer the base of the deposit the stronger the dark color 

owing to the discoloration of the silica by the oxide of iron.

Bull. 55 5 65
66 WASHINGTON LABORATORY. [BULL. 55.

It is very difficult to scale off the green-colored matter from the surface of this deposit in quantity sufficient for analysis without admixed 

silica and iron oxide from the layer beneath it. After separating it as 

well as possible the following figures were obtained by analysis:

SiOa ........................................................ 49.83

A]303 --..................................................... 4.74

FesOs............ ...*...................................... 18.00

AssOs ........ .......*.......-..... .......................... 17.37

H20......................................................... 10.62

100.56

Scorodite, as found in the Park deposits, is a very unstable mineral, 

and only under favorable conditions is it kept from slowly oxidizing,' 

leaving the limonite carrying varying amounts of As2O5 .

For a description of the locality and manner of occurrence of scorodite 

in the Park reference must be made to the paper by Mr. Arnold Hague,1 

in which the whole subject is fully discussed.

1 Am. Jour. Sci., vol. 34,.Sept., 1887.
THE FLOW OF SOLIDS, OR THE BEHAVIOR OF SOLIDS UNDER

HIGH PRESSURE.

BY WILLIAM HALLOCK.

THE QUESTION.

Among the many physical questions that are of vital interest to the 

student of structural geology the one which may well contend for a 

position in the front rank is, What is the effect of pressure, with or 

without a rise of temperature, upon the rocks and rock-making magmas 

which form the outer shells of our earth? As a very important subdivision of this general question we have this: What is the effect of 

pressures upon so-called solids without any rise in temperature above a 

point far removed from their ordinary melting point? In other words, 

can we liquefy solids by pressure alone ? As corollaries we have any 

peculiarities at the instant of liquefaction and possible chemical reaction during this state of enforced liquidity.

These questions have long formed the subject of theoretical discussion, but in spite of the fundamental importance of their satisfactory 

and final settlement, they have seldom been investigated experimentally, 

doubtless owing to the difficulty of obtaining, measuring, and managing 

sufficiently high pressures.

Walther Spring may perhaps be rightfully called the pioneer in this 

work, having within the last few years published the results of much 

experimental work upon this question. His memoirs 1 would seem to 

prove without doubt and finally that pressures under 7,000 atmospheres 

will liquefy the large majority 2 of solids, and it is only a question of a 

little higher pressure to accomplish the result even with the most 

refractory. Further than this, Mr. Spring has investigated the second corollary, and finds-that chemical reaction takes place during this 

fusion j 1 at least when the volume of the products is less than that of 

the original substances.

Unfortunately, however, for the conclusive character of Mr. Spring's 

works, they have been seriously called into question, especially by

1 Bull, de I'Acad. de Bolg.» 2d ser., vol. 49, 1880, and 3d ser., vol. 9,1885; and Bull de 

la Soc. Claim, de Paris, vol. 39,1883, and 46,1886. 

'Bull, de I'Acad, de Bolg., 3d ser., vol.,49,1880,

67
68 . WASHINGTON LABOKATORY. tBULL.55.

Oh. Friedel.1 Bduard Jannetaz 2 repeated many of Spring's experiments, 

and his results confirm Friedel's criticisms rather than Spring's conclusions, which he (Jannetaz) contradicts in every essential point.

Such was practically the condition of the question two years ago, 

when the Director of the U.'S. Geological Survey, J. W. Powell, 

requested me to devote my time and thoughts to what we hoped would 

be its final settlement.3

It would be unjust to leave unmentioned here the elaborate and exhaustive series of experiments made by Henri Tresca 4 on " the Flow 

of Solids," which are fundamental as regards the point investigated, 

which, however, is but a small part of the general question.

In order that my meaning may be clear, I wish for myself and for this 

paper, to impress certain meanings upon certain terms or words. Primarily, t wish strongly to distinguish between causing a body to "flow" 

and rendering it a true liquid. Any substance may "flow" when the 

force acting to cause the molecules to change their relative positions is 

greater than the force with which the molecules are held in their original 

positions; i. e., is greater than the rigidity or viscosity of the substance. 

This can occur from two causes: an increase of the force tending to 

disturb the molecules, or a diminution of the resisting power, the 

rigidity of the material. The first cause may take the form of pressure, 

strain, or such like force; the second cause is heat, and possibly other 

agencies. Whether rupture or flow takes place when the deforming 

overcomes the resisting force depends upon the nature of the substance, its limiting conditions, and the time allowed for the accomplishment of the motion,

It is impossible to draw a sharp line between "liquids" and "solids;" 

for convenience they may well be classed as true liquids, viscous liquids, 

viscous solids, true solids. In the first class would fall such substances 

as, in a small fraction of a second, fill their containing vessel to a horizontal surface. As true liquids we should then have such as alcohol, 

water, glycerine, molasses, etc. Viscous liquids require several seconds 

to fill their containing vessel to a level surface; thick tar is a good 

example. When the substance requires hours or even weeks in which 

to yield to gravity and change its form, I would call it a viscous solid; 

paraffine, shoemaker's-wax, and even lead and some other metals are 

such. A true solid retains its original shape indefinitely under ordinary 

conditions of pressure and temperature, as steel, glass, etc. Of course 

such a thing as an absolutely or perfectly rigid substance is as unknown 

to us as is an absolute or perfect fluid.

1 Ch. Friedel, Bull, de la Soc. Chim. de Paris, vol. 39,1883, p. 626. 

2 Ed. Jannetaz, Bull, dela Soc. Chim. de Paris, vol. 40,1884; Bull, de la Soc. Mineral, 

de France, vol. 8,1885, p. 168.

2 This paper is essentially taken from a report made to Major Powell, dated at Watertown, Mass., September, 1885. (See foot note on page 75.)

4 Henri Tresca, Me"m. de 1'Inst. Savantes Grangers, vol. 18,1868. Comptes Rendus, 

vol. 66, 1868; Ixviii, 1869. See Tregca.., in Bibliography, p. 75.
HALLOCK.] THE FLOW OF SOLIDS. 69

If the above ideas are correct, " true liquefaction" is the diminishing 

of the rigidity or viscosity of a substance until its molecules change 

their relative positions as easily as in a true liquid.

T give these definitions merely that I may be understood in the use 

of these terms, and not because I think them new or especially good. 

In order that a substance may undergo a change in its chemical or 

crystalline character, it is undoubtedly necessary that it should be in 

the condition, at least, of a viscous solid, so that the molecules can 

slowly rearrange themselves, if there be any force urging them thereto. 

Our question is, will pressure alone impart to the molecules such a 

freedom of motion *? A priori it is inconceivable to me how or why it 

should. For with the exception of a few isolated substances at particular temperatures as water between 4° C. and ice at zero an increase 

of liquidity or a diminution of rigidity is simultaneous with an increase 

of volume, that is, with an increase of the iutermolecular distances, 

which is accomplished by " heating" the substance. In general, for one 

and the same substance over considerable ranges of condition, the 

rigidity diminishes as the intermolecular distances increase. How, 

then, can pressing the molecules nearer together be expected to give 

them a property which always accompanies their separation ?

THE APPARATUS.

The first requisite for the experiments was pressure, and naturally 

desiring the best machine, we were able, through the kindness of General Bene"t, Chief of Ordnance, to have the use in its spare moments of 

the testing-machine built by A. H. Emery for that department, and 

situated at Watertown, Mass. This machine undoubtedly enables the 

operator to obtain, measure, and manage high pressures better than any 

other.

Personally, I am greatly indebted to Capt. J. Pitman, of the Ordnance 

Corps, for suggestions as well on the construction of the holders as on 

the theoretical points; and also to Mr. J. E. Howard, the engineer in 

charge of the testing-machine, for his knowledge of the capacity of 

materials, and their best shape and quality to obtain the results desired. The apparatus was constructed by the American Tool and 

Machine Company of Boston, Mass.

For the preliminary tests it seemed desirable to have a holder which 

could be opened, so as to show the compressed material in position, and 

finally the following form was adopted:

Pig. 15 shows a section across the holder on the plane B B of Pig. 14, 

which in turn is a section on A A of Pig. 15. E E are the two halves 

in contact at h 7t, inclosing the cylindrical hole P, in which the substance to be pressed is placed, h li are strips of tissue paper, used as 

packing between the two halves. II and I'l', Fig. 14, are the two pins, 

acting as pistons, fitting into the hole P, to transmit the pressure; a a 

and a a are copper " gas-checks," placed in front of these pins, to flare
70 WASHINGTON LABORATORY. [BULL. 55.

out and fill tightly the hole, preventing any escape of material. Figures 

14 and 15 are one-fifth natural size. PL I shows the manner in which 

the apparatus was held int-he testing-machine and the pressure applied. 

P P P and P' P' P' are the jaws of the hydraulic clamps of the machine 

(capacity 1,000,000 pounds). H H are merely blocks to enable the clamp 

to properly hold the holder E B. F is a block to hold the back stationary pin in place. The lettering in Figs. 14 and 15 apply in PL I. V V 

is the hydraulic clamp on the fixed end of the testing-machine where 

the pressure is weighed. The block B B moves on a spherical surface

FIGS. 14, 15. Diagram of apparatus used in work on high pressures.

(E E E) on the plate T T T, thus permitting the adjustment of the face 

Of 0 perpendicular to the line of pressure or parallel to the rear surface of the pin II. To apply the pressure, the movable clamp P P' is 

forced toward V V by a hydraulic piston, thus forcing the holder E E 

over the pin resting against O; the pressure on O is measured by the 

hydraulic balance of the machine. In this manner a total compressive 

power of one million pounds was available, but as the pins yielded at 

110,000 pounds per square inch, the tests were not carried above 6,409 

atmospheres, or 96,000 pounds per square inch.

EXPERIMENTS.

With the above apparatus, used as described, the following tests were 

made:

FIKST TEST.

A paper roll containing 1.557 pounds "c. p. granulated lead" was 

placed in the hole F, the gas-checks and pins were inserted, the holder 

halves clamped together, and the pressure was slowly applied ; the 

amount of compression was measured in the distance to which E E had 

been forced over the right-hand pin. Multiplying the simultaneous
U. S. GEOLOGICAL SURVEY

DIAGRAM OF APPARATUS USED IN WORK ON HIGH PRE
THE FLOW OF SOLIDS. ' 71

loads and compressions, we obtain the icorlc done, and hence the possible heat generated. In this experiment the work done was 2,330 footpounds, or 3.0 thermal-units, 1 pound 1° F., sufficient to raise 1.557 pounds 

lead alone about 63° F., or 34° C. If the beat generated is dissipated 

into the holder E E, as is sure to be the case, the rise in temperature 

would be less than 1° C., or 1°.8 F.

Under a pressure of 6,000 atmospheres the granular lead showed not 

the least sign of true liquefaction. It was merely pressed together, 

and could easily be broken up and reduced to the original grains between the thumb and finger. It is true these experiments were not performed in vacuo, a condition which Walther Spring considers of importance. But if there is a true liquefaction, why does not the air rise to the 

top of the cavity and allow fusion, as it does when the granular lead is 

heated U There is no liquefaction, only a pressing and sticking together.

SECOND TEST.

Next 0.672 pounds1 of antimony was ground in a mortar until it went 

through a 48-sieve, and then it was similarly submitted to 6,000 atmospheres pressure, with the same result; the grains were simply stuck 

together, and were perfectly distinct in their original form. The cylinder 

formed was hard and tenacious, but gave no signs of liquefaction or recrystallization. The work done in this case might have raised the 

antimony alone 230° F., or 110° C., or holder and antimony 1°.8 F., 

or 1° C.

THIRD TEST.

Well-crystallized calcite, 0.271 pounds,2 was ground, put through a 

48-sieve, and submitted to a pressure of 6,000 atmospheres, producing 

practically no effect; the resulting mass being easily broken between 

the thumb and finger.

Finding it useless to have large quantities of the compressed material 

for elaborate examination, it was decided to expedite matters by putting 

in several substances at one time, and the following rather crucial test 

was made:

FOURTH TEST.

LH

a

OY D \ E / F

RH

FIG. 16. Diagram showing experiment.

L H, left-hand pin, stationary. E H, right-hand pin, entering the hole 

F, moving.

1 0.672 pounds antimony, solid, filled the hole F, 5 inches long. 

- 2 0.271 pounds of solid calcite fills the holder, 5 inches in length.
72 WASHINGTON LABORATORY. [BULL. 55.

The charge was composed as follows:

A. Small section of antimony from test II.

B. A stick of bees-wax -whittled round, nearly fitting the hole.

C. A stick of paraffine whittled round, nearly fitting the hole.

D. Bismuth prepared like the antimony for test II.

E. Paraffine, same as C.

F. Lead from test I.

d d were double-pointed tacks stuck into the top of the bees-wax and 

paraffine, and at a and c two old silver 3-cent pieces were laid on top of 

the wax and the paraffine in the cylinder.

What are we to expect? The silver pieces and tacks would fall 

through the liquid wax and paraffine, and B and C, if liquid, would mixNay, according to Spring's results, we should expect to find along the 

lower part of the mold a semi cylindrical piece of an alloy of lead, antimony, bismuth, possibly silver and iron, and above this the mixture of 

paraffine and wax. The actual result was that the substances all came 

out just as they went into the press. There was not the slightest trace of 

a tendency to flow on the part of the metals; the lead and antimony remained as they were, the bismuth acted precisely as did the antimony 

in test II. There was no sign of fusion of the wax and paraffine, which 

separated on their surface of contact (between B and C) clear and distinct, a, c, d, and d did not sink to the bottom on the contrary, they 

retained their original positions; and the silver pieces were forced against 

the top of the cylinder so powerfully, that their impression left in the 

steel holder was easily seen and felt, and the pieces were bent cylindrical, fitting the inside of the holder. Here we find a much greater rigidity of wax and paraffine under pressure than ordinarily supposed 

possible under any circumstances.

Nowhere was there a sign of true liquefaction. The wax and paraffine had acted only as viscous solids, and flowed only to fill the 

available opening.

FIFTH TEST.

In a similar way the following substances were subjected to a pressure of 6,000 atmospheres, with the results as stated:

Sodium carbonate, dry. Stuck together slightly, resembling chalk; easily cut with a

knife. 

Sodium sulphate. Probably dissolved in its water of crystallization (lOH2o) i it was

forced out between the halves of the holder as a milky liquid which solidified.

The little left in the holder resembled paraffine in appearance, but soon weath- 

 ered to a white powder. 

Zinc sulphate (-j-7H2O). No signs of fusion; merely stuck together; the original

pieces of crystals easily visible. 

Copper sulphate (+5H2O). Same as zinc sulphate. t

SIXTH TEST.

Potassium chloride. Formed a hard lump, whose fracture resembled that of loaf

sugar or that of marble, with the original crystals visible; no trace of fusion. 

Sodium chloride. Similar to potassium chloride, only a little more compact.
MALLOCK.J THE FLOW OF SOLIDS. . 73

Ammonium chloride. Still more compact, resembles vegetable ivory; possibly the 

beginning of fusion. Observe the order of increasing effect:

KC)<NaCl<NH4Cl.

Sulphur roll. Ground and put through a 48-sieve; formed a hard, solid, brittle mass, 

but the original grains were easily distinguishable, there being no trace of a true 

liquefaction.

SEVENTH TEST.

Powdered glass. No effect; scarcely coherent.

Powdered rosin. Very good fusion.

Powdered borax. A compact, chalk-like mass, slightly translucent; no crystallization. . .

Powdered zinc and sulphur. No trace of fusion or chemical union apparent. Carbon disulphicle dissolved out the sulphur so completely, that the remaining zinc 

gave a mere trace of sulphureted hydrogen on treating with hydrochloric acid. 

The zinc was slightly coherent, but there was no fusion and no zinc sulphide 

formed,

After obtaining the above results it seemed useless to continue this 

line of experiments, and preparations were made to use more rigid steel, 

by which it was hoped that pressures of at least 30,000 atmospheres 

might be obtained j also for making the compressions in vacuo. Unfortunately thus far nothing but preparations have been made, since 

the testing-machine is kept fully occupied with the special work of the 

department to which it belongs. It is hoped, however, that this investigation will soon be taken up again and carried to a close; till then 

our conclusions are only temporary.

The above substances were also compressed by W. Spring1 in vacuo 

with the following results:

Lead. Perfect fusion at a pressure of 2,000 atmospheres. At a pressure of 5,000 atmos'

pheres it ran out of all the cracks (fentes) of the apparatus. 

Bismuth. At a pressure of 6,000 atmospheres, perfect fusion. 

Tin. At a pressure of 3,000 atmospheres, fusion. 

Zinc. At a pressure of 5,000 atmospheres, perfect fusion. 

Antimony. At a pressure of 5,000 atmospheres, beginning effusion. 

Sulphur, prismatic. At a pressure of 5,000 atmospheres, fusion to the octahedral form. 

Sulphur, plastic. At a pressure of 6,000 atmospheres, fusion to the octahedral form. 

Sulphur, octahedral. At a pressure of 3,000 atmospheres, fusion to the octahedrs.

form.

Potassium chloride. At a pressure of 5,000 atmospheres, perfect fusion. 

Sodium chloride. At a pressure of 5,000 atmospheres, perfect fusion. 

Ammonium chloride. At a pressure of 4,000 atmospheres, perfect fusion. ' 

Sodium sulphate (10H2 0). At a pressure of 3,000 atmospheres, perfect fusion. 

Zinc sulphate (7H20). At a pressure of 5,000 atmospheres, perfect fusion. 

Copper sulphate (5H2O). At a pressure of 6,000 atmospheres, completely crystallized. 

Sodium carbonate, dry. At a pressure of 5,500 atmospheres, stuck together (agglomcrd). 

Iceland spar. At a pressure of 6,000 atmospheres, imperfect fusion. 

Borax (crystallized). At a pressure of 7,000 atmospheres, imperfect fusion. 

Glass (powdered). At a pressure of 6,000 atmospheres, no effect. 

And so on to the end.

1 Bull, de 1'Acad. R. do Belg., n, xlix, 1880. (See foot-note on page 75.)
74 WASHINGTON LABORATORY. [BULL. 55.

Excepting the last four substances mentioned, our results are directly 

opposed to those of Spring, but support the criticisms of Friedel and 

Jannetaz.

CONCLUSIONS. :

Conclusions at this stage of the investigation are necessarily prema. 

ture and tentative; still it may not be out of placo to summarize the 

results of these and other experiments.

It seems established that pressure alone can not truly liquefy a solid, 

i. e., diminish its rigidity. Consequently, we can scarcely expect chemical and crystalline changes by pressure alone. Solids can be made to 

flow and act in that respect, as liquids, by pressure, which overcomes 

the rigidity without diminishing it. In this case the time allowed for 

the motion is of vital importance.

Whether further investigation will alter these conclusions or not is a 

question of time; at present, I believe them the only true ones to be 

drawn from the available facts.

REFERENCES TO THE LITERATURE.

BATTELI and PALAZZO. On the change of volume of some substances on melting. R.

Ace. del Lincei. 1. 1885. pp. 1-20. 

A. BATTELI. Influence of pressure on the melting point of some substances. Atti

del R. 1st. veneto di Sc. ed Arti. (6). 3. 1885.

 Also, II Nuovo Cimento (3). 19. 1386. pp. 232-243.

 Atti del R. 1st. veneto di Sci. ed Art. (3). 1886. p. 35.

JAMES THOMSON BOTTOMLEY. Melting and regelationof ice. Nature, vol. 5, p. 185

(January 4). 1872.

R. BUNSEN. Rise of the melting point with pressure. Pogg. Ann. 81. 1850. 

L. CAILLETET. Effect of pressure on chemical action. Naturforscher. 5. p. 4. 

MICHAEL FARADAY. Regelation. Proc. Roy. Soc. 10. 1860. p. 430, and Pogg. Ann.,

Ill, 1860. p. 647.

FORBES. Regelation of ice. Phil. Mag. (4). 16. 1858. p. 544. 

ED. FREMY. Formation of coal by pressure. Comptes Kendus, 88. 1879. p. 1048.

May 26. 

CH. FRIEDEL. Criticism of the work of W. SPUING. Bulletin de la Socie"t6 Chimique

de Paris. 39. 1884. p. 626. Reviewed by W. S. B., Amer. Chem. Jour. 6. 1884.

p. 129.

G. P. GRIMALDI. On the variation by pressure of the temperature of maximum density of water. Gazz. Chim. Ital. 15. 1885. p. 297. 

R. VON HELMHOLTZ. The change of melting point calculated from the vapor tension

of ice. Wiedemann Ann. 30. 18?7 p. 401-432. 

HOPKINS. ' Rise of melting and boiling point with pressure. Dingler's Polyt. Journ.,

134. 1854. 

ED. JANNETAZ with NEEL & CLERMONT. Note on the crystallization of substances

under high pressure. Bulletin de la Soc. Chim. de Paris. 40. 1884. p. 51.

 Effects of compression on quartz. Bulletin de la Soc. Mineral, de France. 8.

1885. p. 168. 

E. MALLARD an d H. LE CHATELIER. . On the variation with pressure of the temperature

at which the transformation of iodide of silver takes place. Bulletin de la Soc.

Mineral, de France. 7. 1884. p. 478-484. 

W. PEDDIE. Note on the variation .by pressure of the melting point of paraffine, etc.

Proc. Edin. Roy. Soc., 1884-'85. No. 120. pp. 155-157.
HALWCK.I THE FLOW OF SOLIDS. 75

F. PFAFF. Effect of pressure on chemical action. Neues Jahrbuch fur Mineralogie, 

etc. 1871. pp. 834-839.

 Plasticity of ice. Pogg. Ann. 155. 1 75. p. 169. Also, Sitzungs-Ber. der

phys.-ined. Societat zu Erlangen. 1875. Heft 7. p. 72. 

L. PFAUNDLER. Regelation of ice. Der Naturforscher. 2. 1869. p. 371. 

F. E. REUSCH. Deformation of ice. Pogg. Ann. 125. 1865. p. 304. 

CARL SCHULTZ. On the freezing point of water out of gas solutions and on the regelation of ice. Pogg.'Ann. 137. 1869. p. 252. 

WALTHER SPRING. Eesearches on the property which substances possess of fusion

(de se souder) under pressure. Bulletin de 1'Acad. Roy. de Belg. 2d series. 49.

1880. p. 323-379.

 On chemical union by pressure. Bulletin de la Soc. Chim. de Paris. 39. 

1883. p. 641.

Reaction between sulphate of barium and carbonate of sodium under the influence of pressure. Bulletin de 1'Acad. Roy. de Belg. 3d series. 9. 1885.

p. 204-208. Continued in Bulletin de la Soc. Chim. de Paris. 46. 1886. p. 299. 

SAINT VENANT. Motion of liquid, or ductile s6lid particles flowing through an

orifice. Part I. Comptes Rendiis, GO. 1868. p. 1311-1324. Part II. Comptes

Rendus. 68. 1869. p. 290-301. 

JAMES THOMS'&N. Theoretical considerations on the effect of pressure in lowering

the melting point of ice (freezing point of water). Trans. Roy. Soc. Edin. 16. 

' 1849. p. 575-581. 

WILLIAM THOMSON. Melting point of ice lowered by pressure. Phil. Mag. [3J.

37. 1850. p. 123. 

HENRI TRESCA. On the flow of solids. Mdmoires de 1'Institut, Savants Strangers

Sci., Math. etPbys. 18. 1868. p. 733-799.

 Also, Comptes Rendus. 66. 1868. p. 263-270.

 On the application of the formulae for the motion of permanent liquids to the 

flow of solids. Coinptes Rendus. 66. 1868. p. 1027-1032, 1244-1246, and 

1305-1311.

 On punching and the mechanical theory of the deformation of metals. Comptes Rendus. 68. 1869. p. 1197-1201.

 On the flow of solids. Mdmoires de 1'Institut, Savants Strangers Sci. Math. 

etPhys. 20. 1872. p. 75-137.

 Application of the flow of solids to rolling and punching. Me"moires de 1'Institut Savants Strangers Sci. Math, et Phys. 20. 1872. p. 137-185.

 Continuation of the article on the flow of solids. M6moires de 1'Institut Savants Strangers Sci. Math, et Phys. 20. 1872. p. 281-287.

On the flow of solids and the punching of metals. M<Sinoires de 1'Institut,

Savants Strangers Sci. Math, et Phys. 20. 1872. p. 617-838.

An abstract of the foregoing article appeared in tho American Journal of Science, 

vol. 34, 3d series, 1887, p. 277. In a note published in the same journal (vol. 35, 1888, 

p. 78), Mr. Spring violently attacks my" interpretation of our results, especially rny 

nse of the word "fusion," which I have employed in its secondary sense, as meaning 

a uniting as if by melting with hcnt; the case of actual fusion by heat being specifically 

excluded. It seemed to me best to leave the word in the above article and make this 

explanation of its use. See, also, W. Spring, Bull. Acad. roy. Belg., vol. 16, 1888, p. 

43; also Am. Jour. Sci., vol. 36, 1888, p. 286. And. W. Hallock, Am. Jour. Sci., vol. 

36, 1888, p. 59; also ibid., vol.37, 1889, p. 402; also Zeitschr. fur Phys. Chern., vol. 2, 

1888, p. 378.

MISCELLANEOUS ANALYSES.

77

FELDSPAR. FROM A FELDSPATHIC MICA SCHIST, CENTRAL SHAFT 

OF THE HOOSAC TUNNEL, MASS.

[Collected by J. E. Wolff. Analysis by R. B. Riggs.]

SiO2 ..-.......-....:............-......................... 69.69

AlaOs..................................................... 18.60

FeA-.-.................................................. trace

CaO ......'................................................ trace

MgO ..................................................... .20

NajO ..................................................... 10.28

KaO...................................................... .40

Ignition.................................................. .42

99.59

TWO FELDSPARS. FROM THE PORPHYRITIC MICA SCHIST OF GREYLOCK MOUNTAIN, MASS.

[Collected by J. E. "Wolff. Analyses by R. B. Riggs.]

I. II.

SiO2 ......................................... 68.08 67.83

Ala03 ,Fe903 .................................. 20.11 19.92

MnO ......................................... trace trace

CaO...... ...................................* trace trace

MgO ....w.................................... trace trace

NaaO......................................... 11.00 11.65

KsO.......................................... .36 .25

Ignition...................................... .31 .12

99.86' 99.77

In neither case does the Fe2O3 exceed .5 per cent.

THREE FELDSPARS FROM DELAWARE.

[Separated by J. S. Diller from rocks collected by Prof. F. D. Chester. .Analyses by R. B. Riggs.]

A. Specific gravity, 2.592-2.877. From a typical gabbro. Brandywine Creek.

B, Specific gravity, 2.592-2.749. From Iron Hill hyperite, changing 

to diorite. Near Whitaker's ore-pit.

79
80 WASHINGTON LABOKATORY. [BULL. 55.

C. Specific gravity, 2.592-2.780. From a typical hypersthene gabbro. 

Fifth and Yan Buren streets, Wilmington.

A. B. c.

SiOjt................................ 70.37 44.09 51.44

Ala03 ............................... 18.36 35.41 30.05

Fe203 ............................... .58 .51 .96

MnO ............................... trace trace .....

CaO................................. 5.08 18.47 13.19

MgO ............................... .04 none trace

Na.,0............................... 4.32 .99 4.07

K20 ................................ .63 .19 .21

Ignition............................ .45 .35 .35

99.83 100.01 100.27

B is evidently anorthite.

TRIASSIC SANDSTONE FEOM MARYLAND.

A hard, compact building stone, from the Jaittelle quarry, near Hancock. Color, rich reddish brown. Analysis by F. W. Clarke. 

A. Analysis by fusion with alkaline carbonates. 

B. Analysis by solution in strong HOI.

A. B.

Ignition................ 2.79 Insoluble............... 88.68

Si03 ................... 76.43 Fe2 03 .................. 7.13

A1203 , Fe203 ............ 17.78 CaCO3 ................... 1.32

CaO ................... .84 MgO ................... .66

MgO................... .92 HS 0 .................... 2.20

MnO................... trace 

Alkalies................ undet. 99.99

t Kesidue nearly white. 

98.76

LIMESTONE FROM THE AUGLAIZE RIVER, NEAR DEFIANCE, OHIO.

[Highly bituminous. Nearly black, resembling a slate. Contains visible pyrite. Partial analysis by

J. Edward Whitfleld.]

Ignition ................................................... 24.03

Si02 ....................................................... 39.95

Fe.203,A]203 ................................................ 20.22

MnO ............ .......................................... trace

CaO................*......................... .......... 10.06

MgO...:...........................................-...... 2.92

Alkalies ................................................... undet.

S (pyritic) ................................................. undet.

97.18 

COs in carbonates.......................................... 12.49

Organic carbon ............................................ 5,29
MISCELLANEOUS ANALYSES. 81

TWELVE ROCKS FROM MENOMONEE RIVER, MICHIGAN AND WISCONSIN.

[Collected by E. D. Irving. Analyses by K. B. Riggs.J

A. Massive diabase. Lower Quinnessec Falls, Wisconsin side.

B. Green chloritic schist. Shore just below Lower Quinnessec Falls, 

Wisconsin side.

0.. Light gray gabbro, from near B,

D. Schistose gabbro, adjoining 0.

E. Silvery schist, adjoining D. 

F. Light-colored gabbro. Barrier Rock, at Sturgeon Falls, Michigan 

side.

G. Adjoining and similar to F; altered and somewhat schistose.

H. Silvery schistyadjoining G.

I. Uralitic gabbro. Barrier Eock, Big Quinnessec Falls.

J. Dark-gray granite. Small cove just below the " Horse-Eace," Big 

Quinnessec Falls, Wisconsin sido.

K. "Augengneiss," with red feldspar. Lower end of " Horse-Eace," 

Big Quinnessec Falls, Michigan side.

L. Porphyroid. Just below Big Quinuessec Falls, Wisconsin side.

	A. B. C. D. E. F. 

Si02 ................. 43.80 44.49 47.96 49.19 46.21 51.46

AleOs-................ 16.08 16.37 16.85 18.71 18.38 14.35

Fe2 03 ................. 9.47 '5.07 4.33 5.03 3.30 3.90

FeO.................. 10.50 5.50 4.17 4.04 3.90 5.28

CaO.................. 7.81 7.94 13.25 5.92 6.28. 9.08

MgO ................. 6.54 7.50 9.15 7.98 7.03 9.54

NaaO .................. 1.96 2.59 1.25 1.44 2.14 2.92

K8O.................. .34 .56 .30 .77 .35 .24

HaO .................. 3.99 4.99 2.89 5.05 3.82 3.30

COa .................. 0.8 5.38 .08 1.82 8.32 .20

100.57 100.39 C100.23 99.95 99.73 100.27

G. H. I. J. K. L.

SiOa ................. 3d.05 45.70 48.35 54.83 67.77 60.69

A] S03 ................. 24.73 16.53 15.40 25.49 ' 16.61 16.69

Fe8 p3 ................. 5.65 4.63 ' 4.04 1.61 2.06 2.06

FeO.................. 6.08 3.89 4.63 1.65 1.96 .93

CaO.................. 1.25 4.28 10.38 6.08 1.87 1.40

MgO.... ............. 11.58 9.57 11.61 1.96 1.26 1.15

Na.2 0 ................. 2.54 .55 1.87 5.69 4.35 2.46

K2O .................. 1.94 3.82 .35 1. fc7 2.35 5.23

II.-0.................. 7.53 4.70 3.60 1.18 1.69 1.70"

COa .................. .93 5.95 .08 .18 .19 1.42

100.23 99.62 100.31 100.54 100.11 99.73

ROCKS FROM PIGEON POINT, MINN. 

[Collected by E. D. Irving.]

A. Average granite rock. Analyst, W. F. Hillebrand. 

B. Eed granite, part of A. Analyst, J. Edward Whitfield. 

C. Soda orthoclase from A. Analyst, J. Edward Whitfield. 

Bull. 55 6
82 WASHINGTON LAB6RATORY. [BULL. 55.

D. Altered quartzite in contact with B. Analyst, J. Edward Whitfield.

E. Typical olivine gabbro. Analyst, W. F. Hillebrand. 

F. Augite from gabbro; partial analysis. Analyst, E. B. Eiggs. 

G. Bock occurring between A and E. Analyst, W. F. Hillebrand. 

H. Quartz porphyry. Analyst, W. F. Hillebrand.

I. Mottlings (greenish) from H. Analyst, W. F. Hillebrand.

J. Groundmass of H. Analyst, W. F. Hillebrand.

K, L, M, N, O, P, Q, E. Altered quartzites. Analyst, E. B. Eiggs.

E.

49.88 

1.19 

18.55 

2.06 

8.37 

.09 

9.72 

trace 

.02 

5.77 

.68 

2.59 

none 

1.04 

.16 

trace

SiOs. ............

Ti08 .. ...........

Ala03 . .. ......

FesOs. ...........

FeO.. ...........

MnO ............

CaO. ............

SrO .............

BaO...... .......

MgO ............

K90 .............

NaoO .......... ..

Li3 0... ..........

HS0 .............

P2 06 . .........

01...... .........

80s.....'.. .......

A.

............... 72.16

............... .39

..............I 12.98

............... .67

............... 2.99

............... .09

............... .65

............... ?

............... .15

............... .57

............... 4.94

............... 3.42

..... ...... .... none

............... 1.20

............... .20

B.

68. 36 '

1.57

13.76

2.65

2.75

trace

.70

unclet.

uudet.

.68

4.48

3.56

none

.98

.33

.66

C.

65.00

18.22

2.64

1.06

.06

4.18

8.40

......

.46

D.

63.82

2.66

14.65

3.16

5.12

none

.70

undet.

undet.

2.08

2.81

1.95

none

. 2.62

.19

.33

Si02 .. 

Ti02 . 

A1203 . 

Fe203 . 

:FeO.. 

MuO . 

 aO.. 

SrO .. 

BaO.. 

MgO . K2 0 .. 

Na20 . 

Li aO.. 

H20.. 

P2 05 .. 

01....

100.41 100.48 100.02 100.09 100.12

F.

48.34

1.98

2.90

4.68

14.15

15.10

11.34

G.

57.98

1.75

13.58

3.11

8.68

.13

2.01

trace

.04

2.87

3.44

.3. 56

trace

2.47

.29

trace

99.91

H.

74.00

.34

12. 04

.78

2.61

.05

.85

trace 

.12 

.42

. 4.33 

3.47

trace? 

.86 

.06

trace

I.

77.70

.30

7.67

3.55

3.29

.04

.26

?

none

1.83

1.04

1.96

trace

2.36*

none

J.

76.57

.42

9.21

1.67

3.94

.05

.73

trace?

nonie

1.51

1.02

3.07

trace

1.89

trace

99.93 100.00 100. 08

* By difference.
MISCELLANEOUS ANALYSES. 83

fiiO

Ti03 .

A1203 

Fe2 03 

FeO . MnOCaO .

SrO .

BaO.

MgO 

Na20 

K2 0 . 

Iguiti

SiO»,

A12 03 

Fe203 

 FeO.

MnO 

CaO..

SrO ..

BaO..

MgO 

Na^O 

K2 0 .

Ignitl 

A.

on

From 

H2O .

Si02 .

TiO*.

P206 .

S03 ..

A1203 

Cr203 

Fe203 

FeO.

MuO 

BaO.

SrO..

CaO .

MgO 

K20 ..

Na20

K. 

............................. 73.14

.............................. .04

............................. 12.60

.............................. 7.57

.............................. 1.31

.............................. .43

............................. 1.67

............................. 1.78

............................. 1.00

.............................. .83

100. 37

0. 

.............................. 72.25

............................. trace

............................. 10.73

............................. 8.01

............................. 38

42

............................. 1.85

............................. 2.03

.........r... ................ 2.56

............................. 2.D5

100. 28

TWO ROCKS FROM MONT./ 

. [Collected by A. C. Peale. Analyses by T. ]

Cottonwoocl Creek. B. Hills east

1

L.

71.00 

.44 

12. 88 

6.69 

.65 

trace 

.21 

undet. 

undet.0 

1.68 

1.43 

2.95 

2.03

99.96

P.

83.69 

trace? 

7.50 

1.81 

.38 

trace 

.39 

undet. 

undet. 

.35 . 

2.46 

2.61 

.72

99. 91

1NA. 

M. Chatard. |

of Fort E

A. 

3.19 

51.65 

.55 

.21 

.19 

13.89 

'.08 

2.70 

4.80 

.15 

.19 

undet. 

4.07 

11.56 

4.15 

2.99

M. 

74.22 

.16 

10.61 

7.45 

'.85 

none 

.56 

undet. 

undet. 

1.48 

2.12 

1.08 

1.79

100.32

Q.

73.64 

trace 

11.25 

6.24 

1.04 

none 

.36 

undet. 

undot. 

1.57 

3.04 

1.42 

1.98,

100. 54

lliS.

B.

5.42 

46.90 

.41 

.44

10.17 

.33 

1.22 

5.17 

.10

6.20 

20.98 

2.04 

1.16

N. 

73.65 

trace! 

11.08 

7.24 

.77 

trace 

.40 

undet. 

undet. 

1.52 

1.67 

1.65 

1.88

99.86 

R.

59. 71 

trace 

18.32 

8.11 

.85 

none 

1.05 

uudet. 

undet. 

3.54 

1.93 

3.43 

3.24

100. 18

100.37 100.54
84 WASHINGTON LABORATORY. [BULL. 55.

Separations from B. Partial analyses.

SiOs .... .........................

A1303 . ...........................

Fe203 .... ...........:............

FeO

CaO. ............................

MgO ..... .......................

Groundmass. 

.............. 5.40

............. ' 65,58

............. C 14.94

.............. i little

............. 3.60

.............. 3.45

Pyroxene.

51.95

4 21

5.90

23.32

13.81

99.19

FIFTEEN ROCKS FROM CALIFORNIA.

(Collected by J. S. Diller. Analyses A, B, C, by T. M.Chatard; D, by W. F. Hillebrand and T. M. 

Chatard ; E, by R. B. Biggs; and the remainder by W. F. Hillebrand.]

A. Basalt, from 1 mile southeast of Paine's Creek, on road from Ked 

Bluff to Lassen Peak.

B. Ancient lava. Old crater at head of Mill creek.

C. Lava, from Buntingville.

D. Basalt. Top of Inskip Crater, 25 miles ease of Ked Bluff.

E. Lava. Above falls on south fork of Bear Creek, Shasta County.

F. Basalt. Cinder Cone, 10 miles northeast of Lasseu Peak.

G. Basalt. One mile east of summit of Cascade Range, on road from 

Fort Klamath to Crater Lake. '

H. Andesite lava. One mile west of Summit, on Bidwell's Koad, 

Butte County.

I. Lava. West end of Butte Mountain, Plumas County.

J. Audesite. Tuscan Buttes, 7 miles east of Eed Bluff.

K. Ancient lava. Northeast of Willow Lake, near Geyser, Plumas 

County.

L. Lava. Two miles northwest of I 

M, Lava. Slate Creek, west of Dei 

K Lava. Slate Creek, northwest 

trail. 

O. Lava. Summit of Mount Stover

A. 

Si0.2 ... ............... .....---- 47.93

TiO,.. ......................

AljOg .......... ............

FeO .........................

MnO...... ..................

CaO........................

SrO ........................

BaO.... ....................

MgO.......................

KaO ........................

NasO .......................

Li.3 0 .........................

P806 ........................

.73

18.51

.... 2.07

..... 7.25

..... .20

11.14

9.03

.24

..... 2.28

.76

..... .11

)eer Cree 

er Creek 

of Deer (

-, Plumas

B.

57.11 

.95 

17.78 

3.54 

2.74 

.33 

7.21 

trace ? 

.03 

3.41 

1.86 

3.81

.98 

.26

k meadows, 

meadows. 

>eek meadows 1

County.

C. D.

67. 89 50. 89 

.21 .79 

17.29 16.76 

2. 39 3. 86 

. 21 4. 69 

. 12 . 13 

3.01 11.72 

.04 ..... 

. 03 trace 

.66 - 8. 49 

1. 69 . 32 

5. 11 2. 61

1.34 

.12

.41

.09

Lassen

E. 

68.10 

, .16 

15.50 

3. 20 

none 

trace 

3.02 

trace 

.06 

.10 

3.13 

4.20 

none 

2.72 

.03

100.25 100.01 100.11 100.76 100.21
MISCELLANEOUS ANALYSES. 85

Si02 ... 

TiO2 ... 

A1203 .. 

Fe203 .. 

FeO... 

MnO .. 

CaO... 

SrO... 

BaO ... . MgO-. 

K20...

Li20. 

H20. 

P2 06 .

Si02 .. 

TiOs.. 

A12 03 . 

Fe2O3 - 

FeO.. 

MnO. 

CaO.. 

SrO .. 

BaO.. 

MgO. 

K2O.. 

Na20. 

Li20.. 

H20.. 

P205 ~ 

S03 ...

F.

57. 25

.60

16.45

1.67

4.72

.10

7.65

trace

.03

6.74

1.57

3.00

none

.40

.20

100.38

K.

74.24

.20

14.50

1.27

.67

.06

:ii

trace

.18

.25

3.66

3.00

none

2.04

.07

.03

G.

57.47

.75

18. 86

2.21

4.08

.10

7.42

.11

.03

4.27

.73

3.85

none

.22

.24

100.34

L.

74.65

.21

14.11

1.08

.29

.11

.80

trace

.08

.20

4.59

2.81

none

1.40

trace

H.

55.20

.92

18.68

3.14

4.42

.14

8.02

.02

.03

4.59

1.01

3.66

none

.51

.24

100.58

M.

73. 62

.21

14.24

.93

.67

.08

1.07

trace

.10

.33

4.28

3.25

none

1.29

.02

I.

55.53

.56

17.63

2.81

3.59

.08

8.74

.06

.02

5.85

.92

3.09

none

1.24

.21

100. 33

N.

73.64

.11

13.44

.60

.74

.06

1.26

.02

.11

.26

4.50

3.51

trace

1.99

.06

J.

60.93

.61

18.56

2.68

2.19

.10

6.63

.12

.02

2.37

1.33

3.79

none

.90

.18

100. 41

O.

72.40

.18

14.81

.81

.68

.07

1.94

.04

.10

.47

3.30

3.91

trjvce

.59

.03

100.28 100.33 100.09 100.30 100.13

ORES OF IRON AND MANGANESE.

A. Iron ore from land of William Tabb, 3 miles from Catherine Furnace, Spotsylvauia County, Va.

[Analysis by J. Edward Whitfield.]

Si02 

Fe.. 

Mn. 

S. .. 

P...

A.

4.97

53.39

.60

,09

.66

B. Iron ore, Church Mountain Mine, Eockingham County, Va. 

C. Manganese ore, same locality.
86 WASHINGTON LABORATORY. [BULL. 55.

[Analyses by F. W. Clarke.]

	B. C. 

Ignition..... .......... 12.78 Ignition............... 11.30

Insoluble.... .......... 12.70 Insoluble.............. 22.11

. Fe..................... 43.60 Fe2q3 ,Al203 ............ 5.14

Mn .................... 8.45 Mn !..................... 39.20

S ...................... none Co..................... 2.48

P...................... .14

The manganese ore contains no manganese dioxide. Its high percentage of cobalt is noteworthy.

D. Iron ore. Eidge north of Clinch Eiver, 5£ miles above Stock 

creek, near and just west of Peckover Mill, Wise County, Va.

[Analysis by T. M. Chatard.]

D.

SiOs-.................................................... 14.75

Fe ...... ............................................... 48.97

MnO .................................................... .12

S........................................................ .83

P........................................................ .067

E. Eastern extension of Cranberry bed, three-fourths mile east of 

Cranberry Creek, Mitchell County, N. C.

F. Western extension of Cranberry bed, Hardy Graves' tract, onefourth mile southwest of Elk Park, Mitchell County, N. C.

Both samples are magnetite.

[Collected by J. K. Procter. Analyzed by T. M. Chatard.] t

E. F. !

Si02 .......................................... 25.27 27.65

Fe............................................. 45.43 42.77

MnO ...... .......... ......................... .54 .59

S ........................'.... ................ .07 .08

P............................................. '.009 .007

Gr, Iron ore. Northwest part of Sevier County, Ark.

H. Manganese ore. Southwest part of Polk County, Ark. < 

[Analyses by J. Edward Whitfield.]

G. H.

Si02 .,.......................................... 12.01 4.80

Fe............................................... 42.85 11.36

Mn ............................................ 6.59 13.95

S.............................................. .11 .....

p............:................................. i.48 .....

Ti.............................................. trace .....

The manganese ore contains little dioxide.

I. Two samples iron ore, from Atalla, Ala.: a, from outcrops; ft, 250 

feet below surface.

[Analyses by R. B. Kiggs, as called for.]

A. B.

Fe.............................................. 57.52 7.75

CaO............................................ 1.38 47.64

COs ............................................ '.30 34.90
MISCELLANEOUS. ANALYSES. 87

J, Iron ore. Farm of C. J. Garrison, Buss County, Tex.

[Analysis by J. Edward Whitfield.]

Si02 :. ..........................

Fe .............................

S.. .............................

P...............................

......................... 14.53

......................... 48.56

......................... .41

......................... .405

COALS.

A. Lignite. Near light-house, Gay Head, Martha's Vineyard, Mass.

[Collected by N. S. Shaler. Analysis by J. Edward Whitfleld.] 

, Moisture.................................................. 10.25

Volatile hydrocarbons..................................... 43.09

Fixed carbon ............................'................. 34.90

Ash ...................................................... 11.76

100.00

Ash red. Coal burns well, but is very friable.

B. McNew coal bank, Powell's Mountain, Scott County, Va.

C. Horton mine, south side Powell's Mountain, near base, Scott 

County, Ya.

D. Bear-pen branch, Chimney Eock fork' of Stony Creek, Scott County, 

Va.

E. Hogan's cannel coal. East fork of Staunton Creek, Scott County, 

Va.

F. Coke from C.

[Collected by J. R. Procter. Analyses k, C, D, E, by F. W. Clarke; F, by W. F. Hillebrand.]

Ash

'Coke .........................

A oh

G. Burnet County, Tex.

[Anal

Ash ...................

B. 

1.92 

33. 42 

55.62 

9.04

100. 00 

Good 

Eeddish

yeis by J. I

C. 

1.19 

33. 74

. 58.92 

6.15

100. 00 

. Good 

Eeddish

Jdward AVhitl

D.

1.29 

30.36 

63.27

5.08

100. 00 

Good

ield.] '

E.

.39 

37.15 

42.05 

20.41

100. 00 

Good S... 

...... P..

3 79

..... 42 27

. .... 39.41

..... 14.60

F. 

.35

91.36

8.2"9

100. 00 

.68 

.034

100.00

Ash, dark gray. Coke poor, dark, and friable.

IRON AND STEEL. 

[Two samples, analyzed by J. Edward AVhitfield for the Ordnance Corps, U. S. A.]

 A. Sample from aGrusou chilled cast iron armor plate, tested by the 

Italian Government at Spezia, April 20-29, 1886.

B. Hardened steel- from 43-cm. Krupp shell, fired at Gruson plate 

"A," April 29, 1886.
WASHINGTON LABORATORY. [BULt. 55.

A. 

Fe...................................... 93.91

Mn ...................................

Ni+Co ...............................

Al....................................

Ca....................................

Si ....................................

P.....................................

S.....................................

Graphitic C...........................

Combined C ..........................

1.75

.58

trace

.20

.86

.31

.14

.81

2.04

B.

98.00

.46

.12

.38

100.60

.23 

.02 

.04 

.03

100.16

NITRE FROM UTAH.

[Analysis by T. M. Chatard.]

As found.

Insoluble..................... 12.12

H2 0 .......................... 1.24

Si02 , AUOs.................... .20

CaO .......................... -1.43

MgO.......................... trace

Na............................ .03

Cl........................... .05

S03 ........................... 2.05

K2O........................... 38.38

NagO.......................... .12

N806 .......................... 44.30

	99.92

Probable combination. 

Insoluble..................... 12.12

H2 0........

SiO2 , A1403 . NaCl .......

CaS04 .....

NaNO3 .... .

.............. 1.24

.............. .20

.............. .08

............. 3.48

.............. .33

KN03 ........................ 82.47

99.92

SALT FROM WARSAW, N. Y. 

I" Crescent Fine " brand, made from local brine. Analysis by T. M. Chatard.]

As analyzed.

HS0 .......................... 1.590.

/CaS04 . ......... .008

Insoluble} A1203 .-............ .080

(SiOB ............... .082

Si02 .... ...................... .003

AlsOs......................... .006

CaO.......................... .487

MgO ......................... .040

S03 ...... .................... .442

Cl............................ 59.370

NaaO.................. ....... 51.410

113.518

Less oxygen...... ............ 13. 380

100.138 

Needed, soda, to satisfy acids . .272

Probable combination.

................ 1.59

................ .17

................ .75

................ .45

................ .11

NaCl ......................... 97.34

100. 41

H2O..... 

Insoluble 

CaS04 ... 

CaClB ....

MgCl2 ...

100. 410
MISCELLANEOUS ANALYSES. 89

TWO CLAYS FROM SHORE OP OWEN'S LAKE, CAL.

[Collected and analyzed by T. M. Uhatard.l

Sandy clay. 

H2 0 expelled at 110°.................... 1.41

H3O expelled at red beat ................ 2.73

C02 ..................................... 8.75

Si02 .................................... 53.24

Ti02 ..

A12 03 , Fe203

FeO..

MnO..

CaO..

MgO..

Na20 

S03 .. 

Cl...

.25

10.84

2.59

.77

.10

9.18

5.82

2.64

2.06

.08

.05

Soluble in water

100.51

1.26

Blue clay.

2.05

2.40

7.24

54.92

.30

11.25

2.77

.94

.08

8.76

4.91

2.77

2.10

trace

trace

100.49

CLAY, SAND, ETC., FROM MARTHA'S VINEYARD, MASS. 

[Collected by N. S. Shaler. Partial analyses, as called for.]

A. Average sample of white clay, east end of Chilmark cliffs. 

B. Average sample of clay, north end of Gay Head cliffs. 

0. Sandy white clay, south end of Gay Head cliffs. 

D. Average sample of southernmost red clays, Gay Head. 

E. Average sample of fine white clay, south end of Gay Head cliffs. 

F. Average sample of fine clay and soil, east end of Weyquosque cliffs. 

G. Brown clay, 300 feet south of light-house, Gay Head. 

H. Average sample of red clay from the greensand, north end of 

Gay Head.

I. Average fiample of clays, Weyquosque series, Chilmark cliffs. 

J. Pyritiferous clay, central part of Gay Head section. 

K. Clay containing pyrite, west end of Chilmark cliffs.

[Analyses by F. W. Clarke.]

	A. 

Ignition........................... 3.47

Si03 ............................... 82.95

A13 03 ,Fe203 ........................ 13.45

CaO ............................... none

MgO............................... trace

Na3 0 .............................. ......

K2O .............................. ......

80s................................ ......

P2Os............................... none

B.

11.47 

49.19 

39.77 

none 

trace

C.

10.79 

56.19 

30.65 

none 

trace

..... 2.45

none none

99.87 100. 43 100. 08

D.

9.83

57.50

31.21

.19

.20

c

' I

none

99.33

E.

6.36

73.46

19.06

none

trace

.70

.73

none

none

100. 31
90 WASHINGTON LABORATOEY. [BULL. 55.

Ignition...... ...... .... ....

SiOa...... ..................

Al2 03,Fe2 03 ... ..............

CaO........................

MgO .......................

Na 0

KaO ........................

S03 ... ......................

P206 .... .....................

F.

.............. 3.39

.............. 70.81

.............. 20.67

. ............. trace

.............. 1.99

1.23

.............. 1.67

...... ........ none

G.

7.57

56.62

31.24

trace

1.97

.40

' 2. 76

none

H.

9.98

55.93

33.51

none

.19

none

I.

5.76

61.76

25.35

.51

1.95

1.83

3.01

trace

J.

5.69

72.74

21.46

none

trace

none

99.76 100.56 99.61 100.17 99.89

0 K.

SiOs ...................................................... 47.76

Al203 ,Fe203 ............................................... 30.93

FeSs-..................................................... 7.27

SO3 ....................................................... .43

CaO...................................................... none

MgO ..............................................;...... .38

KaO...................................................... 1.17

Na.?0 ..................................................... nndet

H20 ...................................................... undet

P2O5 ...................................................... trace

L. Average sample of phosphatic nodules from the greensand, north

end of Gay Head cliff.

M. Average sarnpfe of fossil bones, Gay Head. \ 

N. Greensand, northernmost exposure, Gay Head. 

O. Greensand, north end of Gay Head. 

P. Average sample Of white sand, Gay Head section.

[Partial analyses by E. B. Riggs.]

Si02 .. 

A12 03 - 

Fe2 03 . 

CaO.. 

MgO . 

Na20. 

K2O.. 

C02 .. 

P206 ..

L.

17.82

25.73

undet. . 15 <

2.60

23.88

M.

27.21

.56 

.97

3.28

27.80

N.

1.09

.38 

3.87

.16

.48

0.

.65

.33 

4.16

.14

.22

P.

78.69

15.04

.60

trace

undet.

.19 

1.09
MISCELLANEOUS ANALYSES. 91

WATER FROM PARIS, ME.

[From a large spring on the farm of William E. Cooper. Analysis by F. W. Clarke. .Stated in

grammes per liter.]

Per cent, of

Found, total solids.

SiO^ ...... .............. ..!

S04 ........................

C03 . .......................

Cl ...... ...................

K. .........................

Na .........'................

Ca ...... ...... .............

Mg...... ...................

Fe .........................

H (bicarbonate) ............

... 0.0170

... .3696

... .0754

trace

... .0012

... .0262

. . . . 1357

. . . . 0158

. 0021

.0008

2.64

57.41

11.71

.19

4.07

21.08

2.45

.12

Hypothetical combination.

SiO ............

K2SO< .....'.....

Na2S04 .... .....

CaS04 .- ........

CaH2 (CO3 ).2 .....

MgH,(C03 )3 ....

MgC03 .... ....

FeH2 (C03 )2 .....

0.0 L70

.0027

.0809

.4440

.0206

.0391

. 0328

.0067

0. 6438

0.6438 100.00

WATERS FROM SAVANNAH, GA.

[Partial analyses by E. B. Eiggs. Stated in parts per million.] 

A. Savannah Eiver, taken at high water, August 17, 1886. 

B. Savannah JRiver, taken at low water, August 17,1886. 

0. Artesian well adjoining water-works.

Cl..............

Free NH3 .......

Albuminoid NH3 

Inorganic solids . Organic solids ...

A.

trace

none

2.6

45.0

22.0

B.

trace

none

1.0

40.0

15.0

C.

7.3 

none 

none 

174.0

The inorganic solids in 0 consist mostly of carbonates.

ARTESIAN WELLS. IN GEORGIA AND ALABAMA.

[Partial analyses by K. B. Eiggs. Stated in parts per million.]

A. At Albany, Ga. 

B. At Smithville, Ga. 

0. At Americus, Ga. 

D. At Montezuma, Ga. 

E. At Fitzpatrick's, Ala.

CO, ........

S03 .. .......

Si03 ........

AlgOs. ......

CaO. ........

MgO .... ...

Examined with 

lies undetermined

A. B. C. 

.............. 181.0 140.0 177.0

.............. 96.5 65.0 74.0

.............. 9.2 17.1 5.6

.............. 27.0 13.0 43.6

.............. 21.8 6.4 48.4

.............. 1.2 . .2 .5

reference to use in steam-boilers.

D. E.

111.5 271.0

42. 0 93. 0

6. 3 38.6

26.2 40. 8

trace 2.4

11.2 19.8

.14 1.6

Chlorides and alka:
92 WASHINGTON LABORATORY. 

WATERS FROM ARKANSAS.

A. Happy Hollow Spring, Hot Springs.

[ Analysis by B. B. Riggs. Stated in grammes per liter. 1

[BULL. 55.

Found.

C03 ...-....-.°.i ........ .0081

Cl ................. .... .0030

Ca..................... .0017

'Na(K)...... ........... .0031

Si02 ...... ............. .0052

Al2O3 ,Fe2 03 ............ .0008

H2 (bicarbonate) ....... .0001

C02, free............... .0220

Hypothetical combination. 

NaCl............................. .0049

NaHCO3 .......................... .0043

CaH2 (C03 )2 ..............'...'...... .0068

SiO,.............................. .0052

A1203 , Fe203 ...................... .0008

C02 , free

.0440

.0220

.0220

.0440

B. Water of " Potash Sulphur Springs," 8 miles southeast of Hot 

Springs, Garland County.

[Partial analysis by F. W. Clarke on too small a supply of watfer. Stated in grammes per liter.]

Found. 

Si02 ................ ,0275

AlsOs-.............. .0020

Ca ................. .0032

Mg................. none.

H2S ................ none.

K.................. .0227

Na...... ........... .2216

Cl...... ........... .0405

S04 ................ .2027

Per cent, of 

total solids.

4.13 StOs 

.30

.48

. 5202

C03 by difference. .. .1458

3.41

33.28

6.08

30.43

21.89

Hypothetica]. combination.

................... .0275

A1.2O3 ....................... .0020

CaC03 ....................... .0080 '

................... .2572

................... .2988

NaCl....................... .0328

KC1........................ .0433

.6706

100.69 per cent.

.6600 100. 00

WATER FROM A SPRING NEAR FORT WINGATE, N. MEX.

[Analysis by F. "W. Clarke. Stated in grammes per liter.]

 Found. 

SiO*................ .0160

K...... ............ .0024

Na ...... ........... .0156

Ca.......... ....... .1350

Mg................. .0361

CL................. .0066

C03 ................ .2127

SO<...... .......... .282-2

H3 (bicarbonate).... .0026

Per cent, of 

total solids.

2.25

.35

2.20

19.03

5.09

.93

29.99

39.79

.37

Hypothetical combination.

SiOs ........................ .0160

KC1........................ .0046

NaCl....................... .0072

Na2S04 ........ ............ .0395

CaSO, ...... ............... .3620

CaHs(C03 ) 3 .... - .-......... .1153

MgH8 (C03 )3 ................ .0900

MgC03 ..................... .0746

.7092

.7092 100.00
MISCELLANEOUS ANALYSES 93

WATER FROM OWEN'S LAKE, CALIFORNIA.

[Analysis by T. M. Chatard. Stated in grammes per kilo. Sp. gr. 106246, 16».5.]

	Per cent, of 

Found. total solids.

Na ................ 26/837 36.95

K...... ........... 1.548 2.13

A1203 ..........'.... .023 .04

Fe2 03 .............. .013 .02

Ca ................ .014 .02

Mg................ .005 .01

SO,................ 7.060 9.71

01................. 18.215 25.07

Br, I, H2S.......... none ......

C03 ............... 18.266 25.15

B407 .-.. ...... .... .338 .47

Si08 ............... .262 .36

H2 ( bicarbonate)... ,050 .07

72.631 100.00

Hypothetical combination. 

KCI....................... 2.957

NaCl...................... 27.694

.. ................ 10.443

-................. .438

NaaSiOa................... .464

Na2C03 .................... 26.319

NaHC03 .................. 4.233

CaCC-3 .................... .035

MgCO3 .................... .013

A1S03 ...................... ..023

Fe2 03 ..................... .013

72.632

INDEX.

A. Page.

Albany,Ga., water from..................... 91

Alexander County, N. C., mica from ........ 13

tourmaline from.. 28

Alien County, Ky., meteorite from.......... 64

American Eagle Mine, Utah, minerals from. 38

Amoricus, Ga., water from ................. 91

Antlerite................................... 55

Antler Mine, Ariz., mineral from........... 54

Artesian well waters....................... 91

Atalla, Ala., iron ore from.................. 86

Auburn, Me., alteration product from ...... 25

mica from .................... 16

tourmaline from............. 23

Axinite.................................... CO

B.

Baltimore, Md., mica from.......

Bergen Hill, N. J., datolito from. 

Beryl...........................

Biotite..........................

Brazil, 'tourmalines from ........

Brochantite.....................

...... 14

..... 59

..... 16

..... 16

..... 2o'

..... 46

Burnet County, Te'x., coal from ............ 87

Butte, Mont., mineral from ................. 53

C. 

California,rocks from.........*............ 84

Chalcophyllite............................. 43

Chatard, T. M., analyses by. ....83,84,86,88, 89,93

Church Mountain Mine, Va.,ore from...... 85

Clarke, F. W., analyses by...13,14,15,17,18,80,86,

87, 89, 91, 92

studies in the mica groups .. 13 

Clays, analyses of.......................... 89, 90

Clinoclaflite............................... . 43

Coals, analyses of .......................... 87

Colemanito................................. 56

Cornwall, axinito from ..................... 60

Curry County, Oregon, pricoite from ....... 58

Cyrtolito?.................................. 52

D.

Danburite................................. 60

Datolite.................................... 59

Dauphiny, axinite from .................... 61

Death Valley, Gal., colemanitefrom ........ 56

Defiance, Ohio, limestone near.............. 80

De Kalb, N. Y., tourmaline from............ 26

Delaware, feldspars from................... 79

Devil's Head Mountain,Colo., minerals from 48 

Diller, J. S., microscopic notes by.. 13,15,18,28,36,53

E.

Erinite. 40

P.-

Feldspars.................................. 79

Fitzpatrick's, Ala., water from ............. 91

Flow of solids.............................. 67

Fort Wingate, N. Mex., water from......... 92

G.

Gay Head, Mass., clays, etc., from.......... 89

lignite from.............. 87

Gouverneur, N. T., tourmaline from ....... 26

Greylock Mountain, Mass., feldspar from .. 79

H. .

Haddam, Conn., tourmaline from ........... 29

Hallock, William, on flow of solids......... 67

Hamburgh, N. J., tourmaline from ......... 26

Hancock, Md.,sandstone from............. 80

Hebron, Mo., mineral from................. 25

Hillebrand,W. F.,analysis by.............. 40,41,

45, 49, 52, 53, 54, 55, 82, 84, 87

copper minerals from 

, Utah.................. 38

mineralogical notes ...... 48 

Hisingerito................................ 14

Hoosac Tunnel, feldspar from.............. 79

Hot Springs, Ark., waters from near....'... 92

I.

Iron, analysis of ........................... 88

Iron mica................................. 16,17

Iron ores..................................85,86, 87

J. 

Johnson County, Ark., meteorite from..... 63

L.

Lepidomelane.............

Limestone ................

Litchfield, Me., mica from. 

Ludwigite................

14,15

80

15

59

M. 

Mammoth Mine, Utah, minerals from......

Manganese ores............................

95

38
96 INDEX.

Page. 

Martha's, Vineyard,clays,etc., from....... 89,90

lignite from........... 87

Menomonee River, rocks from ...:........

Mica group................................

MitchellCounty, N. C.,iron ores from......

Mixite.....................................

Monroe, Conn., tourmaline from............

Montana, rocks from ......................

Montezuma, Ga., -water fvom ...............

Morawitza, lud wigite from .................

Muscovite.................................

N.

Nantic Gulf, tourmaline from. 

Nitre .........................

28

0.

Olivenite .................................. 39

Orford, N. H., tourmaline from............. 27

Owen's Lake, Gal., clays from ............. 89

. water from......... ... 93

P. 

Pandermite................................ 58

Paris, Me., tourmaline from ................ 24

water from...................... 91

Pearce, R., analyses \>y............... 40, 41,45, 53

Pharmacosiderite .......................... . 40

Pierrepont, X. Y., tourmaline from ......... 28

Pigeon Point, Minn., rocks from............ 81

Polk County, Ark,, ore from ............... 8C

Priccite.............. '..........^........... 58

 R.

Rhodes's Marsh, Xev., ulexite from........ 58

Riggs, R. B., analyses by ................... 24, 25,

2(5, 27, 2K, 29, 30.79, 80, 81, 

82, 83, 84, 86, 90, 01, 92 

19 

54 

23 

87 

GO

on tourmaline.................

Rose Mine, X. Mex., mineral from ..........

Rnmfonl, Me., tourmaline from ............

R.USS County, Tex., iron ore from..........

Russell, N. Y., danburitefrom..............

Salt......................................

Samarskite...............................

Sandstone ...............................

Savannah, Ga., waters from ..............

Scorodito .................................

Scott County, Va., coals from ............

Sevier County, Ark.,iron, ore from.......

Smithville, Ga., water from .............

Solids, behavior under pressure ..........

Spotsylvania County, Va., iron ore from , Steel, analyses of.........................

Stony Point, N. C., mica from ...........

tourmaline from......

T.

Tin tic district, Utah, minerals from . Titanic oxide, new form of.........

Tourmaline........................

Tyrolite ...........................

U.

Ulexite .............

Utah, minerals from 

nitre from ....

88

48

80

91

65

87

86

91

75

85

88

13

28

38

36

19

41

W.

Warsaw, JT. Y., salt from .................. 88

'Washington, H. S., colemanite . ........... 57

copper minerals........ 38

Whitfleld, J. E., analyses by................ 57, 58,

59, CO, 61, 63, 64, 65, 80, 82, 85, 86, 87

on boratesanclborosilicates 56

meteorites.............. 63

scorodite............... 65

Wilmington, Del., feldspar from............ 80

Winslow,Me., beryl from ..... ............ 53

Wise County, Va., iron ore from ........... 86

Y.

Yellowstone Park, scorodite from , 65