DEPARTMENT OF THE INTERIOR

OF THE

UNITED STATES

GEOLOGICAL SURVEY

VOL. VIII

WASHINGTON

GOVERNMENT FEINTING OFFICE 

1889

CONTENTS.

BULLETIN No. 47.

47. Analyses of Waters of the Yellowstone National Park, with an Account of the 

Methods of Analysis employed, by Frank Austin Gooch and James Edward Whitfield.

BULLETIN No. 48.

48. On the Form and Position of the Sea Level, by Robert Simpson Woodward.

BULLETIN No. 49.

49. Latitudes and Longitudes of Certain Points in Missouri, Kansas, and New 

Mexico, by Robert Simpson Woodward.

' BULLETIN No. 50.

50. Formulas and Tables to facilitate the Construction and Use of Maps, by Rob- > 

ert Simpson Woodward.

BULLETIN No. 51.

51. On Invertebrate Fossils from the Pacific Coast, by Charles Abiathar White.

BULLETIN No. 52.

52. Subaerial Decay of Rocks and Origin of the Red Color of Certain Formations, 

by Israel Cook Russell.

BULLETIN No. 53.

53. The Geology of Nantucket, by Nathaniel Southgate Shaler.

BULLETIN No. 54.

54. A Report on the Thermo-Electrical Measurement of High Temperatures, by 

Carl Barus. '

m

184340

ILLUSTRATIONS.

BULLETIN No. 47.

Page. 

FIG. 1. Apparatus for the estimation of carbonic acid........................ 16

2. Apparatus.for the estimation of boric acid............................ 18

BULLETIN No. 51.

PLATE I. Ostrea Dilleri.................................................... 74

II. Ostrea Dilleri.................................................. 76

III. Fulguraria Gabbi, Fulgur Hilgardi, Trophon Condoni, Cancellaria Turneri, Gyrodes Dowelli, Rimella macilenta, Ceratia 

nexilia ...................................................... 78

IV. Scobinella Dilleri, Cominella LeContei, Mesalia obsuta, Trochus 

(Anadema) gemiferas, Stomatia obstricta, Fauntis marcidulus, 

Lysis oppansus, Actaeon inornatus, Vasculum obliquum, Zirphsea plana.................................................. 80

V. Ammonites Turneri............................................ 82

VI. Anatina sulcatina ?, Crassatella tuscana, Clisocolus dubius, C.

cordatus..................................................... 84

VII. Perna excavata, Ammonites Maclurei, Vanikoropsis suciensis.. . 86

VIII. Teredo pugetensis ............................................. 88

I.. Batissa Newberryi, Cardium ?, Cerithium ? ? ..... 90

X. Sanguinolaria ? caudata, Psaiumobia obscura, Cyrena brevidens,

Neritiua 1............................................. 92

XI. Batissa dubia, Corbicula Willisi, C. pugetensis. ................ 94

XII. Ammonites Howelli............................................ 96

XIII. Ammonites Whiteavesi,.Belemnites ?, A. kialagvikensis... 98

XIV. Ammonites Howelli, Belemnites ?, Cucnlltea iucrebescens,

Glycimeris? Dalli ........................................... 100

BULLETIN No. 52.

PLATE I. View of Mount Mitchell, North Carolina; looking north along the

crest of the Black Mountains. Roan Mountain in the distance. 16

II. New Found Mountains; lookiug southwest from Asheville N. C.. 20

III. View of fields of residual clay, near Natural Bridge, Virginia;

looking north. House Mountains in the background.......... 26

IV. Mayo River, North Carolina; illustrating the manner in which 

the rivers of the Piedmont region are eroding their beds. The 

rocks producing the rapids are Newark sandstones............. 34

V. View from Harper's Ferry, W. Va., looking down the Potomac; to 

illustrate the manner in which the rivers of the Appalachians 

are eroding their beds........................................ 36
VI ILLUSTRATIONS.

BULLETIN No. 53.

Page.

PLATE I. Geological map of Nantucket Island .........................Frontispiece

II. Aspect of katne moraine on the northern border, near Shemo Point.: 16

III. Kame valley, with dome-shaped hill, looking south, on north road,

near Shemo Point................................................ 18

IV. Topography of kaine moraine in central district, near north end of

Long Pond, looking north ................................. ...... 20

V. East branch of Hummock Pond, looking south..................... 22

VI. Junction of kame moraine and terrace plain on Gibba Pond; Siasconset in distance................................................... 26

VII. Sankaty Head, looking north from a point 150 yards south of lighthouse ........................................................... 30

VIII. Vie w of coast escarpment 500 yards north of Sankaty light......... 40

I.. Aspect of north shore from near upper end of Long Pond, looking east. 46 

X. Split pebbles, resembling stone implements........................ 50

FIG. 1. Diagrammatic horizontal section of small spit on Coatue Beach..... 13

2. Diagrammatic section through Coatue. Beach....................... 15

3. Generalized section of Squam Head ..................-.............. 16

4. Section at Weewocket............................................. 16

5. Section of border of Lily Pond .................................... 16

6. Section fro nJ Coatue Bay to the ocean..... ...................... 17

7. Diagrammatic section across valleys in sunken plain ............... 20

8. Diagrammatic section showing positions of bowlders on surface of

glacial plain near Gibbs'Pond ................................... 21

9. Section of submerged swamp on north shore........................ 28

10. Section at Sankaty Head.............................'............. 32

11. Diagrammatic section of beds at Sankaty Head .................... 39

12. Section 500 yards south of beds at Sankaty Head................... 41

13. Section showing apparent beach line, near Gibbs Pond............. 45

14. Kames east of Nantucket. village..................... ............ 45

15. Section of shore east of Surf Side, showing beginning of coast apron. 50

16. Profile across Great Head, showing dunes .... ... ... .... 51

BULLETIN No. 54.

FIG. 0. Disposition of apparatus for air thermometry and boiling point. Frontispiece

1. Apparatus for constant temperature between 0° and 100°........... 59

2. Apparatus for constant temperature between 100° and 300°......... 60

3. Boiling-point apparatus for mercury............................... 61

4. Boiling-point apparatus for zinc;. earlier form...................... 63

5. Boiling-point apparatus for zinc; later form; longitudinal section.. 65

6. Boiling-point apparatus for zinc; later form; cross-section......... 66

7. Boiling-point tube for mercury; original form...................... 84

8. Boiling-point tube for sulphur; original form ...................... 85

9. Boiling-point tube for water, etc.; original form.................... 86

10. Boiling-point tube; perfected form ................................ 87

lOo. Boiling-point tube for annealing long wires ........................ 87

11. Boiling-point tube for pressure work................................ 88

llo. Boiling-point tube for pressure work with accessories .............. 88

12. Eing burner ...................................................... 89

13. Original form of boiling-point crucible ............................ 91

14. Perfected form of boiling-point crucible............................ 92

14a. Boiling-point crucible for pressure work ........................... 94

15. Boiling-point crucible with open tube.............................. 94

16. Machine for pressing porcelain insulators .......................... 96
ILLUSTRATIONS. VII

Page. 

FIG. 17. Die for porcelain tubes ............................................ 96

18. Disposition of thermo-electric apparatus ........................... 97

19. Double key ....................................................... 97

20. Standard Daniell cell.......................................... ... 100

21. Chart showing the relation of temperature and electromotive force;

thermo-couples Nos. 17 and 18...... ..... ............ ...... ...... 114

22. Chart showing the relation of temperature and electromotive force;

thermo-coupley Nos. 22, 35, 36, 37, 38, 39, 40...................... 116

23. Apparatus for melting point of platinum........................... 124

24. Resistometer....................................................... 132

25. Detached rider .................................................... 132

26. Chart showing the relation between electrical resistance and temperature coefficient of platinum alloys .............................. 150

27. Chart showing the relation between electrical conductivity and temperature coefficient of platinum alloys ........................... 162

28. Tubular displacement air thermometer............................. 166

29. (Withdrawn.)

30. Diagram of Jolly air thermometer and bulb ........................ 168

31. Non-inglazed, spherical air thermometer bulb...................... 172

32. Non-inglazed, reentrant air thermometer bulb...................... 173

33. Inglazed, spherical air thermometer bulb .......................... 174

34. Machine for soldering porcelain; elevation......................... 175

35. Machine for soldering porcelain; plan ............................. 176

35a. Gasometers ..........................................'............. 179

36. Revolving muffle; diagram........................................ 181

36a. Elliptic revolving muffle; diagram ................................ 181

37. Revol ving muffle and furnace; longitudinal section ................ 182

38. Revolving muffle and furnace; plan ............................... 184

39. Temperature and electromotive force of thermo-couples in corresponding time series............................................. 202

40. Constant pressure air thermometer............. ...... .......... .... 209

41. Chart showing the variation of thermo-electromotive force with temperature ........................................................ 226

42. Chart showing the variation of thermo-electromotive force with ternperature ........................................................ 228

43. General disposition of apparatus for viscosity measurement......... 243

44. Diagram of receiver for distributing pressure ...................... 246

45. Side elevation of the capillary apparatus........................... 247

46. Plan of the capillary apparatus.................................... 248

47. Vertical section through helix ..................................... 258

47a. Plan of helix and thermo-couples .................................. 264

48. Chart showing viscosity as a function of temperature............... 264

49.

50.

51. ^ Diagram of practical transpiration pyrometers .................... 303

52.

53.

54. Chart showing the relation .between apparent viscosity and pressure. 304

55. Disposition of apparatus for differential measurements.............. 305

DEPARTMENT OF THE INTERIOR

BULLETIN

OF THE

GEOLOGICAL SURVEY

No. 47

WASHINGTON

GOVERNMENT FEINTING OFFICE

1888

UNITED STATES GEOLOGICAL SUEVEY

J. W. POWELL, DIKECTOK

ANALYSES OF WATERS

OF THE

YELLOWSTONE NATIONAL PARE

WITH AN ACCOUNT OF THE METHODS OF ANALYSIS EMPLOYED

BY

FKANK AUSTIN GOOCH

AND

WASHINGTON

GOVERNMENT PRINTING OFFICE

1888

CONTENTS.

Page.

"Letter of transmittal........................................................ 7

Introduction................................................................ 9

'Operations in the field ...................................................... 10

Operations in the laboratory................................................. 11

Treatment of natural waters ................................................ 12

Specific gravity .................... ................................. 12

Hydrogen sulphide and free sulphur..................................... 13

Sulphurous acid.... ...................................... . «.-« ' 13

Sulphuric acid.......................................................... 13

Nitric and nitrous acids................................................. 14

Carbonic acid........................................................... 15

Arsenious acid and boric acid............................ .......... 17

Chlorine (with bromine and iodine)...................................... 20

Silica, iron and aluminum, calcium, and magnesium ..................... 21

Sodium, potassium, and lithium......................................... 22

Ammonia and albuminoid ammonia...................................... 25

Treatment of concentrated wafers ........................................... 25

Strength of the concentrated waters.............. . .................... 25

Treatment of the residue................................................ 26

Fluorine................................................................ 26

Barium and strontium .................................................. 26

Phosphoric acid......................................................... 27

Manganese.............................................................. 27

Iron.................................................................... 28

Titanic acid.............................................................. 28

Treatment of the aqueous solution........................................... 29

Iodine and bromine...... ............................................. 29

Lithium ........................................................_...... 30

Csesium, rubidium, and thallium ........................................ 31

Arsenic, antimony, tin, copper, and lead................. . ...... ..J..... 31

Boric acid.............................................................. 33

Statement of the results of analysis.................... 00 .................... 33

Analyses................................................. 0 .................. 36

Cleopatra Spring ....................................................... 36

Orange Spring......................'.................................... 38

HotRiver .............................................................. ' 39

Gardiner River ......................................................... 40

'GardinerRiver............ .............................................. 41

Water supply at Mammoth Hot Springs.................................. 42

Soda Spring ..................... ..................... ............ 43

Fearless Geyser.......-........-..........'.............................. 44

Pearl Geyser............................................................ 46

Constant Geyser ............f........................................... 48

Coral Spring........................................................._ 49

(5) 5
6 CONTENTS.

Page* 

Analyses Continued.

Coral Spring....;..............._..................................... 50

Echinus Spring ................. .......................................... 51

SchlammkesseL...................................._............. _... 52

Fountain Geyser........................................................ 53

Great Fountain Geyser.................................................. 54

Hygeia Spring........................................................... 55

Madison Spring..........................*,.............................. 56*

FireholeRiver .......................... ............................. 57

Excelsior Geyser........................................................ 58-

OldFaithful Geyser.....................................................v 60

Splendid Geyser ......................................................... 62"

Splendid Geyser......................................................... 64

Giantess Geyser.......................................................... 65

Beehive Geyser .... ................................................. 66

Grotto Geyser........................................................... 67

Turban and Grand Geysers......'....................................'.... 68

Artemisia Geyser ......................................................... 69*

Taurus Geyser.......................................................... 70

Asta Spring.......... ................................................ 71

Bench Spring........................................................... 72

Firehole River.......................................................... 7$

Yellowstone Lake....................................................... 74

Alum Creek............................................................. 75-

Chrome Spring.......................................................... 76

Mush Pot Spring........................................................ 78

Devil's Ink Pot.......................................................... 80

Soda Butte Spring...................................................... 81

Summary of analyses........................................................ 82

Index ...................................................................... 83

ILLUSTRATIONS.

Page. 

FlG. 1. Apparatus for the estimation of carbonic acid........................... 16

2. Apparatus for the estimation of boric acid .............................. Id

(6)
LETTER OF TRANSMITTAL.

DEPARTMENT OF THE INTERIOR, 

IT. S. GEOLOGICAL SURVEY, DIVISION OF CHEMISTRY,

Washington, D. C., April 26,1887.

SIR : I have the honor to transmit for publication as a bulletin of 

the Survey a paper entitled "Analyses of waters of the Yellowstoue 

National Park, with an account of the methods of analysis employed," 

by Frank Austin Gooch and James Edward Whitfield. It represents 

work done in the Chemical Laboratory of the Survey and it is an exceedingly valuable contribution to science. 

Yery respectfully,

F. W. CLARKE,

Chief Chemist. 

Maj. J. W. POWELL,

Director U. 8. Geological Survey, Washington, D. C.

(7) 7

ANALYSES OF WATEES OF THE YELLOWSTONE 

NATIONAL PARK

BY F. A. GOOCH AND J. E. WHITFIELD.

INTRODUCTION,

The series of waters forty-three in all of which it is the purpose of 

this paper to give some account comprises typical representatives of 

the geysers, hot springs, mud springs, cold springs, and surface waters found within the limits of the Yellowstone Park. It embraces 

collections made during the field seasons from 1883 to 1886 under the 

direction of Mr. Arnold Hague, geologist in charge of the Yellowstone 

Park Division, and submitted to us for analysis. In our account we 

have to deal simply with the results of analysis and with the analyti. 

cal processes we have used with the latter on the ground that some 

knowledge of the methods employed in the examination and of the 

quantities of material at our disposal is essential to a correct understanding of the meaning and value of the analyses themselves. Discussions of the broader chemical aspects of the problems which are involved in a thorough consideration of the relations of these waters, of 

correlative matters of geological interest, and of the physical phenomena belong properly to others.

The difficulties in the way of collecting and transporting large quantities of water in a region comparatively inaccessible were such that the 

number of large samples, for the more complete analyses, was restricted 

to a half-dozen; but, though at the beginning of the examination it was 

supposed that a partial analysis, such as might be made with smaller 

amounts of material, must suffice, it happened, fortunately, that the 

development of certain methods as the work progressed has so far extended the reach of the analyses of the smaller samples that from them 

it is possible to deduce results of fair accuracy, and, if such elements 

be left out of consideration as are shown by the more elaborate analysis 

to be present either not at all or only as traces in closely comparable 

waters, nearly as comprehensive results as those drawn from the examination of the larger samples.

(9) 9
10 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47, 

OPERATIONS IN THE FIELD.

The examination of the waters was necessarily confined in the field 

to a very few points. Note was made of the clearness or turbidity, the 

reaction to litmus and turmeric, the temperature, and the presence or 

absence of hydrogen sulphide. The tests for the last were the sense of 

smell and the action of the water upon a polished silver blade.

The operations of collecting and preparing the samples for transportation were carried out as simply as possible. The .water was bottled in 

boxed demijohns when it was possible, and otherwise in beer bottles^ 

In every case great care was taken to clean the receptacle thoroughly 

and rinse before bottling with some of the water to be examined. In 

the greater number of cases the waters were so marvelously clear that 

filtration was entirely superfluous. When, however, the need and opportunity occurred the waters were filtered previous to bottling. All 

samples were corked tightly and sealed hermetically.

The size of the sample varied from a half liter to one hundred liters, 

according to the purpose for which it was taken; but the great bulk of 

the largest samples was, in every case excepting one, reduced greatly 

by the evaporation of the main portion of the sample previous to bottling. In the one exceptional case the sample was taken for the specific: 

purpose of examining it as to its contents in the heavy metals, and was 

kept for subsequent reduction in porcelain in the laboratory, in order 

that the danger of contamination by the tin or copper of the tin-lined 

still which was employed to effect the reduction in the field might be 

precluded. No attempt was made to fix with more than a rough approximation the quantities of water evaporated. The concentrated 

waters, with the rinsings of the still in the natural water of the charge- 

(such portions of the residue as adhered to the walls of the vessel having been dislodged as completely as possible by gentle friction with a. 

rubber or the ball of the finger), were carefully bottled and sealed, and 

the determination of the degree of concentration was left to be effected 

in the laboratory in a manner to be described later. A portion of the 

water represented by the concentrated sample was always reserved in 

the natural condition for examination.

For the determination of hydrogen sulphide special samples of from 

600 cm3, to 700 cm3, were generally taken, and to each, if the water did 

not carry free sulphur, was added before corking and sealing a small 

amount of lead acetate in crystals. Doubtless it might have been well 

to fix the hydrogen sulphide similarly in the case of waters carrying 

free sulphur, having first separated this by filtration ; but on the few 

occasions when that need arose the means of removing the sulphur 

were not at hand. In these cases, therefore, the samples were simply 

bottled and sealed with care, and kept for examination in the laboratory.

Nearly all the waters examined were hot when the samples were

(10)
OOOCH AND WHITFIELD.] METHODS OF ANALYSIS. 11

taken and not surcharged with carbonic acid. It was considered unnecessary, therefore, under the circumstances, to take a special samplefor the determination of the carbonic acid and treat it in the field so» 

as to fix that gas in insoluble form, but for this estimation reliance was 

placed upon the general sample which, as has been said, was corked 

and sealed with great care.

OPERATIONS IN THE LABORATORY.

The operations in the laboratory comprised the determination of thespecific gravity of the waters and, in the concentrated samples at handj> 

the estimation of the following substances:

* Silicic acid. Iodine. Barium.

Titanic acid. Fluorine. Strontium.

* Sulphuric acid. * Sulphur. . * Calcium.

Sulphurous acid. * Hydrogen sulphide. * Magnesium.

* Carbonic acid. Copper. Caesium.

Nitric acid. Lead. Rubidium.

Nitrous acid. * Arsenic. * Potassium.

Phosphoric acid. Antimony. * Sodium.

* Boric acid. * Iron. * Lithium.

" Chlorine. * Aluminum. * Ammonia.

Bromine. Manganese. * Albuminoid ammonia.

In analyses for which the natural water alone was available thosesubstances only were sought which are marked in the table with an 

asterisk (*).

The determination of what is known as the total residue, the amount 

of solid matter left upon evaporating a known amount of water, i& 

usually regarded as desirable, if for no other reason than to serve as a 

control of the summation of the determinations of the individual constituents : but the complexity of these waters and the relations of the 

combined salts are such that it is riot possible to arrive at the same end 

in two successive treatments by evaporation and desiccation of the, 

residue. The action of free silica, which is an abundant constituent of 

the waters, is to set free during the process carbonic acid from the carbonates and boric acid from the borates; to magnify the tendency of 

the chlorides of calcium, magnesium, and lithium to exchange chlorine 

for oxygen, and, if the temperatures be pushed sufficiently high, ta 

dehydrate the silica and to volatilize sulphuric acid. Furthermore, the 

extent of such action is variable and indeterminate. There is obvious 

reason, therefore, for the difficulty which we experienced in obtaining 

residues of constant composition; and similar obstacles, as we found 

practically, oppose the attempt to reduce the residue to a definite con 

dition by evaporation and ignition with sulphuric acid in excess. By 

means of no device which occurred to us (and several lines of experimentation which need not be mentioned here were followed) were we 

able to apply, in any form, this general method of control. The proof

(11)
12 WATERS OP YELLOWSTONE NATIONAL PARK. [BULL. 47.

of the accuracy of our analytical work rests, therefore, upon the agreement of duplicate determinations.

For convenience in the matter of arrangement, we describe first those 

methods of analysis which were applied to waters in the natural condition ; and the account of the treatment of concentrated waters follows. 

Methods for the determination of certain substances are described under 

both heads. For when the entire work was done upon the natural 

water the mode of examination was sometimes made, of necessity, by 

processes different from those which were applied in the examination of 

concentrated water; and under reversed conditions the 'converse was 

true. In some of the earlier analyses methods were employed which 

later experience taught us might be advantageously replaced by processes which were developed subsequently. In the account of the 

methods employed all of these are placed under the proper head; and 

in the statement of analyses mention is made, when there might be 

doubt, of the particular method adopted.

TREATMENT OF NATURAL WATERS.

Specific gravity. The figures which stand for the specific gravity of a 

water represent the weight of any volume of the water under consideration at 15.5° C. compared with the weight of the same volume of 

distilled water at the same temperature. The determinations were nearly 

all made with a Geissler bottle, fitted with a ground tubular stopper and

 cap, and a thermometer. In a few of the earlier determinations a bulbapparatus similar in general principle, but wanting the immersed thermometer, was employed. The temperature of the water in the bottle 

was taken immediately after the final adjustment of volume, and the 

latter was effected instantly and without handling after the filled bottle 

had been permitted to stand a few moments to bring about an equal 

distribution of temperature, When the bulb-apparatus was employed

the temperature of the water was taken before filling the bulb and after 

weighing, and the mean of the two readings was assumed to be the 

temperature of the water at the time when the volume was adjusted. 

The weight shown by the balance was taken as the weight of the water 

which would fill the apparatus at the temperature noted. The weight

 of the same volijme of the water at 15.5° 0. was calculated from the 

weight observed, upon the assumption that the co-efficient of expansion

 of the water under examination was the same as that of pure water. 

The rates of the value thus found to the value found by a similar treatment of pure water is the specific gravity at 15.5° 0. It is obvious 

that, in order that the assumption of the identity of the co-efficients of 

expansion of the water under examination and of pure water may be 

the occasion of the least error, the observed temperature must be as 

near 15.5° 0. as may be; and that the temperature of the balanceroom should be not far from the same, in order that errors which may 

arise from changes of temperature in the water during the manipula-

(12)
OOOCH AND WHITFIELD.] METHODS OF ANALYSIS. 3 $

tion, and from the establishment of air-currents in the balance-case 

may be less liable to occur. So far as we were able these sources of inaccuracy were guarded against, but the conditions under which the 

work was performed necessitated the application of corrections rather 

greater than we shouldo wish. The figures which represent the specific 

gravity in the statement of the analyses are probably riot accurate beyond the fourth decimal place.

Hydrogen sulphide and free sulphur. Hydrogen sulphide in waters 

which did not carry free sulphur was determined in the special sample 

to which lead* acetate had been added in crystals at the time of bottling. Before breaking the seal of the bottle a scratch was made upon 

the neck on the line of the meniscus of the water within, and the volume of the sample usually about 600 cm3 was determined subsequently with sufficient accuracy (the amount of hydrogen sulphide present being always trifling) by finding the volume of water necessary to 

fill the bottle to the mark, The precipitate which had been formed in 

the bottle by the addition of lead acetate was left undisturbed at first, 

and the supernatant liquid decanted as completely as possible. Them 

the precipitate was easily removed, and for the most part dissolved by 

means of a little sodium hydrate in Solution, and the solution and remaining precipitate were added to the water previously decanted. At 

this point the lead sulphide showed itself, if any was present, and 

was collected without difficulty by filtering the alkaline liquid in which 

it floated through a felt of asbestos in a perforated crucible, in themanner described by one of us previously.1 The felt and the adherent precipitate were transferred to a beaker, treated with potassium chlorate and hydrochloric acid to oxidize the sulphide, and the 

sulphuric acid thus formed was determined by precipitation as barium 

sulphate. From waters carrying free sulphur that element was separated by filtration. The residue, after washing sufficiently to remove 

the sulphates, was.treated with hydrochloric acid and potassium chlorate, and the resulting sulphuric acid was determined as barium sulphate. The filtrate from the sulphur contained the hydrogen sulphide^ 

if it was present in the sample, and this was removed by lead acetate 

and estimated in the manner described above.

Sulphurous acid. The test for sulphurous acid was made in the case 

of a few waters which did not carry more than a trace of hydric sulphide 

by titrating 200 cm3 of the water, acidified with sulphuric acid, with a 

standardized solution of potassium permanganate. In none of these 

was a reducing action found greater than was attributable to the action 

of the hydrogen sulphide and arsenic (assumed to be in the condition 

of arseuious acid) known to be present.

Sulphuric acid. The sulphuric acid was precipitated from a known

weight of water, after acidifying distinctly with hydrochloric acid and

heating to boiling by means of barium chloride. After cooling and

i Am. Chem. Jour., vol. 1, 1879, p. 317.

(13)
14 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

settling, usually after twelve hours, the supernatant liquid was decanted as completely as possible from the precipitate and passed 

through an asbestos felt in a perforated crucible. The precipitate remaining in the beaker'was boiled with a small portion of strong hydro- 

 chloric acid, and the latter was removed by evaporation on the water, 

bath. Treatment with hot acidulated water left the precipitate as pure 

as barium sulphate may be, and ready for collection upon the same felt 

through which the supernatant liquid had been poured. Thorough 

washing, ignition, and weighing completed the operation.

Nitric and nitrous adds. In examining the waters as* regards their 

contents in nitric and in nitrous acids a modification of the indigo 

method was followed. The action of these acids upon iudigo is known 

not only to be variable with the conditions of dilution, temperature, 

and the proportion of sulphuric acid added, but also to be dependent 

upon the order in which the solution of iudigo, the sulphuric acid, and 

the nitrous or nitric acid are intermixed. On this account great care 

was taken to secure uniformity of treatment of the standard solutions 

and the water under the test. For preliminary testing a portion of 

water was reduced by evaporation to a volume of 50 cm3, cooled to the 

temperature of the air, introduced into an Erlenmeyer flask, and mixed 

with an equal volume of strong sulphuric acid. To the mixture the solution of indigo was added until a distinct tinge of green became visible. In this manner the amount of the solution of indigo from which a 

given amount of the water under test would discharge the color became 

known approximately. For the exact test the portion of water, after 

evaporation and.cooling, was brought to a volume which was less than 

50 cm3, by an amount equivalent to the volume of the solution of indigo 

used in the preliminary test. To the portion thus prepared were added 

50 cm3, of strong sulphuric acid at once, and the solution of iudigo as 

rapidly as the catching of the exact point at which the tinge of green 

appeared would permit. At the instant of coloration the flask with its 

contents was placed in a bath of paraffine heated to 140° C. The volume of the solution of indigo which had been added was noted and, if 

at the end of five minutes' heating in the bath the tinge of color was 

atill visible, this volume was taken as the measure of the nitrates and 

nitrites in the water. If, on the other hand, the color vanished during 

the heating, it was reproduced by the addition of more indigo, and the 

digestion in the bath at 140° 0. was prolonged during another interval 

of five minutes.

This mode of treatment was repeated until the coloration was permanent during the interval of digestion. The total volume of the solution 

of indigo employed was recorded, and its value in terms of nitric acid 

determined in the manner to be described.

As Warrington has shown, 1 the oxidizing power of nitric acid upon 

indigo decreases as the dilution of the solution in which the action takes 

J Jour. Chem. Soc. London, 1879, p. 578. 

(14)
<SOOCHANDWHITFIELD.] .METHODS OF ANALYSIS. 15

place increases. It is plain, therefore, that in order that the exact value 

of the volume of the indigo solution employed in the test may be known, 

the amount of nitric acid needed to discharge the color from an equal 

amount of the same solution under the conditions of the test must 

be determined. To effect this determination we made use of a solution 

of potassium nitrate of known strength, and found by experiment the 

amount of it which, mixed with 50 cm3, of strong sulphuric acid, with 

water enough to bring the final volume to 100 cm3 ., and with the 

amount of the solution of indigo employed in the test, was just adequate to .discharge all color excepting the faint characteristic tinge 

which must remain unchanged after five minutes' heating. The oxidizing power of the nitrates and nitrites in the water is exactly measured 

by the amount of nitric acid in the quantity of the standard nitrate 

solution which is required to produce the end-reaction. The solution, 

of potassium nitrate which we used contained 0.0001 g. to 1 cm3. 

The mode of manipulation which we adopted keeps the proportion of 

strong sulphuric acid added to the mixture (excepting the preliminary 

tests) always the same, and consequently the heat generated in the 

reaction is the same always. The order in which the re-agents are 

brought together is the same in all cases,.and sources of inaccuracy 

due to the variability of the action of nitric acid with the degree of 

dilution are eliminated.

Carbonic acid. The greater number of the waters with which we 

have had to deal were hot when the sample was taken, and not surcharged with carbonic acid. In view of the circumstances under which 

the waters were collected it was thought that a portion of the general 

sample, which was carefully sealed, might be made to serve the purpose 

of determining the carbonic acid contained in the water, instead of portions taken specially for that end and treated in the field with a mixture of ammonia and calcium chloride to fix the carbonic acid gas. Accordingly dependence was placed upon the large general sample for this 

estimation. The presence of free silica in the waters and the complexity of composition place so great au obstacle in the Way of determining the/ree carbonic acid that the attempt to make the estimation was 

not undertaken. The method which we adopted for the determination 

of the total carbonic acid is that well-known process which rests upon 

the boiling of the acidified liquid and the absorption and weighing of 

the gas evolved. The apparatus which we employed, differing some- 

 what from that in ordinary use for this purpose, is shown in Fig. 1. 

It consisted essentially of a flask in which to boil the water, a cooler to 

return the condensed steam to the flask, a (J tube filled with anhydrous 

cupric sulphate to intercept traces of hydrochloric acid which might 

escape condensation in the cooler, a second U tube charged with calcium chloride to dry the gas, potash bulbs to retain the carbonic acid, 

and two tubes filled with calcium chloride, one of which was to retain 

moisture carried over from the potash bulbs and was weighed with

(15)
16 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

them, the other serving to protect the weighed tube from the action of 

the external air. Through the rubber stopper of the flask passed the 

tube of a separating funnel, the end of the condensing tube, and a tube 

which connected the interior of the flask with the system of bottles and 

scrubbing tower, which furnished at will and under slight pressure a. 

supply of dry air free from carbonic acid.

FIG. 1. Apparatus for the estimation of carbonic acid.

Before beginning the operation of determining the carbonic acid in » 

water the atmospheric air was expelled from the apparatus and replaced 

by pure air free from carbonic acid. The stop-cock in the funnel tube 

and the connection with the aspirator having been' closed, the water 

started through the cooler, and the joint broken between the potash^ 

bulbs and the drying tube immediately preceding it, a few cubic centimeters of distilled water were put into the flask and boiled. The steam 

generated drove the air from the flask, and that remaining in the tubes 

was swept forward by pure air admitted from the aspirator. The outer 

opening of the tube at the end of the line was closed, the source of heat 

removed, and the flask allowed to fill with air from the aspirator. The 

whole apparatus having been filled thus with air free from carbonic acid, 

the water to be examined we found 200 g. to be a convenient amount 

was introduced into the flask through the funnel tube and followed by 

a little boiled water and a sufficiency of sulphuric acid, care being taken 

to exclude the outer air during the operation. The connection between 

the line of drying tubes and the absorption bulbs was reestablished, the 

liquid in the flask was brought to the boiling point, and, to secure constant and quiet ebullition as well as to aid in transferring the carbonic 

acid from the flask to the absorption bulbs, a current of pure air was

(16)
GOOCH AND WHITFIELD.] METHODS OF ANALYSIS. 17

sent slowly through the boiling liquid which covered the end of the aspirating tube and that of the funnel tube. At the end of half an hour 

the burner was removed from under the flask and the apparatus was 

permitted to cool during another half hour, the current of air being 

kept in motion through it. The difference between the weights of the 

potash bulbs, with the drying tube which accompanies them, before and 

after the operation, was taken to be the weight of carbonic acid absorbed, and the total carbonic acid of the portion of water examined.

When the water under examination contained hydrogen sulphide, a 

little cupric sulphate was introduced before acidifying into the portion 

which was to serve for the determination of carbonic acid.

Arsenious acid and boric acid. To the portion taken for analysis 

usually 500 g. hydrochloric acid was added in distinct excess, the 

temperature of the liquid was raised to 70° 0., and the source of heat 

having been removed, hydrogen sulphide gas was introduced in a gentle

current for several hours. The precipitation of the arsenious sulphide 

began at once, but the action of the precipitant was continued to insure 

completeness. The precipitate was collected upon an asbestos felt, 

washed, and dissolved in fuming nitric acid. The solution in nitric acid 

was evaporated to dryness, the residue was dissolved in hydrochloric 

acid, and from this solution, made strongly ammoniacal but kept small 

in volume, the arsenic was precipitated by the addition of the magnesium chloride mixture and brisk agitation. The precipitated ammonium-magnesium arsenate was allowed twelve hours in which to settle and was then transferred by means of the mother liquor, without 

the use of other liquid, to a perforated crucible carrying an asbestos, 

felt, washed thoroughly with the mixture of one part of ammonia to 

three of water, usually employed for this purpose, but with the sparing 

use of the washing material which this mode of filtration permits, dried 

carefully, ignited gently at first, and at a low red heat afterward, in an 

atmosphere of oxygen. The great faults of this process, originally Levol's, have been the solubility of the precipitate in the mother liquor 

and, more especially, in the ammoniacal wash water, and the difficulty 

in drying or igniting the precipitate collected on paper. These sources 

of inaccuracy vanish, however, so completely with the use of the asbestos filter and due care in keeping the volume of mother liquor and the 

washings small, that the filtrate, freed from ammonia, acidified and 

charged with hydrogen sulphide, fails to yield arsenious sulphide. As 

a test for the presence of arsenic the method has enjoyed an excellent 

reputation, and in the form in which we have made use of it we believe 

it to be exact.

The filtrate from the precipitate of arseuious sulphide, containing all 

the boric acid, was nearly freed from hydrogen sulphide by the transmission of air, and the chlorine, with residual traces of hydrogen sulphide, 

was removed by treatment with silver nitrate and filtration. The filtrate from the precipitated sulphide and chloride was treated with sodium

(17) 

Bull. 47 2
18 WATERS OF YELLOWSTONE NATIONAL PARK. [HULL. 47.

hydrate, in quantity a little more than sufficient to precipitate the excess of silver, as completely as may be. The whole was evaporated 

until the precipitate took on a compact and granular form, then filtered, 

and the filtrate was evaporated nearly to dryness. The residue was 

treated with nitric acid, first just to acidity, and then with a sufficient 

(measured) amount to make it certain that the boric acid was entirely 

free. The concentrated solution of the nitrates, nitric acid, and boric 

acid was drenched with methyl alcohol to precipitate the first and dissolve the last. The solution of boric acid was quickly separated from 

the precipitate by means of the vacuum filter, and the residue washed 

sufficiently with methyl alcohol. When much boric acid is present the 

precipitated nitrates should be dissolved in water and the process of 

precipitation with methyl alcohol repeated; but when small quantities are dealt with, as was the case in the most of our work upon these 

waters, a single treatment leaves no boric acid in the residue. From 

the solution in methyl alcohol, the boric acid was separated and its 

amount estimated by a method devised by one of us and described elsewhere in full.1

This process consists essentially in distilling to dryness the solution 

in methyl alcohol, containing free nitric acid and nitrates, and treating

Fig. 2. Apparatus for the estimation of boric acid.

1 Bulletin of the U. S. Geological Survey, No. 42. Am. Chem. Jour., vol. 9, p. 23.'

(18)
ooocn AHD WHITFIKI.D.] METHODS OF ANALYSIS. 19

the residue by successive drenchings with methyl alcohol and distillations. The distillate, carefully protected, contains at the end of the 

operation all the boric acid, and this is fixed as calcium borate by 

the evaporation of the distillate over lime. The difference between 

the weight of ignited lime and the weight of the same after having 

been submitted to the action of the alcoholic solution and ignition is 

the weight of boric anhydride in the solution.

The distillation was effected by means of an apparatus which consists 

of retort, condenser, and bath for heating (Fig. 2). For the last a bath 

of paraffine is on the whole most convenient. The condenser is set vertically to facilitate changing the level of the retort within the bath, and 

to secure at the same time continued and thorough washing of the tube 

by its own condensations. The retort, somewhat like the well-known 

drying tube of Liebig in general shape, is easily made of a pipette by 

bending the tube at one end to a right angle, at the other to a gooseneck, as shown. To the former end is fitted, by a rubber stopper or section of tubing, a glass funnel-tube provided with a stop-cock; the end 

of the goose-neck passes tightly through a rubber stopper in the upper 

end of the condensing tube. This is essentially the apparatus; but it is 

convenient to attach, to receive the distillate, a small Erlenmeyer flask, 

which moves with the condenser and is joined to it, in the manner indicated in the figure, by means of a thistle tube and a rubber stopper 

grooved to permit the free passage of air. In carrying out the distillation the liquid is introduced into the retort either by the funnel tube or 

previous to its insertion, the glass stop-cock is closed, the water started 

through the condenser, and the retort lowered into the hot paraffine, 

care being taken to begin the operation with the retort not more thail 

half full and so inclined that only the rear dips below the surface of the 

bath. If the precaution to heat the retort at the start in this manner 

be overlooked it may sometimes happen that the sudden and violent 

expulsion of air through the liquid will carry portions of it bodily into 

the goose-neck and even into the condenser. With this point considered, the remainder of the operation presents no difficulty and requires^ 

little care. The size of the retort may be suited, of course, to the particular case in hand, but for most purposes a pipette of 200 cm3, capacity 

makes a retort of convenient dimensions, neither too large for the distillation of small charges nor too small to permit the treatment of 100 

cm3, of liquid comfortably. The tube of the-goose-neck should be wide 

enough to prevent the formation of bubbles in it; 0.7 cm. is a good 

measure for the interior diameter. It is of advantage to heat the bath 

to a point considerably above the temperature at which the liquid to be 

distilled boils something between 130° 0. and 140° C. does very well 

for water, and is not too high for methyl alcohol and under such circumstances, and when the retort is entirely submerged, it often happens 

that evaporation takes place with extreme rapidity from the surface of 

the liquid in perfect quiet and without actual boiling.

(19)
20 WATERS OF YELLOWSTONE NATIONAL PARK. IBULL.«.

Experiment showed that six successive treatments by drenching with 

10 cm3, of methyl alcohol and distillation to dryness were more than adequate to remove 0.2 g. of boric anhydride entirely from a residue containing 2 g. of sodium nitrate j but, in order to break up the crusted residue, 

which by its insolubility in the alcohol might effect to some extent the 

protection of the boric acid from the action of the alcohol, it was found 

best to introduce and evaporate 2 cm3, of water between the second and 

third, and again between the fourth and fifth distillations. In most of 

the cases with which we were concerned in the work upon these waters 

four treatments by drenching and distilling, with one intermediate 

moistening with water, were entirely sufficient to volatilize the boric 

acid; but in every case the residue was examined for boric acid by the 

exceedingly delicate turmeric test, taking care to first oxidize nitrites 

by means of bromine, and to expel the last before applying the test.

When the solution of boric acid in methyl alcohol is put over lime and 

evaporated at once some volatilization of the boric acid is apt to take 

placej but a short period of digestion from five to fifteen minutes is 

sufficient to fix the boric acid completely.

To secure the proper exposure before evaporation, with the least delay, the lime which is to retain the boric acid, first ignited in the crucible 

in which the evaporation is to be made subsequently, is transferred to 

the receiving flask attached to the condenser before the distillation is 

begun, and so has opportunity to exert its action upon the boric acid 

as the distillation progresses. At the end of the distillation the distillate, containing the alcohol, boric acid, nitric acid, and lime, is transferred again to the crucible, evaporated to dryness at a very gentle 

. heat, and ignited to a constant weight over the blast lamp. The greatest care is to be taken to secure similarity of conditions under which 

the crucible and lime are weighed before and after ignition, and definite 

periods of cooling before weighing ten minutes is a suitable timeshould be allowed to pass, in order to eliminate, as far as possible, the 

effect of atmospheric condensation upon the large surface of platinum.

The tendency of the process is to yield figures slightly larger than 

the truth, as was shown in the test analyses which are given in the full 

description of the process, to which reference has been made. In distilling 0.2 g. of boric anhydride and fixing it in 1.5 g. of calcium oxide, 

the mean error was shown to be about 0.0010+g. In the work upon 

the waters parallel determinations rarely differed by more than that 

amount.

£ Chlorine (ivith bromine and iodine). The precipitation of chlorine, together with bromine and iodine, was usually effected without difficulty 

by treating the weighed portion of water from 100 g. to 500 g., according to the circumstances with nitric acid to a slightly acid reaction and 

silver nitrate in excess, directly and in the usual manner, excepting that

(20)
AND WHiTfiELD.1 METHODS OF ANALYSIS. 21

the operation was effected in the cold and that the whole was allowed to 

stand quietly in the dark for several hours to secure perfect subsidence of 

the precipitate. In only one or two cases did the silica, which the waters 

carry abundantly, give rise to trouble in the precipitation. In such cases 

comparative tests were made as just described upon portions treated 

previously with an excess of pure sodium hydrate, it having been noticed 

that certain very siliceous waters, which of themselves very quickly 

 filled the pores of the filter with an invisible coating of silica, could be 

made to filter with rapidity by first treating them with sodium hydrate 

in excess, and then with nitric acid to slight acidity. Treatment with 

acid alone did not bring about the desired condition of the silica. In 

the case of the water of the Coral Spring the proportion of silica is so 

great and its character such that to secure satisfactory results we were 

obliged to convert the silica to hydrofluosilicic acid, by the addition of 

hydrofluoric acid and nitric acid, before precipitating the silver salt. 

The silver chloride (including the bromide and iodide) was collected 

upon asbestos in a perforated crucible, dried directly over the free, 

flame of a Bunsen burner turned very low and at a temperature below 

its melting point, and weighed. In the case of waters containing hydrogen sulphide in quantity precipitable by silver nitrate the portion for 

analysis was rendered ammoniacal before the addition of the silver salt, 

and the precipitated silver sulphide was filtered off. The silver salts 

of the halogens were then precipitated from the filtrate by nitric acid, 

and the process was completed as described.

Silica, iron and aluminum, calcium, and magnesium. A single weighed 

portion of water served for the determination of the silica, iron and 

aluminum, calcium and magnesium. The water was acidified with hydrochloric acid, evaporated to dryness in platinum over the water-bath, 

again acidified and again evaporated. The residue was digested with 

hot water containing a little hydrochloric acid, and the solution was 

filtered from the residue of silica, which was ignited in platinum and 

tested as to its purity in the usual manner with hydrofluoric acid.

In the filtrate ammonia, in the slightest excess, precipitated ferric 

andaluminic hydrates from the boiling solution, and these were collected, 

ignited, and weighed as oxides in the usual manner. The lime was 

thrown out of the hot ammoniacal filtrate by ammonium oxalate, and 

the calcium oxalate filtered off after standing twelve hours in the cold. 

When the amount precipitated exceeded a few milligrams it was dissolved in hydrochloric acid, reprecipitated by ammonia and ammonium 

oxalate and collected upon a filter, the filtrate from the second precipitation being added to that from the first. The calcium oxalate was 

dried, ignited, and weighed as calcium oxide,

The filtrate (or the united filtrates) from the calcium oxalate was 

evaporated in platinum, and the residue was gently ignited to destroy 

the ammonium oxalate which tends to delay the precipitation of the 

magnesia if permitted to remain in the solution and dissolved in hy-
22 WATERS otf YELLOWSTONE NATIONAL PARK.

drochloric acid. From this solution the magnesia was precipitated in 

the usual manner by microcosmic salt and ammonia, and after standing 

twelve hours or more, the phosphate was collected upon asbestos in a 

perforated crucible, washed with the mixture of one part of ammonia to 

three of water, commonly used in the process, moistened at the end of 

the washing with a strong solution of ammonium nitrate in ammonia, 

ignited for a moment to redness, and weighed as the pyrophosphate.

Sodium, potassium, and lithium. In some of the earlier work onlysodium and potassium, of the alkalies, were determined in the natural 

water, and for the determination of the lithium portions of the concentrated water were treated by the method which will be referred to later. 

In the greater number of cases the same portion of the natural water 

served for the determination of lithium as well as sodium and potassium. The portion for analysis was acidified in platinum with hydro, 

chloric acid and evaporated to dryness. The residue was extracted 

with hot water slightly acidulated with hydrochloric acid, the solution 

was separated from the precipitated silica by filtration, and to the filtrate was added, with care to secure a sufficiency and yet to avoid a 

great excess, barium hydrate made from the nitrate, itself purified by 

precipitation by nitric acid. Filtration separated the precipitated hydrates of aluminum, iron, and magnesium, with barium sulphate 5 and 

from the filtrate ammonium carbonate and ammonia precipitated, upon 

boiling, nearly the whole of the barium and calcium as carbonates. 

The filtrate from the precipitated carbonates was evaporated to dryness, 

and the residue was gently ignited to remove ammonium chloride, treated 

with hydrochloric acid, freed from the excess of acid by evaporation on 

the water-bath to dryness, dissolved in a very small amount of water, 

and treated again with a few drops of the solution of ammonium carbonate and ammonia. This treatment usually results in the precipitation of traces of barium carbonate which have previously escaped removal by the similar treatment of the larger volume of liquid. The filtrate from this last slight precipitate was again evaporated and treated 

as before; and, in case any further precipitation took place, the process 

was repeated until the purification was complete. Usually, however, the 

first precipitation in the larger volume of liquid and the second treatment in the solution reduced to small bulk are together sufficient to 

remove the barium carbonate completely. The filtrate from the last 

precipitate was evaporated in a weighed platinum dish, and the residue, consisting of the chlorides of sodium, potassium, and lithium, was 

dried, gently ignited, and weighed.

From the mixed chlorides the lithium salt was separated by a process 

which, devised by one of us during the progress of the work and described elsewhere in full,1 needs but brief outlining in this place. To 

the concentrated solution of chlorides ainyl alcohol is added and heat 

is applied, gently at first to avoid danger of bumping, until, the water

1 Bulletin of the U. S. Geological Survey, No. 42, p. 73; Am. Cbem. Jour., vol. 9, p. 33.

(22) -
660CH AND WHiTtfiELD.j MEf HODS OF ANALYSIS. 23

disappearing from solution and the point of ebullition rising and becoming constant for some minutes at a temperature approximately that 

at which the alcohol boils by itself, the chlorides of sodium and potassium are deposited, and the lithium chloride is dehydrated and taken 

into solution. At this stage of the proceeding the liquid is cooled, a 

drop or two of strong hydrochloric acid being added to reconvert traces 

of lithium hydrate possibly in the deposit, and the boiling is continued 

until the alcohol is again free from water. If the amount of lithium 

chloride present in the mixture of salts is small it is now found in solution ; the chlorides of sodium and potassium, excepting the traces for 

which correction will be made subsequently, are in the residue; and 

the separation may be effected by filtration and the washing of the residue with amyl alcohol previously dehydrated by boiling. If, on the 

other hand, the weight of lithium chloride present exceeds ten or twenty 

milligrams it is advisable, though not absolutely essential to the attainment of fairly correct results, to decant the liquid from the deposit, 

wash the latter with a little anhydrous amyl alcohol, dissolve in a few 

drops of water, and repeat the separation by boiling in amyl alcohol.

The filtrates, first measured apart, are united with the washings 

and evaporated to dryness, and the residue, treated with sulphuric 

acid in excess, ignited gently at first and finally to the fusing point, is 

weighed as the neutral lithium sulphate, containing traces of the neutral sulphates of sodium and potassium. From the weight thus found 

the subtraction of 0.00109 g. for every 10 cm3, of filtrate exclusive of 

washings makes the proper correction for the amounts of the sodium 

and potassium salts present, and the residual weight represents the 

pure lithium sulphate. In cases where the precipitate consists solely 

of sodium chloride, the correction upon the weight of the sulphate is 

0.00050 g.; when potassium chloride constitutes the residue the correction amounts to 0.00059 g. for every 10 cm3 , of filtrate. The alcohol used in washing has, within reasonable limits, no appreciable solvent effect upon the precipitate.

The precipitate, consisting entirely of sodium chloride and potassium 

chloride, is ready for the balance after drying a few minutes directly 

over a flame turned low, if the filtration is effected by means of asbestos 

in the perforated crucible; if paper is used as the filtering medium, 

after the solution of the precipitate, the evaporation of the solution and 

the gentle ignition of the residue. The weight of the insoluble chlorides actually obtained is corrected for the solubility of the salts in 

amyl alcohol by adding 0.00092 g. for every 10 cm3 , of amyl alcohol 

in the filtrates, exclusive of washings ; 0.00011 g. of this representing the sodium chloride dissolved, and 0.00051 g. the potassium chloride. With due attention to the reduction of volume of the residual 

alcohol before filtering the correction may be held easily within narrow limits.

(23)
24 WATERS OF YELLOWSTOtfE NATIONAL PARK. (BULL. 4?.

In applying this method to the analysis of the waters of the Yellowstone Park the practice of reducing the volume of amyl alcohol to about 

15 cm3, before filtering was followed uniformly. The corrections, therefore, were always the same, and amounted to an addition of 0.0007 g. 

to the apparent weight of sodium chloride, 0.0008 g. to that of potassium chloride, and a subtraction of 0.0017 g. from the weight of 

lithium sulphate indicated by the balance. In many cases the lithium 

present in the waters, though capable of detection by the spectroscope, 

amounted to so little in the portions devoted to its determination that 

the application of the correction left nothing to be called lithium sulphate. In such cases the lithium is counted as a " trace."

From the mixture of sodium chloride and potassium chloride the potassium salt was separated as potassio-platinic chloride. The chlorides 

were dissolved in a small amount of water, platinic chloride was added in 

solution, in quantity considerably in excess of the amount necessary to 

effect the conversion of all the potassium and sodium present to the 

double platinum salts, and the mixture evaporated on the water-bath to 

the point at which the residue becomes pasty if removed from the bath 

and allowed to cool. The crust thus formed was drenched with alcohol of 80 per cent., digested in the cold until thoroughly disintegrated, 

filtered off on an asbestos felt, washed with alcohol of 95 per cent., dried 

at a gentle heat, and weighed.

The lithium and potassium having been thus found directly, the sodium 

is given, in. the form of the chloride, by the difference between the sum of 

the lithium and potassium chlorides and the total weight of the three 

chlorides ; or, by thedifference between the weight of potassium chloride 

found and the weight of the chlorides of potassium and sodium found 

(the proper correction having been applied) after the separation of the 

lithium. It may be urged against the former plan that to bring the 

three chlorides to a definite condition for weighing is a difficult undertaking in view Of the great tendency of lithium chloride to exchange 

chlorine for oxygen in the presence of water. Our experiments indicated, however, that under repeated treatments by moistening and ignition the mixed chlorides did not change in weight materially, and we 

are disposed to attribute the result in part to the protective influence 

of the sodium and potassium salts upon the relatively small amount of 

lithium chloride, and in part to the care taken to secure thorough drying 

at alow temperature previous to the gentle ignition. In our work upon 

the waters we weighed the three chlorides together and found the sodium chloride by deducting from this weight the weights of potassium 

chloride and lithium chloride deduced by analysis.

A weak point in the process which we have employed in the determi. 

nation of the alkalies would seem to be found in the separation of the 

magnesia by means of barium hydrate. In connection with this subject it is of interest to note that in the greater number of waters magnesia was present only in inconsiderable quantity, and further, that in

(24)
&OOCH ASD wdifpiELD.] METHODS o$ ANALYSIS. 425

the case of those in which it did appear in appreciable ainounts the 

examination of the solution of the lithium sulphate, after the separation by amyl alcohol, failed to indicate the presence of magnesia in 

amount sufficient to be precipitable by inicrocosinic salt in an ammoniacal solution and under the usual conditions of the test, though this 

would be the place in which magnesia should appear if it had escaped 

removal from the chlorides. We are constrained to believe, therefore, 

that the process of separation which we adopted was exact within reasonable limits.

Ammonia and albuminoid ammonia. The determination of ammonia 

was effected in the usual manner by distilling a measured portion of 

water with sodium hydrate, and nesslerizing the distillate. A second 

portion of water was distilled with sodium hydrate and potassium permanganate, and the distillate was nesslerized. The former process 

gives the combined ammonia present in the water 5 the latter the total 

ammonia, which includes, beside the ammonia existing as such in combination, that ammonia which is developed from other nitrogenous compounds by the action of the permanganate. Thedifference between the 

figures of the two processes is the albuminoid ammonia, so called. The 

composition of these waters renders them peculiarly liable to boil explosively, and some difficulty was experienced at first in the distillation ; 

but the apparatus which is described in the paragraph on the determination of the boric acid proved to be of service in this case also, and 

made the determination practicable. The Nessler solution was very 

delicately adjusted, and the tests were made in small .tubes and carried to the limit of 0.000001 g.

TREATMENT OF CONCENTRATED WATERS.

In the examination of the concentrated waters the whole sample was 

evaporated to dryness, and the residue thus left was extracted with hot 

water. It is usual in treating concentrated waters to add sodium carbonate during the evaporation, and to wash the residue until the washings cease to show an alkaline reaction. Four of the waters of which we 

had concentrated samples were, however, so alkaline of themselves that 

 the addition of sodium carbonate was superfluous, and all were so siliceous that to wash the residue of evaporation until it was free from 

alkali was a matter of the greatest tediousness and difficulty. We 

found it best and sufficient to wash only to the vanishing point of the 

spectroscopic reaction for lithium in the washings. In this manner the 

separation of the greater part of the silica with the insoluble constituents of the water was effected without an entirely unreasonable expenditure of time and effort. The filtrate and washings were thoroughly 

mixed and made up to a definite weight. The. residue was kept by 

itself for separate treatment.

The filtrate should contain the bromine, iodine, boron, arsenic, antimony ; the copper, lead and tin, which can be present in the waters

(25)
26 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 41

only in traces; the lithium, caesium, rubidium, thallium, and part of the 

silicon and aluminum. The precipitate should* contain the titanium, 

phosphorus, fluorine, iron, manganese, barium, strontium, calcium, 

magnesium, with the remainder of the aluminum and silicon.

STRENGTH OF THE CONCENTRATED WATERS.

The degree to which the concentration of the waters had been carried 

in the field was fixed by the determination of the total amount of halogens in a weighed portion of the extraction of the residue of evaporation. This portion was diluted, acidified with nitric acid, treated with 

silver nitrate until the precipitate ceased to form, and the last was collected on asbestos in a perforated crucible, dried (over the free flame of 

a Bunseu burner turned low) at a temperature considerably below its 

melting point, and weighed. Determinations of this sort were made in 

duplicate. Knowing the weight of the silver salt thus found and the 

weight of the same precipitable from a known weight of the natural 

water, the exact value of the concentrated water, in terms of the natural water which it represented, became known.

TREATMENT OF THE RESIDUE.

Fluorine. The residue, dried by gentle heating, with the ash of the 

filter employed in separating and washing it, was placed in a retort of 

the pattern described in the section treating of the determination of 

boric acid in the natural water, drenched'wilh strong sulphuric acid, 

and heated to .150° C., while a slow current of dry air wastforced through 

the emulsion and thence directly into a U tube partly filled with dilute 

ammonia. The fluorine contained in the water should appear in the 

residue as calcium fluoride, should be volatilized as silicon fluoride by 

the action of the sulphuric acid, and, if present in more than very small 

amounts, should be indicated by the precipitation of silica in the U tube

containing ammonia. Proceeding in this manner we found in the waters 

which we examined no fluorine; and on treating the ammoniacal liquid 

of the U tube according to the method of Berzelius, with zinc oxide 

dissolved in ammonia, evaporating until the solution ceased to evolve 

ammonia, filtering, adding to the filtrate calcium chloride followed by 

sodium carbonate, boiling, igniting the precipitate and extracting it with 

acetic acid, we were not able to detect a residue of calcium fluoride; 

nor in the zinc oxide precipitated by the expulsion of the ammonia dissolving it could we discover silica.

Barium and strontium. The contents of the retort were transferred 

to platinum, treated with hydrofluoric acid (purified by redistillation; 

in sufficient amount to volatilize all silica, and evaporated to drynesa 

with a little sulphuric acid. To insure thoroughness of action this process of treatment was repeated. The residue was fused with sodium carbonate and tlie melt was extracted with hot water containing a few dropa

(26)
600CH AtfD METHODS OF ANALYSIS. 27

of alcoliol. The precipitate was separated from the solution by filtration and digested with hot dilute acetic acid, which should dissolve the 

barium, strontium, calcium, and magnesium carbonates. The solution 

in acetic acid, separated by filtration from the portion unacted upon, 

was nearly neutralized with ammonia, and to it was added in solution 

an amount of ammonium sulphate equal to fifty times the weight of the 

alkaline earths present, the whole being permitted to stand quietly 

twelve hours. By this treatment barium and strontium, should be 

precipitated as sulphates, while calcium and magnesium should remain dissolved. The sulphates of barium and strontium may be separated afterward by digestion during twelve hours (at the ordinary temperature and with frequent stirring) in ammonium carbonate, the decantation of the supernatant liquid, the repetition of the treatment 

with ammonium carbonate, and, finally, the action of hydrochloric acid 

upon the residue the strontium carbonate dissolving and the barium 

sulphate remaining insoluble in this acid. This mode of Separating the 

barium and strontium was not actually applied in our work, inasmuch 

as we obtained from the quantities of water with which we had to deal 

no precipitate by ammonium sulphate, and it is mentioned only for the 

purpose of completing the scheme of analysis.

The solution which had been treated with ammonium sulphate to 

precipitate barium and strontium was preserved for subsequent examination for manganese.

Phosphoric acid. The extract of the fusion in sodium carbonate was 

acidified with nitric acid, evaporated to small bulk, and from it the 

phosphoric acid was precipitated in the usual manner as a phosphomolybdate of ammonia. The precipitate, after standing twelve hours, 

was separated by filtration through a felt of asbestos in a perforated 

crucible, washed with the precipitant, and dissolved in ammonia. From 

this solution the phosphoric acid was precipitated by the magnesium and 

ammonium chloride mixture, and the ammonio-magnesiuin phosphate 

was filtered off on asbestos, washed with dilute ammonia (one part of 

ammonia to three of water), moistened with ammonium nitrate in ammonia, dried, ignited at a red heat, and weighed as magnesium pyrophosphate.

Manganese. The residue left, after the extraction of the fusion in the 

sodium carbonate with water containing a little alcohol and the treatment with acetic acid, was fused again in a little sodium carbonate, the 

melt was dissolved in the crucible by heating with strong sulphuric acid, 

and this solution was poured into cold water. In this manner was obtained a solution containing the titanium and iron, and a part of the 

aluminum and Inauganese. From it all these elements, excepting the 

last, were precipitated by adding ammonia to an alkaline reaction followed by acetic acid to faint acidity, and boiling. The precipitate was 

kept for examination later. The solution was mixed with that which 

had been treated with ammonium sulphate in the test for barium and

' .(27)
28 WATERS OF YELLOWSTO^D NATIONAL PARK.

strontium, and to the mixture, heated on the water bath, were added 

ammonia in excess and bromine water. The precipitate thus obtained 

was ignited, and weighed as Mn3O4, it being so trifling that solution and 

reprecipitation as the phosphate was unnecessary. 

. Iron. The precipitate of ferric, titanic and aluminic hydrates was 

fused in a little sodium carbonate, the fusion was dissolved in strong 

sulphuric acid, this-solution poured into cold water, and the dissolved 

iron, titanium, and aluminum were separated as follows, by a process 

devised by one of us and described fully elsewhere.1 Tartaric acid, 

amounting to three times the weight of the oxides of iron, aluminum, 

and titanium present, was added to the solution, which was then made 

faintly arnrnoniacal and submitted to the action of a current of hydrogen 

sulphide. The precipitated ferrous sulphide was filtered off (care having been taken that the solution should still be alkaline before filtering), washed with hot water sufficiently but expeditiously, dissolved in 

hydrochloric acid, and the iron, first oxidized by bromine, was precipitated by ammonia and weighed as the oxide.

Titanic acid. The filtrate from the ferrous sulphide was acidified 

strongly with sulphuric acid, heated to the boiling point, and treated 

with potassium permanganate until its characteristic color appeared. 

The final products of the action of the permanganate upon the tartaric 

acid are carbonic acid and water, but formic acid appears as an intermediary step in the oxidation. During the first action of the permanganate its conversion to manganous sulphate is rapid, but with the 

development of formic acid there takes place by its action upon the permanganate freshly added a precipitation of a brown hydrate of manganese which, redissolving readily so long as tartaric acid remains, yields 

only slowly to the further action of the formic acid. When, therefore, 

manganic hydrate appears abundantly in the boiling solution and does 

not dissolve perceptibly one may be reasonably certain that the conversion of the tartaric acid to at least the intermediary stage has been 

accomplished ; but for the sake of greater security, the addition of the 

permanganate may be continued until the appearance of its color. 

When the amount of tartaric acid in the solution is known, as should 

be the case always, a simple mode of proceeding is, perhaps, to employ 

for the oxidation the amount of permanganate theoretically required. 

A weight of potassium permanganate amounting to two- and a half 

times the weight of the tartaric acid to be destroyed is sufficient to 

carry the oxidation to the ultimate limit, providing there be no deposition of a manganic hydrate.

The residual permanganate and the insoluble hydrate were reduced 

and dissolved by the addition of a little ammonium bisulphite to the 

acid solution, and, the excess of sulphurous acid having been boiled off, 

acetic acid was added to the clear solution in quantity sufficient to make

1 Bnlletia of the U. S. Geological Survey, No. 27, p. 16; Am. Chem. Jour., vol. 7, 

l885-'86, p. 283.

(28)
GOOCH AJJ'IJ wHiTFiKLD. ] ' METHODS OF ANALYSIS. 29

 s

the amount of the absolute acetic acid present from 7 to 11 per cent, by 

volume; enough sodium acetate was introduced to fix all the sulphuric 

acid as sodium sulphate, and the. solution was boiled. If titanium is 

present it is precipitated under these conditions, while the aluminum remains dissolved. If the quantity of the precipitate thus obtained is 

considerable, it should be filtered from the liquid in which it floats and 

purified from the traces of manganese which it may carry, by fusion in 

a small quantity of sodium carbonate, the solution of the melt in sulphuric acid, and reprecipitation by ammonia.

In the waters which wo examined we found no precipitate of titanic 

hydrate at the point in the process where it should appear were titanium present,

TREATMENT OF THE AQUEOUS SOLUTION.

The aqueous solution, its degree of concentration having been determined in the manner already described, was divided into five portions. 

Two of these were taken for the determination of bromine, iodine, 

lithium, caesium, rubidium, and thallium, in duplicate; two for the determination in duplicate of arsenic, antimony, tin, copper, lead, and 

boron; and the remaining portion was reserved to be used in an emergency.

Iodine and bromine. The portion for the determination of the elements of the former group was weighed and evaporated to a pasty condition. The residue was thoroughly extracted with strong alcohol, 

treated with water reduced again nearly to dryness, and again extracted 

with alcohol. The extract was evaporated after the addition of a drop 

or two of a strong solution of sodium hydrate, and this residue was extracted with alcohol like the former residue. The residues of the extractions with alcohol were kept for subsequent treatment. The alcoholic solution containing presumably all the iodine and bromine, with a small 

proportion of the chlorine originally in the water, was evaporated to dryness, and the solution of the residue in water was acidulated with sulphuric acid mixed with a solution of ferric sulphate introduced into a 

retort of the pattern previously described and figured in connection 

with the determination of boric acid in the natural waters, and distilled. 

The distillate was collected in a U tube attached to the condensing tube 

and sealed with carbon disulphide and water. If iodides are present in 

the retort to the minutest degree the iodine is set free as such, its characteristic color appears in the seal of carbon disulphide, and its amount 

may be determined by titratiou in the usual manner with sodium hyposulphite.

In the waters which we examined iodine was not present in sufficient 

quantity to appear in the test of the amounts at our disposal.

To the liquid remaining in the retort after the distillation had been 

prolonged sufficiently to insure the complete volatilization of the iodine 

a few crystals of potassium permanganate were added, and the distilla-

(29)
30 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

tion was continued. This distillate was collected as before in a U tube 

joined to the condenser, but the seal was made with chloroform and 

water. At the beginning of the operation the seal of the U tube showed 

in most cases the characteristic color of bromine, but this was discharged before the end of the operation by the excess of chlorine and 

replaced by the color of the latter. The contents of the U tube were 

transferred to a beaker and treated with pure sodium hydrate and zinc, 

and from the solution of sodium bromide and chloride thus obtained 

the silver salts were precipitated by silver nitrate, in the usual manner, 

after acidifying with nitric acid. The silver bromide and chloride thus 

precipitated were collected together upon asbestos in a perforated crucible, dried, weighed, and dissolved in potassium cyanide. From the 

cyanide solution the silver was deposited by electrolysis, according to 

the process described elsewhere by one of us for the indirect estimation 

of bromine in the presence of chlorine.1 In this manner we obtained 

the weight of the mixture of silver chloride and silver bromide, and the 

weight of the silver contained in the mixture. The amounts of bromine 

and chlorine in the mixed salts were determined from these data by the 

solution of a simple algebraical equation.

Lithium. The contents of the retort after the distillation of the bromine were united with the residues of the extractions by alcohol, the 

excess of sulphuric acid was volatilized, the residue dissolved in hjrdrochloric acid, the sulphates converted to chlorides by means of barium 

chloride, the baric sulphate thus formed separated by filtration, alumina, 

silica, and barium carbonate precipitated by ammonium carbonate and 

separated by filtration, and the solution evaporated to dryness. The 

residue was gently ignited to remove ammonium chloride, dissolved in 

water acidulated with hydrochloric acid, and this solution, concentrated until just ready to deposit, was drenched with strong alcohol. 

The sodium chloride precipitated was washed with alcohol until the

spectroscope indicated entire freedom, from lithium chloride. The alcoholic solution of lithium chloride was evaporated to dryness, and the 

residue was dissolved in a little water acidulated with hydrochloric 

acid. This solution was treated with a little pure barium hydrate 

(made from the nitrate precipitated from nitric acid) to remove traces 

of magnesia, and filtered, and from the filtrate the barium was removed 

by treatment with ammonium carbonate, repeated if necessary. From 

the solution of lithium chloride thus obtained the lithium was separated 

according to Mayer's method2 by evaporation with hydro-disodic phosphate and sodium hydrate, the treatment of the residue with sufficient 

hot water to dissolve the salts, which should be soluble with the aid of 

gentle heat, the addition of an equal volume of ammonia, and digestion

1 Bulletin of the U. S. Geological Survey, No. 42, p. 89; Am. Chein. Jour., vol. 8, p. 

421. 

3 Freseniu8's Quant. Anal., 6th Aufl., Band II. p. 215.

(30)
ooocti AHD wiuTFiitu). ] METHODS OF ANALYSIS. 31

iii the cold during twelve hours. The precipitate was filtered upon asbestos in a perforated crucible, washed with a mixture of equal parts 

of ammonia and water, ignited, and weighed. The filtrate from this 

precipitate was evaporated, and the residue of evaporation was again 

treated asi before to recover traces of lithium; and a similar process of 

treatment was applied .to the filtrate from the second precipitate. The 

three precipitates thus obtained contained presumably all the lithium 

as the tribasic phosphate.

This is the method of determining lithium which was employed previous to the development of the process which has been described in 

connection with the account of the determination of lithium in the natural waters (p. 22). Were the work to be repeated we should unquestionably employ the amyl alcohol process exclusively, although it may 

be said for the determinations by Mayer's method that their actual error 

was very much diminished by the use of comparatively larger portions 

of material for the analysis, and we are confident that the results are, 

on that account, fairly trustworthy.

Cccsium, rubidium, and thallium. The filtrate from lithium phosphate 

was freed from ammonia by boiling ; the phosphoric acid was precipitated by ferric chloride and ammonia, with the usual precautions to 

secure a suitable proportion of the iron salt and to keep the excess of 

ammonia at the lowest possible limit, and removed by filtration; the 

filtrate from ferric phosphate and ferric hydrate was evaporated to dryness and gently ignited to remove ammonium salts; the residue thus 

left was dissolved in water and treated with platinic chloride in excess 

of the amount necessary to convert all the alkaline chlorides present 

to platinum salts.

Th© precipitate by platinic chloride was extracted by boiling repeatedly with small portions of water, and the residues of this treatment were tested from time to time spectroscopically. The characteristic lines of cesium and rubidium appeared more distinctly toward 

the end of the process of extraction when they were visible at all, 

Thallium, which should appear, if present, in the intermediate extracts, 

failed to show itself in any of the waters.

Arsenic, antimony, tin, copper, and lead. The weighed portion of the 

concentrated solution was acidified with hydrochloric acid, heated to 

70° 0.. and submitted to the action of a current of hydrogen sulphide 

during several hours. The precipitated sulphide was filtered off upon 

anthracene -in a perforated crucible, following the method described by 

one of us.1 The crucible with the adherent filter of anthracene and the 

precipitate were placed in a small beaker, drenched with benzol, and 

gently warmed until the anthracene dissolved. Water containing sodium hydrate was added and, after sufficient digestion on the waterbatb, the liquid and precipitate were transferred to a paper filter, pre1 Bulletin of the U. S. Geological Survey, No. 42, p. 86; Am. Chem. Jour., vol. 7, 

1885-'86, p. 87.

(31)
32 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

viously moistened with water. In this manner the aqueous solution, 

carrying the arsenic, antimony, and tin, if present, was permitted to 

traverse the filter, while the sulphides of copper and lead, with possibly 

free sulphur, remained with the benzol upon the filter. After thorough 

washing with water the receptacle for the filtrate was changed, the 

filter was moistened with alcohol, and thus the benzol, with the anthracene in solution, was induced to pass through the paper, which, with 

the residue upon it was washed with benzol followed by alcohol and 

then by water. The filter was carefully incinerated, and the ash was 

digested with a few drops of nitric acid. The solution thus obtained 

was evaporated to dryness, the residue was moistened with hydrochloric acid, and, after the volatilization of the most of the acid, dissolved in hot water. From this solution hydrogen sulphide should precipitate copper and lead as sulphides. In the single case of that water 

which had been concentrated in porcelain no black sulphide was obtained at this point in the operation j in other cases, a trifling black 

precipitate fell, which subsequent examination proved to be copper 

sulphide exclusively, doubtless originating'in the concentrating vessel.

The second precipitation with hydrogen sulphide was introduced to 

test the presence of copper and lead, in the process just outlined, because the residue left upon the filter when the benzol is washed from it 

is apt to be dark in color, even in the absence of black sulphides.

The alkaline filtrate from the benzol and the insoluble residue were 

acidified with hydrochloric acid, after the addition of a drop or two of 

ammonium sulphide; the precipitate was filtered off' on asbestos in a 

perforated crucible; the filter and precipitate were dried and treated 

in a small beaker with fuming nitric acid; the solution in nitric acid 

was evaporated to dryuess, the residue was dissolved in hydrochloric 

acid, and from this solution, made strongly alkaline with ammonia containing some ammonium sulphide (the last to keep tin, if present, in 

solution), but kept small in volume, the arsenic was precipitated by the 

magnesium chloride mixture. The liquid was briskly stirred and then 

allowed to stand quietly for twelve hours at least. The precipitate was 

transferred by means of the mother liquor, without the use of other 

liquid, to a perforated crucible carrying an asbestos felt, washed with a 

mixture of one part of ammonia to three of M ater, dried carefully, ignited in an atmosphere of oxygen, and weighed as magnesium pyroarsenate.

The filtrate from the ainmonio-magnesium arsenate, which should 

contain the antimony and tin of the water, was evaporated to remove 

the great excess of the ammonia, and acidified with hydrochloric acid. 

The sulphur thus precipitated should carry with it the antimony and 

tin as sulphides. In no case were we able to detect antimony in this 

precipitate. In one or two cases there were evidences of the presence 

of tin, but this doubtless came from the lining of the vessel in which

(32)
GoocHAi;nvmiTFiELD.j STATEMENT OF ANALYSIS. 33

concentration was effected; in the water which was concentrated in porcelain no tin was found.

Boric acid. The.filtrate frorn the original precipitate by hydrogen sulphide in the acid solution was warmed gently, submitted to the action 

of a current of air to blow out the excess of hydrogen sulphide, brought 

nearly to neutrality by the addition of sodium carbonate, made faintly 

alkaline with ammonia, filtered from the precipitate thus thrown down, 

and evaporated nearly to dry ness after the addition of enough sodium 

hydrate to expel the .ammonia and yet preserve strong alkalinity. The 

residue was acidified with hydrochloric acid and extracted thoroughly 

with alcohol, and the alcoholic solution was made alkaline with sodium 

hydrate and evaporated to dryness. This residue was dissolved in 

water, just acidified with hydrochloric acid, and from the solution the 

last traces of silica, alumina, lime, and phosphoric acid were removed 

by the action of ammonia and ammonium carbonate, and filtration. In 

the filtrate the boric acid was determined according to Marignac's process, by treatment with magnesium chloride, ammonium chloride, and 

ammonia, evaporation to dryness, ignition at a red heat, extraction 

with boiling water, and the repetition upon the extract of the process 

of evaporation, ignition, and extraction. The residues left after extraction were together ignited and weighed, and the magnesia in the 

weighed material was determined by precipitation as the amnionio-magnesiurn phosphate and weighing as the pyrophosphate. The difference 

between the weight of the residue and its contents in magnesia is boric 

acid.

This was the process which we employed in the earlier determinations. 

The process which was developed later, and applied to the determination of boric acid in the natural waters, is preferable.

STATEMENT OF THE RESULTS OF ANALYSIS.

In stating the facts deduced from the analysis of the waters, it has 

seemed best to adopt the plan of recording the oxygen acids as anhydrides, the basic elements as such, and the oxygen which must exist in 

combination with the bases by itself; thus avoiding an arbitrary division 

of the basic elements among the oxygen acids and halogens. The 

basic oxygen, so-called, of the alkaline waters was found by computing 

the amount of oxygen which would exist in the.oxides of the basic elements and deducting from this amount the weight of oxygen equivalent 

to the halogen discovered by analysis. In the case of waters which 

carried such an excess of acid that the halogens maybe supposed to be 

uucombined with bases, the basic oxygen is the amount of oxygen which 

would exist in the oxides of the basic elements. In waters of such acidity 

that a portion only of the halogen may be supposed to be in combination with basic elements the equivalent in oxygen of the amount of

Bull. 47 3

(33)
34 WATERS OF YELLOWSTONE NATIONAL PAKK. [BULL.*?.

halogen which is regarded as in. combination was deducted from the 

total amount of oxygen of the oxides in computing the basic oxygen. 

The -halogen which remains uucombined with the -basic elements was, 

as a matter of course, assumed to be in association with hydrogen.

The hypothetical combination of the elements found in the waters 

must necessarily be largely imaginary, for nothing is more plainly 

evident than the impossibility of stating authoritatively, in the present 

condition of knowledge, the actual division of a number of acids among 

a number of bases iu solution. This we do know, that the 'combination 

is determined not only by the relative proportions of all the constituents, but by the absolute quantities of all associated in a definite 

amount of liquid. It is with no purpose, therefore, of attempting to 

represent actual conditions of combination, but only for the sake of 

securing a common ground of comparison among themselves and with 

other waters, that we have assumed arbitrarily the existence in these 

waters of the definite and simple combinations of the following 

scheme:

In alkaline waters, bromine has been combined as KBr; B2O3 as 

Na 2B4O7 ; As2O3 as NaAsO2 ; P2O5 as Na2HPO4 ; chlorine has been assigned to the bases in the order NH4, Li, K, Na; SO* has been linked 

with such bases as remain in the order NH4 , Li, K, Na, Mga Ca; residual 

bases have been classed as neutral carbonates in the order Mg, Ca, Na j 

residual sodium has been represented as lsraSiO3 ; aluminum and iron 

have been put down as A12O3 and Fe2O3 ; and residual CO2 and SiO2 

have been shown as such.

In making up the hypothetical composition of acid waters the same 

general arrangement has been kept as far as possible in order to secure 

ready comparison with the alkaline waters. Though the relative avidity of hydrochloric acid is greater at ordinary temperatures than that

of sulphuric acid, we have nevertheless represented hydrochloric acid

as the free acid whenever it became necessary to represent one of them 

as free.

The sulphuric acid indicated by the analysis has been combined with 

the bases in the order Ca, Mg, A1 2 , -Fe2 , Na, K, Li, NH4 ; the residual bases 

have been combined with chlorine in the same order 5 the anhydrides 

B2O3 , As2O3 , P2O.-,, Si02 , CO2 , and residual SO3 , have been stated as 

such; residual chlorine has been represented as HC1, and H2S as such.

It is apparent that in some instances combinations have been imagined which might exist under some of the circumstances encountered, 

but which are improbable under other conditions met with in waters of 

a generally similar character ; thus, for the sake of uniformity, we have 

represented the boric acid of the alkaline waters invariably as Na2B4O7 , 

and the phosphoric acid as Na2HPO4 , regardless of the variable action 

of an excess of alkaline carbonate upon these salts in hot solutions and 

under prolonged digestion. So, also SiO2 has been stated as free, 

when, if so, it must have been in solution in the presence of the carbon-

(34)
GOOCII AND wiiiTFiELD.l STATEMENT OF ANALYSIS. 35

ates of sodium, magnesium, and calcium; theueutral carbonates have 

been represented as such in the presence of free carbonic acid, both in 

hot and in cold waters; and potassium has been arbitrarily associated 

with bromine; and ammonium, lithium, and potassium have been preferred to other bases in combining the chlorine.

In the following tables are given the direct results of analysis in 

grams per kilogram of water, and the percentage composition of the 

material shown by the analysis; the hypothetical combination in grains 

per kilogram of water, and the percentage composition of the material 

of the hypothetical combination; the quantity of water used in each determination, and the number of determinations of each constituent. In 

the final table all the direct results of analysis are summarized.

(35)
36 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

ANALYSES. 

CLEOPATRA SPKLNG.

(Locality, Mammoth Hot Springs; date of collectiou, July 23, 1884; temperature,

67° C.; reaction, alkaline; specific gravity, 1.00205.) 

Sample No. 1 was taken from the center of the spring.

Constituents.

SiOz.. .......

so3 .... ......

C02 . ...... -.

BzOs. ........

AszCh .......

Cl...........

Br ..........

HaS. ...... .-

0 (basic).....

Fo ? A1 J. ........

Ca.. .........

Hg .......... 

K... .........

Na...... ....

Li ...........

NH4. ........

Grams per kilo 

of water.

0. 0517

0. 4395

0. 6287

0. 0226

0. 1749

Tr'i/*ft

0. 1951 

0. 0049 

0. 3070

0. 0729 

0. 0511

0 l'>99

. 0. 0023

0. 00063

2. 08523

Percent, of total material 

in solution.

2.48

21.08

30. 15

1.08

0.15

8.C9

9.37 

0. 23

3.50 

2. 45

C. 23

0.11

0.03

100. 00

Determinations.

2

0

0

 )

o

1

1

2 

<>

2

2

2

1

Grams of water 

employed in 

each determination. 

200

200

200

500

500

200

100

COO

200 

200

200 

200

200

200

50

Albuminoid ammonia (not in aummation) 0.00020 grams per kilo. 

Hypothetical combination.

Constituents.

NH4C1. ......

LiCl. ........

NaCl. .......

KC1..... ....

KBr.........

NaaSCM ...... 

MgS04 . ......

CaS04....... 

Na2B4 07 ..... 

NaAsOz...... 

CaCOs.......

AbOs- ........

SiOz...... ...

COa. .........

H«S.. ........

Grams per kilo 

of water.

0. 0019

0.0140

0. 1903

0. 0976

0. 1448

0. 19f)3 

0. 0226 

0. 004 1 

0. 6254

0. 0093

2. 0852

Percent, of total material 

 in solution.

0.09

0.07

9.13

4.68

6.94 

17.48

9.37 

1.56 

0.20 

. 29. 99

0.45

2.48

16.96

100. 00

(36)
OOOCH AND WHITFIELD.] RESULTS OF ANALYSIS. 37

Sample No. 2 was taken at a point in the overflow about 85 feet (25 

vertically and 60 horizontally) from the margin of the basin, for the purpose of getting some idea of the rate at which the water near the source 

was depositing travertine. The sample was collected at the same time 

with No. 1. The temperature of the water had fallen at the place where 

the sample was taken to 44° C. The determinations were not duplicated, and a portion of 150 g. was devoted to each determination. The 

deposit of calcium carbonate, which was found in the sample on cooling 

and standing though the water was clear when it was bottled was 

analyzed separately.

Constituents.

so3 ..........

CO-2. ...... ..

Ca..........

Mg ..........

Grams per kilo of water.

In the water.

0.4573 

0.3433 

0. 1926 

0.'0786

In the deposit.

0. 0433 

0. 0578 

0. 0011

Total.

0. 4573 

0. 3806 

0.2504 

0. 0797

If it be assumed that at the point at which the sample was taken, 

the water still carries the sulphates with which it lelt the source and 

this assumption is consonant with the fact.that the travertine deposits 

of these springs carry only trifling amounts of sulphuric acid the comparison of the analyses of Nos. 1 and 2 indicates that during the flow of 

the water, hot, thinly spread, and thoroughly churned, 4 per cent, of it 

was lost by evaporation; and that every kilogram of water which left 

the source and made this passage deposited something like 0.1C75 g. of 

calcium carbonate.

Sample No. 3 was taken as a preliminary specimen October 11, 1883. 

The sulphuric acid, carbonic acid, and calcium were alone determined:

S03

Grams 

per kilo.

. 0.4254

C02 ................................................... 0.5071

Ca .................. .................................. 0.3006

It will be noted that the small sample of 1883 carried about the same 

amount of lime, a little less sulphuric acid, and very much less carbonic 

acid than the sample of the year following. The deficiency in carbonic 

acid may have resulted from imperfect sealing of the bottle in which 

the water was preserved, 'and the lapse of time before (he analysis was 

made.

(37)
38 WATERS OF YELLOWSTON.E NATIONAL PARK, [BULL. 47.

OKANGE SPKING.

(Locality, Mammoth Hot Springs ; date of collection, October 11, 1883; temperature, 

63° C.; reaction, alkaline.)

Constituents.

SiOa .........

SOs. ......

CO, ...... ...

BaCh. ........

AssOz. .......

Cl....... ...

Br...........

HsS..........

0 (basic)..... 

Fe I Al J ------ 

Ca. .......- -.

Mg ..........

K. ...........

Na...........

Lift..........

NEU.........

Grams per kilo 

of water.

O fln(V">

0. 3378

0.1623

0. 1790 

0. 0012

0. 2821

0. 0610

0. 0010 

1. 7057

Per cent, of total material 

in solution.

2.94

19.81

9.51

10. 53

0.07

16. 54

3.58

7.23

0.09

100. 00

Determinations.

1

1

1

1

1

1

1

1

1 

1

1

1

1

1

1

Grams of water 

employed in 

each determination.

500

250

500

250

500

500

500

500

500

500

a As received in tbe laboratory. b By Mayer's method.

Hypotlietical combination.

Constituents.

LiCl. ........

NaCl...... --

KC1... ......

KBr. ........

NasSC>4 ...... 

HgSCh.......

CaS04. ...... 

CaCOs. ......

AlzOg........

SiO*. ........

co2 ...... ....

Grams per kilo

of water.

O ftfiQ?

0. 1636

0.1165

Trjico

0.1834 

0. 3295

0. 2002 

0.5580

0. 0022

0. 0502

0. 0924

1. 7057

Percent, of total material

in solution.

0.57

9.59

6.83

10.75 

19. 32

11.74 

32.71

0.13

2.94

5.42

100 00

(38)
COOCH AND WillTFlRLD.] RESULTS OF ANALYSIS. 39

HOT RIVER.

(Locality, Mammoth Hot Springs; date of collection, October 5, 1834; temperature, 

5b° C.; reaction, alkaline; specific gravity, 1.00157.)

Constituents.

Si02 .........

80s. .........

CCh.... ......

BsOa .........

AssOs........

Cl. ..........

Br.... .......

TItS. ........

0 (basic)....

Fe Alj--------- ?

Ca..........

Mg .........

K...........

 Sa... ........

Li ...........

NH«.........

Gramspevjulo 

of water.

0. 0500

0.4230

0. 4270

0 01 9ft

0.0004

0. 1G04

0.1C82

n 9<?fifl

0. 0402

0.150G

0.0011

o. coon

1. 74401

Per cent, of total material 

in solution.

2

07

24.20

24.49

O

f70

0.02

9.20

9.64

0 n 9

10 p;fj

8. 63

0.01

100. 00

Determinations.

2

2

0

2

1

1

2

9

t)

2

2

1

Grams of water 

employed in 

each determination.

200

200

200

500

500

100

100

COO

200

200

100

100

50

Albuminoid ammonia, traco.

Hypothetical combination.

Constituents.

NH4C1.......

LiCl. ........

Nad ........

KC1.... ......

XnsSOj ..... 

MgSOj.......

 CuSCh .......

Nfi 2Bj07 .... 

JTaAsO-j ----- 

CaCOs .......

A1203 - ------

SiO"

C02 .... ......

Grams por kilo 

of water.

0. 0068

0. 1856

O noo-j

0. 22C5

0. 14 CO

0. 0185 

0.0004 

0. 4W3

O.C007

0.0500

0. 2143

1. 7440

Per cent, of total material 

in solution.

0.02

0.39

5.00

12.98

S

o -i

LOG

0.02 

27.71

0.56

2.87

12.29

100. 00

(39)
40 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

GARMNER RIVER.

(Locality, above Hot River; date of collection, October 12,1833 ; temperature, 8° C.)

Constituents.

SiCh .........

SOs..........

CCh .........

Cl ...........

O (basic) .... 

Fe ? Al j. ........ 

Ca. ..........

Mg.... ......

K. ...........

Li ...........

Grams per kilo 

of water.

O.OiCO

0.0117

0. 0710

0. 0049

0. 021C 

0.0012

0. 0250

0. 0005

0. 0079

0.0200 '

0. 2137

Percent, of totill material 

in solulioti.

21. 05

5.47

33.23

2.29

10. 11 

1.9G

11.70

0.23

3,70

9.:!G

100. 00

Determinations.

9

2

9

2

2

2

2

2

2

Grams of water 

employed in 

each determination.

100

100

200

100

100

100

100

100

Hypothetical combination.

Constituents.

LiCl. ........

.KC1 .........

IGSC-4 .......

jSra2SOj ......

Na2CO3 ..--.. 

MgCOs ...... 

CaCOs.- -.-..

AbOs ........

SiO*. ........

CCb.-.. ......

Grams per kilo 

of water.

0.0103

0.01GL 

0. 03-40 

0.0018 

0. 0625

0.0079

0.0 109

0. 02feG

0. 2137

Percent, of total material 

in solution..

4.82

2.C2

7.53

15.91 

0.84 

29. 2r.

3.70

21. 95

13.38

100. CO

(40)
GOOCH AND WHITFIELD.] RESULTS OF ANALYSIS. 41

GARDINER RIVER.

(Locality, Mammoth Hot Springs, below Hot River; date of collection, September 

26, 1884 ; temperature, 13° C.)

Constituents.

SiOs .........

SOs..........

COs..........

Cl ..........

0 (basic)..... 

Fe» A , j. ......... 

Ca. ..........

Mg ..........

K. ...........

Li ...........

Grams per kilo 

of water.

0. 0272

0. 0802

A 1 79 S

0.0301

0.(M87

0. 0749

0.0105

0.0311

0. 4037

Percent, of total material 

in solution.

*; 11

10.24

34 94

6.1.0

0.86 .

15. 1.7

2.13

6.30

. 100. 00

Determinations.

9

9

2

2

2

2

9

9

Grams of water 

employed in 

each determination.

500

500

500

500

500

500

500

500

500

Hypothetical combination.

Constituents.

LiCl.........

KC1. .........

KaCl.. .......

NaaSCU .----. 

MgS04.......

MgCOs ...... 

CaCOs.......

AbOa ........

SiOa .........

COj... .......

Grams per kilo 

of water.

Trice

O AOOQ

0. 0540 

0. 0739

0. 0094 

0. 1873

0. 0019

0. 0272

0. 0852

0. 4937

Per. cent, of total material 

in solution.

4.05

6.87

11.12 

14.97

1.90 

37. 94

0.38

5.51

17.26

100. 00

(41)
42 WATERS OF YELLOWSTONE NATIONAL TAKE. [BULL. 47.

WATER SUPPLY AT MAMMOTH HOT SPRINGS.

(Locality, faucet in hotel; date of collectiou, July 28, 1884.)

Constituents.

SiCh .........

80s. .........

COz. .........

Cl ...........

0 (basic) .....

Fe AMj ......... 

Ca.. .........

Mg ..........

K.... ........

Na .........

Li...........

Grams per kilo 

of water.

0. 0310

0. 1230

0. 0022

0. 0248 

0.0011

0. 0310

0. 0089

0.0031

0. 0145

0. 2757

Percent, of total material 

in solution.

19 CO

11.24

44.61

0,80

9.00 

0.40

11.46

3. 23

1.12

5.26

100. 00

Determinations.

2

0

9

0

2

9

2

2'

9

Grams of water 

employed in 

each determination.

1000

1000

2uO

500

'1008

1000

1000

1000

1000

Ammonia, 0.000022 gram; albuminoid ammonia, 0.000028 gram; 

0.000115 gram per kilo.

Hypothetical combination.

nitric acid,

Constituents.

KC1..........

K2S04 .......

Na2S04 ...... 

MgS04. ......

HgC03 ...... 

CaC03 .......

AT n

SiCh .........

pn

Grains per kilo 

of water.

0.0015

0. 0448 

0. 0076

0. 0258 

0. 0700

0. 0021

0.0748

0. 2757

Per cent, of total material 

in solution.

0. 54

16. 25 

2.76

9.36

0.76

19 Qft

27. 13

100. 00

Grains per 

TJ. S. gallon.

O

OPO0. 0875

2.6151 

0. 4436

1. 5060 

4. 6114

0. 1225

16. 0930

(42)
GOOCH AND WIIITFIELD.1 RESULTS OF ANALYSIS. 43

SODA SPRING.

-(Locality, Mammoth Hot Springs; date of collection, , 1887; temperature, 6°C.; 

reaction, acid; specific gravity, 1.00041.)

Const! tnents.

SiOa .........

SO.!....--..-.

co«..........

BaOa .........

Cl ..........

HjS... .......

0 (basic) ..... 

Pe. ..........

Al. ..........

Ca.... .......

Mg ..........

K...... ......

Na. ..........

Li ...........

HH«. ........

Grams per kilo 

of water.

0. 0184

0. 0390

0. 6735

0. 0044

0. 0432 

0. 0053

0. 0004

0. 0808

0.0100

0. 0027

0. 0039

0. 0005

0. 8827

Percent, of total material 

in solution.

2.08

4.42

76.30

0.50

4.89 

0. GO

O.OG

9.15

1.20

0.31

0.44

.05

100. 00

Determinations.

0

2

2

2

2

2

-

2

2

2

2

2

2

2

2

Grains of water 

employed in 

each determination.

500

200

200

1,000

1,000

200

200

500

500

500

500

200

200

200

50

Albuminoid ammonia: Trace.

Hypothetical combination.

Constituents.

UIUCl.......

Lid.........

KC1 .........

MaCl ........

Na2S04 ...... 

M>S04.......

MgCOs... ... 

CaCOs .......

FoiOs ........

SiOz ....-..'..

C02..........

C-rnrnsper kilo 

of water.

0. 0015

0. 0051

0.0015

0. 0102 

0. 0500

0.0021 

0. 2020

0. 0070

0. 0008

0. 0181

0. 88-J7

Percent, of total material 

in solution.

0.17

0.58

0.17

1.16 

5.67

.24 

22.88

8ft

09

2.08

CO. 10

JOO.OO

(43)
WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

FEARLESS GEYSER.

(Locality, Norris Geyser Basin; date of collection, August 18, 1884; temperature, 

88° C.; reaction, neutral; specific gravity, 1.00110.)

Constituents

SiOi .........

TiOs. ........

SOa.... ......

COz.. ........

N2 05 . ........

PA ...... ...

BzOs.........

AssOa. .......

Cl ...........

Bz ...........

I.............

Fl ...........

H2S. ........ 

O(basic) ..... 

Fe..... ......

Al. ..........

Mn .........

Ba...........

Sr ...........

Ca.... .......

Mg ..........

Cs ...........

Kb...........

K.... ........

'LI ...........

NH4 .........

Grams per kilo 

of water.

0. 4180

0. 0367

0. 0046

0. 0022

0. 6705

0. 0026

Trace 

0. 0113 

0. 0006

0. 0002

0. 0092

0. 0001

rPrtnfi£v

0. 0415

0. 4046

0.00816

0. 00025

1. 63275

Percent, of total material 

iu solution.

25.60

2.25

0.28

1.36

0. U

41.06

0.16

0.70 

0.04

0.01

0. 56

0. 01

2.54

24.77

0.50

0.02

100. 00

"Determinations.

2

1

2

2

1

1

2

2

2

2

2

1

1 

2

2

1

1

1

2

1

1

2

2

2

1

Grams of water 

employed in 

each determination.

500

39, 500

1000

500

400

39, 500

7,900

7,900

200

7,900

7,900

39, 500

600 

39, 500

500

39, 500

39, 500

39, 500

500

500

7,900

200

200

7.900

500

i Found by Marignac's method, b Found by Mayer's method. 

Albuminoid ammonia (not in summation) 0.00001 grams per kilo.

(44)
GOOCH AND WHITFIELD.j RESULTS OF ANALYSIS.

Hypothetical combination.

Constituents.

NH4C1.......

LiCl ........

KC1 .........

XBr. ........

CsCl.........

RbCl.........

NaCl ........

NasSOi ...... 

MgS04- ......

CaSUi .......

NasUiO, ..... 

NaAsOi......

FeCo3 . .......

AlsOa. .......

SiOz .... ....

H5S.. ........

Grams par kilo 

of water.

0. 0007

0.0492

0. 07G8

0. 0039

Tl'flCO

Trace

0. 9760

0. 0404 

0. 0005

0. 0230

0.0319 

0. 0029 

0. 00«1.

0.0011

0. OOOi

0. 4180

0. 0019

1. 6328

Percent, of total material 

in solution.

0.04

3

n*>

4.71

0.24

59.78

2.47 

0.03

1.41

1.90 

0.18 

0.37

0.06

0.02

25.60

0.11

100. 00

The analysis of a preliminary sample of 1,350 cm3 ., taken September 27, 1883, yielded 

the following figures, whicb signify grams of material per kilogram of water: SiO-j 

0.3463; SO3 O.C501; Cl 0.6476; Fe, Al 0.0021; Ca 0.0098; Mg trace; K 0.0443; Na 

0.3931; Li 0.0042.

(45)
46 WATERS OF YELLOWSTONE NATIONAL PARK. -[BULL. 47.

PEARL GEYSER.

(Locality, Norris Geyser Basia ; date of collection, August 20, 1884 ; temperature, 

84° C.; reaction, neutral; specific gravity, 1.00110.)

Constituents.

SiOz. ........

TiOj........

^O*

C02 .. ........

N2 05 ........

PaOo ........

T> rrf~jn

AsiOs ........

Cl ...........

Br..... ......

I ............

El ...........

H2S. .........

Fe. ..........

Al..........

Mn ..........

Sr ...........

Ca...........

Mg ..........

Cs.... .......

Rb ..........

K.... ........

Li ........:..

NH4 .........

Grams per kilo 

of water.

0. 4636

0. 0075

[0. 0273]

0. 0038

0. 6520

0.0134

Trace

0. 0031

0. 0064

0. 0009

0. 0544

0. 4046

0. 0022 b

0.00021

[1.66221]

Percent, of total material 

in solution.

97 gg

1

OU

0.45

[1. 65]

0.23

39.22

0

01

0.18

0.38

0.05

3.27

24.34

0.14

0.01

[100. 00]

Determinations.

2

1

2

1

1

2

2

1

1

1

2

1

1

1

2

2

2

2

o

1

Grams of water 

'employed in 

each determination.

500

54 OOG

liooo

200

54, 000

3,200

200

54, 000

600

54000

500

54, 000

54, 000

54, 000

500

500

200

200

10, 800

1,000

a 0.000038 gram. b By Mayor's method. 

Albuminoid ammonia (not included in summation) 0.00001 g.

(46)
GOOCH AND WHITF1KLU. JJESULTS OF ANALYSIS. 47

Hypothetical combination.

Constituents.

Nruci... ...

LiCl.........

KC1 .........

Nad. .......

NazS04 ......

CaS04. ......

NaA aOs .....

Na2~B407 .....

MgCOs .....

CaCOs. ......

Al«-O->

SiO« .........

HaS..........

G rams pr.r kilo 

of water.

0.0133

0. 1039

0. 9738

0.0300

0. 0037

0. 0050

[0. 0394]

0. 0031

0.0133

0.0059

0. 4G36

Trace

[1.6C22]

Percent, of total material 

in solution.

0.03

0.80

6.26

58.59

2.21

0.22

0.30

[2. 37]

0.18

0.80

0.35

27.89

[100. 00]

An accidental loss of the material for analysis prevented the determinations 'of the 

boric acid, bromine, iodine, calcium, and rubidium. In the figures given above it 

has been assumed, in order that the analysis may be utilized as far as may be for comparison with the others, that the boric acid was present in amount just sufficient to 

neutralize the excess of base over all acid in the dissolved material. This supposition is probably not very far wrong, if we may draw any conclusion in this matter 

from the composition of adjacent waters, but it is nevertheless purely an assumption.

(47)
48 WATERS OF YELLOWSTONE NATIONAL PARK.

CONSTANT GTCYSEU.

[BULL. 47.

(Locality, Norris Basin; date of collection, September 13,1835; temperature, 92° C.; 

reaction, acid; specific gravity, 1.00115.)

Constituents.

SiOz... ......

SOi. .........

C02 . .........

BzOs. ........

AsaOs........

Cl. ........

Br...........

HzS..........

O(basic). ... 

Fo. ..........

Al ...........

Ca. ..........

Mull. ...........

Na.. .........

Li............

NH4 . ........

H(inHCl)...

Grains per kilo 

of water.

0. 4685

0. 0923

0.0155

0. 0317

0.0018

0. 5740

0.0185

0.0146

0. 0018

0. 0745

0.3190

0. 0030

0.00127

0. 0008

1. 62207

Percent, of total material 

in solution.

28.88

5.69

0.95 '

1.95

0.11

35.39

1.14

0.90

0.11

4.60

19.67

0.19

0.08

.05

100.00

Determinations.

2

2

9

0

2

1

2

2

2

2

2

2

2

1

Grams of water 

employed in 

each determination.

200

200

200

500

500

200

. 100

600

200

200

200

200

200

200

200

50

a As received in the laboratory. 

Albuminoid ammonia, none.

Hypothetical combination.

Constituents.

NHiCl...... 

LiCl. ........

KC1... .......

KBr .........

NaCl. ...... 

NajSOa ...... 

MgSth. ......

CaS04 .......

Ah(S04)3....

Fe2 (SO.i)3 .... 

SiOz .........

BsOs .........

As203........

COz.... ......

HC1..........

Grams per kilo 

of water..

0. C038 

0. 0182

0. 1423

0. 7590 

0. 0635 

0. 0090

 0. 0490

0. 0304 

Trace 

0.4C85

0.0317

0.0038

0. 0155

0. 0287

1. 6220

Per cent, of total material 

in solution.

0.23 

1.14

8.77

46.79 

3.91 

0.55

 3.07

1.88 

28.88

].95

0.11

0.95

1.77

ioo. oo

(48)
GOOCH AND WJ1ITF1EUX] RESULTS OF ANALYSIS. 49

CO.UAL SPKIXG.

(Locality, Norris Geyser Basin; date of collection, August 20, 1884; temperature, 

73° C.; reaction, acid; specilio gravity, 1.00130.)

Constituents.

SiOz.........

80s. .........

co»..........

. B20s ..-....-

AsgOs ........ 

Cl ..........

H«S..........

0 (basic)..... 

Fe...........

Al. ..........

C«

Mg ..........

K. ...........

JSa,. ..........

Li ...........

isriTj .........

H(innCl)...

Grams per kilo 

of water.

0. 6070

0. 0264

0. 0425

O nooQ

0. 0007

0 7flC7

0. 0053

0 00^9

0. 0022

0. 0729

0. 0020

0. 0022

1. 91082

Per cent, of total material 

in solution.

a 1.77

9 2°

1.71

0.04 

37.09

0.28

0 15

0. 11

3

0-1

20. 60

0.11

0.02

0.17

100.00

Determinations.

2

2

I

0

n

2

1

Grams of water 

employed in 

eacli cietermiwatiou.

200

200

200

1,000

3,000 

100

600

200

200

200

100

100

100

50

Albuminoid ammonia (not in summation), 0.00010 grams per kilo.

Hypothetical combination.

ConstituentsLT H4C1. ...... 

LiCl. ........

KC1 .........

NaCl ........

MgClz. ......

AlsClc. ......

ITeaCls.......

MsfSO*. ......

CaSO.i .......

E-iO:i .........

AssOa. .......

SiOz.........

CDs. .........

EC1 ... .....

Grams per kilo 

of water.

0. 0012 

0. 0121

0. 1393

1.0011

0.0016

0.0143

0.0328

0. 0007

0.6070

0. 0425

0.014:3

1. 9108

Percent, of total material 

in solution.

O.OG 

0 64

7 90

rjo 39

0.03

O ^K

0.46

1 QO

t 72

0.0-1

31.77

2.22

0.76

100. 00

Bull, 47-

(49)
50 WATERS OF YELLOWSTONE NATIONAL PARK.

CORAL SPRING.

[BULL. 47.

(Locality, Norris Geyser Basin; date of collection, October 11, 1886; temperature, 

72° C.; reaction, faintly acid; specific gravity, 1.00124.)

Constituents.

Si02 .........

SO...........

co2 . .........

B203 . ........

Cl. ..........

H2S.... ......

O(basic) ..... 

Ee...........

Al...........

Ca..........

Mg .........

K.. ..........

Na...........

Li...........

NH4 . ........

Grams per kilo 

of water.

0. 5805

0. 0280

0. 0262

0. 03C8

0. 0009

0. C701

0. 0175

0. 0077

0. 00-71

0. 0014

0. 0815

0. 3925

0. 0040

0. 0003

1. 8545

Per cent, of total material 

in solution.

31.30

1.51

1.41

1 98

0.05

36.14

0.94

0.42

0.39

0.07

4.40

21.16

0.21

0,02

100. 00

Determinations.

2

2

2

2

2

2

1

2

2

2

2

2

2

2

1

Grams of water 

employed in 

each determination.

200

200

200

500 .

500

200

COO

200

200

200

200

200

200

200

50

Albuminoid ammonia (not in summation) 0.00060 gram per kilo.

Hypolihctical combination.

Constituents.

NH4C1. ......

LiCI ........

: KCI .........

NaCl ........

NasSCu ...... 

MgS04 ...... 

CaS04 .......

:Na2B407 ..... 

NaAs02 . ... 

CaC03 . ......

A120S ........

Fe203 ........

Si02 .........

C02 ... ......

Grams per kilo 

of water.

0. 0009

0. 1557

0. 9483

0. 0228 

0. 0070 

0. 0179

0. 0031 

0. 0012 

0. 0048

0. 0139

Trnpn

0. 0241

1. 8545

Per cent, of total material 

in solution.

0.05

1 *?1

o on

R1 11

1.23 

0.39 

0.96

2.86 

0.07 

0.26

0

7K

01 OA

1 30

100. 00
GOOCF1 AND WHITKIELU. RESULTS OF ANALYSIS. 51

ECHINUS SPRING.

(Locality, Nofris Geyser Basin; date of collection, August 20, 1884; temperature, 

91° C.; reaction, acid; specific gravity, 1.00071.)

Constituents.

SiOs .........

s<v .........

CCh ..........

BiOs .........

Cl ...........

Br.... .......

HzS.... ......

O(basic) ..... 

Fo. ...... ...

Al ..........

Mg. .........

K. ...........

Li ...........

NH4 . ........

H(inHCl) ..

Grams per kilo 

of water.

0. 2532

0. 0173

0.0016

0. 1207

Trace

0. 0386

0. 0027

0. 0115

0 0395

0. 1265

0. 00106

0. 0007

0. 8312C

Percent, of total material 

in solution.

30.46

23.21

2.08

0.10

14.52

4.64

0.33

1.38

15.22

0.13

0.08

100. 00

Determinations.

2

2

2

2

2

2

2

1

2

2

2

2

2

2

1

Grama of water 

employed in 

each determination.

200

200

200

500

500

200

100

COO

200

200

200

200

200

50

Albuminoid ammonia: None.

Hypothetical combination.

Constituents.

NH4C1 .......

LiCl..... ...

KCl .........

KBr ........

NaCl ........

NazSlfc ...... 

CaSOj . ..... 

A12 (S03 )4 .... 

SiO* .........

BA-. .......

As203 . .......

CO...........

HC1 .........

HjS.... ......

Grams perkilo 

of waier.

0 (\7~\d.

Trip A

0. 0908

0. 2803 

0. 0391 

. 0. 0171 

0. 2532

0. 0173

0. 0016

0 0^50

0. 0275

0. 8313

Percent, of total material 

in solution.

0.48

0 07

10.92

33.72 

4.70 

2.06 

30.46

2.08

0 19

3 01

3.31

100. 00

(51)
52 WATEKS OF YELLOWSTONE NATIONAL PAKK.

^

SCHLAMMKKSSEL.

[BULL. 47.

(Locality, Norris Geyser Basin; date of collection, August 20, 1834; temperature, 

91° C.; reaction, acid; specific gravity, 1.00130.)

The water was filtered from material in suspension.

Constituents.

Si02 .........

<s n

coz .... ......

B203 .........

AS203 . .......

01............

Br ...........

H2S..........

0 (basic) ..... 

Fe......... ,

A1 $

Ca...........

M> ..........

K...... ......

Na. ..........

Li ...........

KET4 .........

H (in HC1) . . .

Grams por kilo 

of water.

0. 4577

0.1012

0. 0175

0. 0390

0. 6391

0. 0202

0. 0081

0. 0078

0. 0254

0. 3C54

0. 0020

0. 00633

0.0019

1. 69283

Percent, of total material 

in solution.

27.04

5 no

1.04

9 <*n

37 7^1

1.10

0.48

0.46

0.02

1.50

91 ro

0.17

0

07

0.12

100.00

Determinations.

2

9

1

2

1

2

2

2

2

Grams of water ' 

employed in 

each determination.

200

100

100

200

200

100

100

200

200

200

200

50

a As received in the laboratory. 

Albuminoid ammonia (not in summation) 0.00040 grams per kilo.

Hypothetical Combination.

Constituents.

TSTH4C1 .......

LiCl.........

KC1 .........

KBr...... ...

NaCl........

Na2S04 ...... 

MgSOj ...... 

CaSC-4 ...... 

A12(S04) 3 -- ) 

Fe2 (S04) s - - 5 

SiOs. ......... 

B«0s. ........

coz. .........

HC1.... ......

HsS..........

Grams per kilo 

of water.

O fll Qft

0. 0176

0. 0485

0.8585

0. 08G2 

0. 0015 

0. 0205

0.0513

0. 4577 

0. 0390

0. 0175

0. 0697

Trace

1. 6928

Percent, of total material 

in solution.

1.11

1 fl3

2.86

50.72

5.09 

0.09 

1.57

3.03

27. 04 

2.30

1.04

4.12

100. 00

(52)
GOOCn AND WH1TFIE.LD.] RESULTS OF ANALYSIS. 53

FOUNTAIN GEYSER.

(Locality, Lower Geyser Basin; date of collection, August 24, 1884; temperature, 

82°C.; reaction, alkaline; specific gravity, 1.00100.)

Constituents.

SiOj ..... - -

TiO«.........

SOj ..........

CO,... .......

NzOs.........

p2 o*..... ...

B*0S .' .......

AasOs. .......

Br ..........

1 ............

PI ...........

HsS..........

TV

Al ...........

Mn ..........

"Rn

Sr ...........

Ca. ...... ....

Mg ..........

Cs...........

lib..........

K... .:......

N.I...;. ......

NH4 . ........

Grams per kilo 

of water.

0.3315

0. 0195

0. 2307

0. 00004

0. 0027

0. 3337

'P tin ft A

0. 0002 .

0. 0057

0.0014

0. 0010

0. 0379

'0.3522

0. 00015

1. 39979

Per cent, of total mateiial 

iu solution.

23.69

1.39

Hi. 48

0. 99

0.19

23. 84

0.03

0.01

0.41

0.10

0.07

2.71

25. 16

0. 25

0.01

100. 00

Determinations.

0

1

2 

o

1

I

o

2

2

2

2

1

1

0

2

1

1

1

2

o

2

2

2

0

2

Grams of water 

in each determination.

200

31,000

200

200

500

31,000

6,200

6,200

100

6,200

6,200

31, 000

600

31, 000

200

31, 000

31, 000

31, 000

200

 200

0,200

0, 200

100

100

6,200

500

a By Mariguac's method, b 0. 000003. grains. cBy Mayor's method. 

Alouminoid ammonia (uot in summation) 0.00033 grams per kilo. 

Hypothetical combination.

Constituents.

NHiCl.......

LiCl.........

JICl .........

KBr.........

NaCl ........

NanSCh .....

Na!iB4 Oj .....

NaAsOs .....

NazCOs......

MgCOa ......

CaCOs.......

FeC03 .. ...

MnC03 ......

A1.20, ........

SiOz. ........

COi. .........

H»S..........

Grams per kilo 

of water.

0. 021 3

0. 0720

(i. 4G3fi

0. 034 G

0. 0198

0. 0035

0. 3541

0. 0035

0. 0035

0. 0004

Trace

0.0108

0. 3315

0. 0801

1. 3997

Per cent, of total material 

in solution.

0.02

1.52

33.12

2.47

1.42

0.25

25. 30

0.25

0.02

0.77

. 23. 69

5.73

100. 00

(53)
54 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

GREAT FOUNTAIN GKYSER.

(Locality. Lower Geyser Basiu; date of collection, August 24, 1884; temperature, 

82°-93° C.(«); reaction, alkaline; specific gravity, 1.00104.)

Constituents.

SiOz .........

S03 ...- ......

C02 ..........

B2 03 ........ 

AssOs..--. --

Cl ...........

K3S. .........

0 (basic)..... 

Fe...........

Al. ..........

Ca...........

Mg. .........

K........ ..

Na.... .......

Li ..........

Grams per kilo 

of water.

0. 3182

0.0187

0.2107

0.01006 

0. 0017

0. 3508

0. 0472

0. 0021

0. 0017

0, 0023

0.0145

0.3351

0. 0025

1.3155

Percent, of total material 

in solution.

24.19

1.42

1U.02

0. 76

0 1 3

26.67

3.59

0.16

0.13

0.17

1.10

25.47

0.19

100. 00

Determinations.

2

2

2

1

o

2

2

2

2

2

2

2

2

Grams of water 

employed in 

each determination.

2CO

100

200

50 

500 -

100

600

200

200

200

200

'100

100

100

a The usual range of temperature during the interval between eruptions.

b Heats on one determination, and that made with an insufficient amount of water, the remainder 

having been lost accidentally.

Hypothetical combination.

Constituents.

LiCl...-. .

KC1 ........

NaCl .......

!Na2S04 .....

NasB-tO? ....

NaAsOj' .....

NaaCOs......

MgCCh.....

CaC03......

AlsOs. .......

reao3 .......

' SiOz.. ......

COa..........

Grains per kilo 

of water.

0.0152

0.0277

0.5354 .

0. 0332

0. 0144

(1. 0022

0. 2536

0. 0080

0. 0043

0. 0040

Trace

0.3182

0. 0993

1. 3155

Percent, of total material 

in solution.

1.15

2.11

40.70

2.52 

1.09

0.17

19.28

0.61

0.33

0.30

24.19

7.55

10U.OO

(54)
GOOCH AND WHITFIEUU. RESULTS OF ANALYSIS.

I1YGEIA SPRING.

(Locality, Lower Geyser Basin; date of collection, September 11,1885; temperature, 

43° C.; reaction, alkaline; specific gravity, 1.00107.)

a As received in t.he laboratory. 

Albuminoid ammonia, none.

Constituents.

SiO».... ......

S03 ..........

COz. .........

B203 - ........

AssOs. .......

ci. ..........

Br. ..........

H*S'.... ...... 

0 (basic). ... 

Fe. ..........

Al..... .....

Mg.......... 

K...... ......

 M-q

Li ...........

Ntti.........

Gramsperkilo 

of water.

0. 2477

0. 0196

0. 2907

0. 0239

O ftlYM

 0. 2487

Trace

Noneo. 

0. 0504 

Nono

0. 0064

0. 0022 

0. 0154

0. 2654

0. 0032

0. 00021

1, 1808 1

Per cent, of total material 

in solution.

20.08

24. fc2

2.02

21.06

.....:

4.27

...... 

0 °1

0.54

0.19

oo ,jg

0.27

0.02

100. 00

Determinations.

9

o

2

2

2

"?.

2

2

2

Grams of water 

employed in 

each determination.

200

200

200

500

200

100

200

200

200

200

200

200

50

Hypothetical combination.

Corstitnents.

NHnCl. .....

LiCI ..........

KC1 .........

KBr. ........

 NTaCl .......

NasSOi ......

NlwBiOr .....

NaAsCh .....

NazCOs ......

MfiCO, ......

CaC03 .......

AhOa ........

SiOa ........

co»..........

Grains per kiln 

of venter.

0. 0006

0. 0194

0. 3594

0 0*^94

0. 0348

0. 0345

0. 0049

0. 2393

0. 0077

0. 0160

0.0068

0. 2477

0.1803

1. 1808

Percent, of total material 

iu solution.

0.06

j C4

30.44

2 49

2.95

2.92

0.41

20.26

0.65

1 ^P»

0.58

15 27

100. 00

(55)
56 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

MADISON SPRING.

(Locality, Terrace Springs, near junction of Gibbon and Firebole Rivers; date of 

collection, September 11, 1885; temperature, 60° C.; reaction, alkaline; specific 

gravity, 1.00100.)

Constituents.

Si02 .. ........

sos ..........

CO*.-.......

BjO.-. .........

Cl. ..........

Br. ..........

HsS.... ......

0 (basic) ..... 

Fo. ..........

Al...........

Ca. ..........

Mg ..........

Z.... .........

Na. ..........

Li ...........

2TH4. ........

Grama per kilo 

of water.

0. 1507

0. 0123

0. 6140

0. 0130

0. 0098

0. 1002

0. 0255

0.0017

0. 0385

0. 2930

0. Of 04

0.0008

1. 3259

Percent, of total material 

in solution.

n i7

0.93

46. 31

0.98

8.01

1.92

0.13

9 on

22.10

0.03

0.06 .

100. 00

Determinations.

f»

' 1

i

0

1

2

2

2

2

2

2

2

Grains of water 

employed in 

eacli determination.

200

500

500

200

100

200

200

200

200

200

200

200

50

a A.S received in the laboratory. 

Albuminoid ammonia (not in summation), 0.00020 grams per kilo.

Hypothetical combination.

Constituents.

3fH4Cl. ......

LiCl .........

KC1 .........

NaCl ........

Na-SOi.......

NnsBjO? .....

NaAsO^......

NasCOi ......

MgCOa.......

CaCO^.......

Si02 .... .....

C02 ..........

Grams por kilo 

oi' water.

0. 0024

0. 0024

0. 0735

0. 0513

0. 0218

0. 0187

Trace

0. 0025

0.0038

0.1507

0. 3328

1.3259

Percent, of total material

in solution.

0.18

0.18

5.54

3.87

1.65

1.41

45.44

0.45

481

11.37

25.10

100. 00
GOOCH AND WIIITF1ELD J RESULTS OF ANALYSIS. 57

FIREHOLE KIVER.

(Locality, above the junction of Nez Perc6 Creek; date of collection, August 24, 1884;

temperature, 8° C.; reaction, alkaline; specific gravity, 1.00031.) 

The water was filtered before bottling.

Constituents.

SiOj .. ......

Qn

COs... .......

BiOa .........

,01..... ......

UsS..........

O (basic) ..... 

Fe........ ..

Al. ..........

Ca. ..........

Mg ..........

K. ...........

Na. .....!....

Li ...........

Granisporliilo 

of water.

0. 0905

0. 0084

0.1010 '

0. 0060

0. 0737

0. 0265 

Trace

0. 0031

0. 0000

0. 0007

0.0170

0. 0930

0. 0011

0. 4306

Per cent, of total material 

in solution.

22 10

1.92

1.37

18.89

6.07

0.71

1.51

0.10

3. S9

21.30

0.25

100. 00

Determination.

f>

0

2

1

1

2

2

2

2

2

2

2

Grams of water 

employed in 

each determination.

100

200

340

500

100

200

200

200

200

100

100

100

Hypothetical combination.

Constituents.

LiCl. ........

KC1 ..... ..

NaCl ........

NazSCh .....'. 

NazBjO? ..... 

NaaCCb...-.- 

MgCOs.......

CaCOs- ......

AhOs........

Fe20s .......

SiOz .....

CO*. .........

Grams per kilo 

of water.

0. 0007

0. 0325

0. 0867

0. 0149 

0. 0087 

 0.1201 

0. 0024

0. 0105

0. 00,-i9

0. 0905

0. 4300

Percent, of total material 

in solution.

1 53

7.44

1Q Qf\

3. 42 

1.99 

27.51 

0.55

3.78

1.35

22. 10

10.47

100. 00

(57)
58 WATEKS OF YELLOWSTONE NATIONAL PARK. [BULL. 47.

EXCELSIOR GEYSER.

(Locality, Midway Basin; date of collection, August 25, 1884; temperature, 92C C.; 

reaction, alkaline; specific gravity, 1.00110.)

Constituents.

SiOii .........

TiOs. ........

SOs- .........

CCh..........

NsOs.........

P»0s. ........

BsOs- ........

AszOs........

Cl. ..........

Br ...........

I.............

Fl. ..........

H*S..........

O (basic) ..... 

Fe. ..........

Al. ..........

Mn ..........

Ba. ..........

Sr ...........

Ca. ..........

Mg ..........

Cs. ..........

Kb...........

K.... ........

Na. ..........

Li ...........

NH4 . ........

Grams per kilo 

of water.

0. 2214

0. 0146

0. 3825

0. 0161 a

0. 0026

0 97Q-1

0. 0055 

0. 0018

0. 0012

0. 0022

0. 0022

0. 0325

0. 4186

0. 0020 6

0. 00001

1. 47251

Percent, of total material 

in solution.

15. 04

0.99

9f. Q7

1.09

0.18

18. 96

6.49 

0.12

. 0.08

0.15

0

1 C

2.21

28.43

0.14

100. 00

Determination.

2

1

2

2

2

1

2

9

9

2

1

1

2

2

1

1

1

2

9

2

2

9

Grams of water 

employed in 

each determination.

200

24, 000

200

200

120

24, 000

2,400

2, 400

100

2,400

2,400

24, 000

600

24, 000

200

94 Oflfi

24, 000

24, 000

200

200

2,400

2,400

100

2,400

a By Marignac's method. I By Mayor's method.

Albuminoid ammonia (not in summation), 0.00002 gram per kilo.

(58)
GOOCH AKD WH1TP1ELD.J RESULTS OF ANALYSIS. 59

Hypothetical combination.

Constituents.

NttiUl. ......

 Lid .........

KCL... ......

KBr. ........

NaCl ........

NaaS04 ...... 

Na2B407..... 

NaAsOj ..... 

Na2HP04.... 

NasCOs...... 

MgCOs ...... 

CaCOs .......

FeCO, .......

Ah03 . .......

SiOz. ........

C0». .........

HzS..........

Grams per kilo 

of water.

Trace

0.0121

0. 0621

0. 3948

0. 0259 

0. 0232 

0. 0034 

Trace 

0. 5739 

0. 0077 

0. 0055

0. 0037

0. 0023

0. 2214

0. 1365

Tract?

1. 4725

Per cent, of total material 

iu solution.

Trace

0.82

4.22

26.81

1.76 

1.58 

0.23

38.97 

0.52 

0.37

0.25

ft 11

15.04

9.2(J

100. 00

A preliminary sample of 600 cm3., taken August 29, 1883, yielded as analysis the 

following figures, which signify grams of material per kilogram of water: Si02 , 

0.2727; SO3, 0.0107; B3O3, present; 01, 0.2765; Fe and Al, 0.0009; Ca, 0.0055; Li, 

present.

(59)
60 . WATERS OF YELLOWSTONE NATIONAL PARK. [BULU 47.

OLD FAITHFUL GEYSER.

(Locality, Upper Geyser Basin ; date of collection, September 1, 1884 ; teraperatare, 

84°-88c C. (a); reaction, alkaline ; specific gravity, 1.00096.)

Constituents.

SiOz. ........

TiO«. ........

80s ..........

COz.. ........

NjOs.........

P20S .........

E203 .........

AszOs ........

Cl ...........

Br ...........

I.............

M ...........

H2S..........

0 (basic)..... 

Fe. ..........

Al...........

Mn ..........

Ba... .......

Sr ...........

Ca...........

Mg ..........

Cs. ..........

Kb...........

K.... ........

Li ...........

NH4 . ........

Grams per kilo 

of water.

0.3828 -

0. 0152

0. 0894

Nouo

0. 01486

0.0021

0. 4391

0. 0034

None

None 

0. 0002

0. 0419

0. 0009

0.0015

0. 0006

Trace

0. 02G7

O.OOSGd

0. 00001

1. 39081 

Percent, of total material 

in solution.

97 ^9

1 09

6 43

1.07

0.15

o i C7

0 9*

0.01

3.02

0.06

0.11

0.04

1.92

26.36

.40

100. 00

Determinations.

n

i

2

2

o

1 .

9

2

2

2

9

1

1

2

2

1

1

1

2

2

2

2

2

2

2

1

Grams of water j 

employed in 

each determination.

500

84, 000

1,000

200

1,500

84, 000

13, 500

13, 500

200

13, 500

13, 500

84, 000

600

84, 000

500

84, 000

84, 000

84, 000

500

500

27, 000

27, 000

200

200

13, 500

50

a The usual range of temperature in the pools about the crater, from which 

the sample was taken immediately after eruption. 

6 By Marignac's method, 

c 0.000005 grams. 

(I By Mayer's method.

Albuminoid ammonia (not in summation), 0.00002 grams per kilo.

(60)
GOOCII AND WHlTl'lELD.l RESULTS OF ANALYSIS. 61

Hypothetical combination.

Constituents.

NH4C1. ......

LiCl.........

KC1.. ........

KBr ..........

CsCl. ........

KbCl .......

Nad.........

NasSOi...... 

N2 aB4 07 ..... 

NaAsOa...... 

NazCOs...... 

NasSiOa ...... 

HgCOa........

CaCOs.......

FeC03 ....... 

MiiCOs ...... 

AljOa ........

SiOz .........

HjS.........

Grams per kilo 

of water.

0. 0340

0. 6393

0. 0178

0. 0051

0. 0270 

0. 0213 

0. 0027 

0. 2088 

0. 0279 

0. 0021

0. 0038

Trace 

Trace

0. 0002

1.3908

Percent, of total material 

in solution.

2.44

45.97

3.44

0.37

1.94 

1.53 

0.19 

15.02 

2.01 

0.15

0.27

0.12

26. 54

0.01

100. 00

(61)

ERRATA. -

OLD FAITHFUL GEYSER HYPOTHETICAL COMUINATION. 

Corrections in above table.

For KC1 read NaCl 

" KBr " KC1

" NaCl " KBr
62 WATERS OF YELLOWSTONE NATIONAL PARK. [BULL, 47.

SPLENDID GEYSER.

(Locality, Upper Geyser Basin; date of collection, September 10,1885 ; temperature,

93° C.; reaction, alkaline; specific gravity, 1.00132.) 

The concentration of the water was effected in porcelain.

Constituents.

SiOz... .......

TiOa.........

b03 ..........

co2 . .........

NsOs.- .......

PsOs. ....-'...

B203 . ........

Cl ...........

Br.... .......

I.............

Fl ...........

H2S... .......

0 (basic) ..... 

Fe...........

Al...........

Mn ...........

Ba...........

sr. ......:...

Ca.... .......

Mg ..........

Cs ...........

Kb...........

K ...........

fjn

Li...........

NH4 .........

Grams per kilo 

of water.

0. 2964

0. 0158

0. 4225

0. 00012

0. 0234

0.0019

0. 3227

0. 0897 

0. 00008

0. 0027

0. 0030

0. 0005

0. 0121

0. 4407

0. 0023

0. 00008

1. 63398

Per cent, of total material 

in solution.

18.14

0.97

25.86

0.01

1.43

19.75

5.49 

0.005

0.16

0

1 Q

0.03

1

0.74

26.97

0.14

0.005

100. 000

Determinations.

2

1

2

2

9.

1

2

2

2

2

2

1

1

2

2

I

1

0

2

2

2

o

0

1

Grams of water 

employed in 

each determination.

500

22, 000

500

200

400

22, 000

500

200

4,500

4,500

22, 000

. COO

22, 000

500

22, 000

2O HAH

500

9,000

200

200

200

KA

Albuminoid ammonia (not in summation), 0.00002 grams per kilo.

(62)
OOOCIl AND WHITl'IELD.' RESULTS OF ANALYSIS. 63

Hypothetical combination.

Constituents.

NH^Cl.......

LiCI.........

KC1 .........

NaCl ........

Na2SO.........

]STa2Bj07 .....

.NaAsOj .....

Na2HP04 ....

NajCOs......

MgC03 ... 

CaC03 .......

I'eCOg. ......

 A1203 . .......

Si02 .........

CO,.. ....... .

Grams per kilo 

of water.

0. 0002

0. 0140

C. 0231

0. 4940

0. 0281

0. 0335

0. 0025

0. 0002

0. 5280

0. 0018

0. 0075

0. 0001

0. 0051

0. 2904

0. 1989

1. 6340

Percent, of total material 

in solution.

0.01

0.86

1.41

on f>*>

1.72

2.05

0.15

0.01

32.36

0.11

o;46

0.01

0.31

18. 14

12.17

100. 00

(63)
64 WATERS OF YELLOWSTONE NATIONAL PARK, [BULL. 47.

SPLENDID GEYSER.

(Locality, Upper Geyser Basin; date of collection, August 28, 1884; temperature, 

93° C.; reaction, alkaline ; specific gravity, 1.00127.)

Constituents.

Si02 . ........

so3 .........

CO...........

T> f\

Cl ...........

Br.... ......

H2S.........

0 (basic) .... 

Fe. ...........

Al.... .......

Ca.... .......

Mg..........

K. ...........

Na.... .......

Li ...........

NH4 . .'.......

Grams per kilo 

of water.

0. 3000

0.0158

0. 4042

0. 0240

0.0010

0.318L

0. 08GG

0. 0034

0. 0034

0.00] 5

0. 0152

- 0.4179

0. 0037

0. 00042

1. 59522

Percent, of to 

tal material 

in solution.

18.81

0 99

25. 34

0.00

19.94

5.43

0.21

0.21

0.09

0.95

26.20

0.23

0.03

100. 00

Determinations.

2

2

2

2

o

1

2

2

o

2

2

2

2

2

Grams of water 

employed in 

each determination.

200

100

200

500

500

100

100

GOO

200

200

OAA

200

100

100

100

50

Albuminoid ammonia, (not in summation) 0.00020 grams per kilo.

Hypoilictical combination.

Constituents.

NH4C1.......

' LiCl .........

KC1.... ......

NaCl. ........

!Na2S04 .......

Na2B407 ..... 

NaAs02 ...... 

jSTa2C03 ...... 

MgC03 ...... 

CaC03 .......

Al20a - .......

Si02 ..........

co2 ... .......

Grams per kilo 

of water.

0. 0012

0. 0290

0. 4G92

0. 0280

0. 0346 

0.0010 

0.4977 

0. 0053 

0. 0085

0. 0004

0. 3000

0. 1912

1. 5952

Per cent, of total material 

in solution.

0.08

1.41

1.82

29.41

1.76

2.17 

0.10 

31.20 

'O. 32 

0.53

0.40

18.81

11.99

100. 00

(64)
GOOCH AND WHITFIELD.J RESULTS OF ANALYSIS, 65

GIANTESS GEYSER.

(Locality, Upper Geyser Basin; date of collection, August 29, 1884; temperature, 

93° C.; reaction, alkaline; specific gravity, 1.00100.)

Constituents.

Si02 .........

on

COj..........

T> f\

n

Br. ..........

TT Q

0 (basic) .....

TV

Al

, Ca... ........

Mg ..........

K...... ......

TO-j,

Li...........

NH4 ."........

Grams per kilo 

of water.

0. 3917

0. 0167

0. 1055

0. 0233

0. 0006

0. 4408

0. 0411 

Trace

0. 0049

0. 0007

0.0012

0. 0410

0. 3451

0. 0057

1.4183

Per cent, of total material 

in solution.

27.62

1.18

7.44

1 fid

0.04

31.08

2,90

0.34

0.05

0.08

2.00

24. 33

0.40

100. 00

Determinations.

2

2

2

o

2

1

2

2

Grams of water 

employed in 

each determination.

200

Oflfk *

200

200

200

100

100

600

200

200

200

200

100

100

100

Hypothetical combination.

Constituents.

LiCl. ........

KC1 .........

KBr. ........

MaCl . .......

NajSOa...... 

Na^O, ..... 

NaAsOa. .... 

NaaCOs...... 

MgCOs ...... 

CaCOa. ......

A1203 -- 

SiOa .........

CCb..........

H3S. .........

Grams per kilo 

of water.

0. 0346

0. 0783

0. 6173

0. 0296 

0. 0336 

0. 0008 

0. 1959 

0. 0042 

0. 0017

0. 0093

0. 3917

0. 0213

1. 4183

Per cent, of total material 

in solution.

2.44

5.52

« w

2.09 

2.37 

0.06 

13.81 

0.30

0 19

nij g*n

1 ^A

*

100. 00

The analysis of a preliminary sample of 1,300 cm3 ., taken August 28, 1883, yield 

the following results, which are given in grams of material per kilogram of water: 

Si02, 0.3843; SOa, 0.0144; Cl, 0.4384 ; Fe and Al, 0.0030; Ca, 0.0058; Mg, 0.0002; Li, 

0.0043; Na and K, weighed together as chlorides, 0.9559. The chlorides of the 

sodium and potassium found in the preceding analysis amount to 0.9564 gram.

(65) 

Bull, 47 5
66 WATERS OF YELLOWSTONE NATIONAL PARK.

BEEHIVE GEYSER.

(Locality, Upper Geyser Basin; date of collection, September 1,1884; temperature, 

93° C.; reaction, alkaline; specific gravity, 1.00095.)

Constituents.

SiCb. ........

SOs..........

COs..........

BsOs. ........

As=0s. .......

Cl ...........

Br. ..........

H2S..........

0 (basic) ..... 

Fe. ..........

Al. ..........

Ca. ..........

Mg... .......

K.... ........

Na...........

Li ...........

NH4- ........

Grams per kilo 

of water.

0 3019

0. 0271

O flQ9n

0. 0145

0. 0011

0. 3894

0. 0364

0.0029

O nn^Q

0. 0002

O noiQ

0. 3118

0. 0061

0. 00021

1. 21111

Per cent, of total material 

in solution.

91 19

2.24

7. CO

1.20

0.09

Q9 11

3.00

0.24

O qo

0.02

1.76

95 71

0.50

0.02

100. 00

Determinations.

2

2

2

1

2

2

0

2

Grams of water 

employed in 

each, determination.

200

100

200

500

500

100

100

600

200

200

2GO

200

100

100

100

Albuminoid ammonia, none.

Hypothetical combination.

Constituents.

NKiCl. ......

LiCl. ........

KC1 .........

KBr. ........

NaCl ........

Na2S04 ......

Na2B407 .....

NaAsOz .....

NasCOa......

MgCOs ......

CaCOs. ......

AlsOs. .......

SiOz- ........

CO?.... ......

Grams per kilo 

of water.

0. 0006

0. 0407

0. 5582

0. 0481

0. 0209

0. 0014

0. 1754

0. 0007

0. 0098

0.0055

0.3042

0. 0086

1. 2111

Percent, of total material 

in solution.

0.05

3

(\K

6.36

46 09

3.97

1.73

0.12

14.48

0.06

0.8"!

O n

25.12

0.71

100. 00

(66)
RESULTS OF ANALYSIS. 67

GROTTO GEYSER.

(Locality, Upper Geyser Basin; date of collection, August 28, 1884; temperature, 

93° C.; reaction, alkaline; specific gravity, 1.00120.)

Constituents.

SiO* .........

SOa.... ......

CO*. .........

BjOa. ........

Cl ...........

Br. ..........

as..........

0 (basic) .....

re...........

Al. ..........

Ca. ..........

Mg ..........

K...... ......

tfa...........

Li..........

NH4. .......

Grams per kilo 

of water.

0. 2590

0. 0148

0.3155

0.0290

0. 0003

0. 3045

None

0. 0807

0. 0036

0. 0039 

0. 0010

0. 0249

0. 3853

0. 0041

0. 00023

1. 42683

Per cent, of total material 

in solution.

18.15

1.04

22.11

2.03

0.02

21.34

5.66

0.25

0.28

0.07

1.74

27.00

0.29

0.02

100. 00

Determinations.

2

2

2

2

2

2

2

1

2

2

2

2

2

2

2

1

Grams of water 

employed in 

each determination.

200

100

200

£00

500

100

100

600

200

200

200

200

100

100

100

50

Albuminoid ammonia (not in summation) 0,00010 gram per kilo.

Hypothetical combination.

Constituents.

JTEUCr.......

LiCl.- .......

KC1 .........

KBr. ........

KaCl........

tfasSOi ......

Na2B407..-..

NaAs02 .....

K"a2C03 ......

MgCOa ......

CaCOa. ......

AbOs. .......

SiOz .........

C0»..........

Grams per kilo 

of water.

0. 0007

n n9do

0. 0476

0. 4293

0. 0263

0. 0418

0. 0004

0. 4573

0. 0035

O fiftQ7

0. 0068

0. 2590

0. 1195

1.4268

Per cent of total material 

in solution.

0.05

1 7S

3

ni

80.09

1.84

2.93

0.03

32.05

0.25

0.47

IS 1 f\

8

07

100. 00

(67)
68 WATERS OP YELLOWSTONE NATIONAL PARK. [BULL. 47.

TURBAN AND GRAND GEYSERS.

(Locality, Upper Geyser Basin; date of collection, September 1, 1884; temperature, 

91° C.; reaction, alkaline; specific gravity, 1.00108.)

The vents of these geysers connect with one another.

Constituents.

Si02 .........

S03... .......

co»..........

BaCh. ........

AsaOa. .......

Cl ...........

Br. ..........

H2S. .........

0 (basic) ..... 

Fe...........

Al...........

Ca...........

Mg ..........

K...... ......

Na...........

Li ...........

NH4. ........

Grams per kilo 

of water.

0. 3035

0. 0218

0. 1950

0. 0243

0. 0011

0. 3767

Trace

0. 0596

0. 0032

0. 0028

0. 0167

0.3818

0. 0036

0. 00042

1. 39052

Percent, of total material 

in solution.

21.83

1 Wl

14.02

1 7^

0.07

27.09

4.28

0.25

0.20

1.20

27.46

0.25

0.03

100. 00

Determinations.

O

2

2

2

2

2

1

2

2

2

2

2

2

1

Grams of water 

employed in 

each determination.

200

100

200

500

500

100

100

600

200

200

200

200

100

100

100

50

Albuminoid ammonia (not in summation) 0.00020 gram per kilo,

Hypothetical combination.

Constituents.

NHC1

LiCl. ........

KC1 .........

KBr. ........

NaCl. .......

Na2B407 .....

liTaAsOz .....

NaaCOs......

MgC03 ......

CaC03 . ......

Si02 .........

C02 . ..........

H2S.... ......

Grams per kilo

of water.

0. 0012

0. 0319

0. 5643

0. 0387

0. 0350

0. 0014

0. 3209

None

0. 0070

0. 0061

0. 3035

0. 0587

1. 3905

Percent, of total material 

in solution.

0.08

2 90

2.79

2.52

0.10

23.08

......

0.50

0.43

21.83

4.22

100. 00

(68)
RESULTS otf ANALYSIS.

ARTEMISIA GEYSER.

(Locality, Upper Geyser Basin; date of collection, September 1, 1884; temperature, 

89° C.; reaction, alkaline; specific gravity, 1.00121.)

Constituents.

Si02 .........

SOs. .........

COj.... ......

B203 - ........

Cl ...........

Br...........

H2S. .........

O(basic) ..... 

Fe...........

Al.... .......

Ca...........

Mg ..........

K.... ........

Na...........

Li...........

NHa. ........

Grams per kilo 

of water.

0 9707

0. 0127

0. 3607

0. 0177

0. 0014

O OQQfi

Trino

0. 0903 

Trip ft

0. 0014

0. 3988

0. 0070

0. 00021

1. 48771

Per cent, of total material 

in solution.

ia 30

0.85

24.24

1.19

0.09

9ft 13

6.06

0.09

1 flQ

9fi CA

0.47

0.01

100. 00

Determinations.

2

2

2

2

2

2

2

1

2

2

2

2

2

2

0

1

Grams of water 

employed in 

each determination.

200

100

200

500

500

100

100

600

200

200

200

200

100

100

100 .

50

Albuminoid ammonia, trace.

Hypothetical combination.

Constituents.

NH4C1. ......

Lid ......

KC1- ........

KBr.........

NaCl ........

NajSOa ......

Na2B407 .....

NaAsOa .....

Na2CO«......

MgCOs......

CaCOs.......

AhOi........

SiOj. ........

COa... .......

Gf ams per kilo 

of water.

0. 0006

0. 0425

0. 0311

Trap A

0.4101

0. 0226

0. 0202

0. 0018

0. 5245

None

0. 0035

0. 0150

fl 9737

0. 1421

1. 4877

Percent, of total material 

in solution.

0.04

2.86

2.09

27.56

1.52

1.36

0.12

35.26

none.

0 9Q

1.01

18.40

9

KK

100. 00

(69)
OP tELLOWSTONE NATIONAL PARK.

TAURUS GEYSER.

(BULL. 4?.

(Locality, Shoshone. Basin; date of collection, July 20, 1887; temperature, 92° C.; 

reaction, alkaline; specific gravity, 1.00105.)

Constituents.

SiO». ........

SOa. .........

C03 . .........

BsOa.........

AszOs. .......

Cl ...........

Br.... .......

H2S. .........

Fe. ..........

Al. ...........

Mg ..........

K...... ......

Na...........

Li...........

NH4 .. .......

Grams per kilo 

of water.

0 9Q9R

O nooct

0 391 ft

0.0149

0. 0007

0. 1935

0. 0781

0. 0040

0. 0009

O fiOQK

0. 3202

0. 0009

0. 0010

1. 2898

Per cent, of total material 

in solution.

99 fid

9 QS

9<1 8Q

1.16

0.05

15.00

C.05

0^31

0.07

1.82

24.83

0.07

0.08

100. 00

Determinations.

2

2

2

2

2

2

2

2

2

2

2

2

Grams of water 

employed in 

each determination.

eriA

200

200

1,000

1,000

200

100

500

500

500

500

200

200

200

50

Albuminoid ammonia, 0.0002 grams per kilo.

Hypothetical combination.

Constituents.

NKjCl.......

LiCl. ........

KC1. ........

NaCl .......

NazSOi ....... 

MgSOa. ......

NazBiO? ..... 

NaAsOa...... 

NajSiOa...... 

SiOz. ........

COa. .........

AlzOj........

FejOs. .......

Grams per kilo 

of water.

0. 0030

0. 0055

0. 0449

0. 2729

0. 0630 

0. 0045

0. 0215 

0. 0009 

0.4971 

0. 0480

0. 3210

0. 0075

Trace

1. 2b98

Per cent, of total material 

,in solution.

.24

.43

3.48

91 1 ^

4.88 

.35

1.67 

.07 

38.54 

3.72

9d fid

.58

100. 00

(70)
COOCtl AND WHITFIELD. 1 RESULTS OF ANALYSIS. 71

ASTA^ SPRING.

(Locality, Hillside Springs; date of collection, September 16,1884; temperature, 84°C.;

reaction, alkaline.)

Constituents.

SiOj .........

SOa..........

CO-2.... ......

B203 . ........

AssOs .......

Cl ...........

Br ...........

HsS..........

O (basic) .... 

F6 J......... A i

Ca. ..........

Mg ..........

K...... ......

Na. ..........

Li ...........

Grams per kilo 

of water

0. 1650

0. 0324

0. 1800

0. 0947

0. 0392 

0. 0059

0.0118

0. 0010

0. 0116

0. 1340

0. 0008

0. 6764

Per cent, of total material 

in solution.

24.40

d. 70

26.61

14.00

5.79 

0.87

1.75

0.15

1.72

19.80

0.12

100.00

Determinations.

1

1

1

1

1

1

1

1

1

1

Grains of water 

employed in 

each determination.

200

200

200

200

100

200

200

200

2CO

200

200

Hypothetical combination.

Constituents.

LiCl.........

KC1 .........

NaCl ........

NasS04 ......

NWBiO? .....

NaAsC-2 .....

KazCOs...-.-

MgCOs ......

CaCOs. ......

A12 03 - .......

SiOz .........

C0»..........

Grams per kilo 

of water.

0. 0048

0. 0221

0. 1320

0. 0575

Trace

......

0. 1463

0. 0035

0. 0295

0. 0112

0. 1650

0. 1045

0. 6764

Per cent, of total material 

in solution.

0.71

Q 97

19.51

8.50

......

......

21.63

0.52

4.36

1.65

24.40

15.45

100. 00

(70)
72 WATERS OF YELLOW3TONE NATIONAL PARK.

BENCH SPRING.

(Locality, Upper Geyser Basin; date of collection, Septembers, 1884; temperature, 

88° C.; reaction, slightly acid.)

Constituents.

SiOj. ........

80s. .........

COa.. ........

B203.........

Cl ...........

HzS..........

0 (basic)..... 

Fe> A1 J.. ....... 

Ca. ..........

Mg .... ......

K.... ........

"N"n

Li..... ..-

Grams per kilo 

of water.

0. 2400

0. 1151

0. 0350 

0. 0145

Trace

0. 0097

0. 0574

0. 4717

Percent, of total material 

in solution.

50.88

24.40

7.42 

3.07

2.08

12.17

100. 00

Determinations.

1

1

1

1

1

1

1

1

1

1

1

Grams of -water 

emplo\7 ed in 

each determination.

40

300

100

40

40

40

100

100

100

Hypothetical combination.

Constituents.

K2S04 .......

tfajSCh ...... 

MgSO* ......

CaS04. ......

Al2(S04)3 ....

AbOs.. ......

SiOz. ........

HC1 .........

co»..........

Grair.s per kilo 

of water.

0. 0210

0. 1772 

Trace

0. 0066 

0. 0263

0. 2400

TranA

' 0. 4717

Per cent, of total material 

in solution.

4.58

37.57

1.40 

5.57

50.88

*

100. 00

(72)
tJOOCH AND WHTTFIELD.1 RESULTS OF ANALYSIS.

FIREHOLE RIVER.

(Locality, above Upper Geyser Basin ; date of collection, August 27,1884; temperature, 12° C.; reaction, sliglitly alkaline; specific gravity, 1.00015.)

The water was filtered before bottling.

Constituents.

SiOa .........

SOi..........

COa. .........

B;Ai. ........

Cl. .. ........

HzS. .........

O(baaic) .....

Fe. ..........

Al ...........

Ca...........

Mg ..........

K.... ........

Na...........

'Li ......... ..

NH4 . ........

Grams per kilo 

of water.

0. 0407

0. 0062

0. 0305

0. 6105

0.0103

O ftAOQ

0. 0052

0. 0094

0. 0151

0. 00002

0. 13192

Per cent, of total material 

in solution.

30.86

4.70

23.11

7.96

7.81

9 on

3 94

0.83

7 13

11 45

0.01

100.00

Determinations.

2

2

2

2

2

2

2

O

2

2

2

2

o

2

Grams of water 

employed in 

each determination.

200

100

200

500

500

100

200

200

200

100

100

100

50

Albuminoid ammonia (not in summation), 0.00010 grams per kilo.

Hypothetical combination^

Constituents.

ttEUCl.......

LiCl.........

KCl .........

NaCl ........

KaaSOi ...... 

NasBdOr..... 

jSasCOs.--.-. 

MgCOs ...... 

CaCOa. ......

AlaOs. .......

COs. .........

Grams per kilo 

. of water.

0. 0181

0. 0030

0. 0110 

Trace 

0. 0210 

0. 0038 

0. 0130

0. 0055

0. 0407

0. 0158

0. 1319

Per cent, of total material 

in solution.

Trace 

13.72

2.27

8.34 

Trace 

15.92 

2.88 

9.86

4.17

30.86

11.98

100. 00

(73)
74 WATERS OF YELLOWSTONE NATIONAL PARK. . [BULL. 47.

YELLOWSTONE LAKE.

(Locality, near outlet; date of collection, September 18, 1884; specific gravity,

1.00014.)

The water was filtered through linen.

Constituents.

Si02 .........

SO,. ....... ..

COs. .........

B203 -. .......

Cl ...........

H2S..........

0 (basic) ..... 

Fe ...........

Al ...........

Ca ...........

Mg ..........

K............

Na.. .........

Li...........

NH4 . ........

Grams per kilo 

of water.

0. 0420

0. 0070

0. 0725

0. 0094

0. 0100

0. 0021

0. 0086

0. 0003

0.0047

0. 0156

0. 00042

0. 17262

Per cent, of total material 

in solution.

94 39

4.04

42.00

 5.43

5.78

1.21

4.97

0.16

2.71

9.36

0.02

100. 00

Determinations.

o

2

2

2

2

2

2

2

2

2

2

2

1

Grams of water 

employed in 

each determination.

200

100

200

500

500

100

200

200

200

200

100

100

100

50

Albuminoid ammonia (not in summation), 0.00022 grams per kilo.

Hypothetical combination.

Constituents.

NH4C1.......

LiCl. ........

KC1. ........

NaCl ........

NazSOi.......

NasCOs ...... 

MgC03 - ......

CaC08 .......

A13 03 ........

Si02 ..........

C03 . .........

Grams per kilo 

of water.

0. 0012

0. 0090

0. 0071

0. 0124

0. 0202 

0. 0010

0. 0215

0. 0040

0. 0420

0. 0542

0. 1726

Percent, of total material 

in solution.

0.69

5 91

4.11

7.18

11.73 

0.58

12.45

2.32

24.33

31.40

100. 00

(74)
GOOCII ASD WHITFIELD.] RESULTS OF ANALYSIS. 75

ALUM CREEK.

(Locality, at the crossing of the road; date of collection, September 19, 1884; reaction, acid; specific gravity, 1.00105.)

The water was filtered through linen before bottling.

Constituents.

SiOa. ........

80s ..........

COs. .........

BaOs-... ....

AssOs. .......

Cl ...........

Br. ..........

H2S... .......

0 (basic) ..... 

Fe... ........

Al. ..........

Ga. ..........

Mg ..........

K.. ..........

Na..... ......

Li ...........

NH4.........

H(inHCl)...

Grams per kilo 

of water.

0. 2180

0. 4202

0. 0075

0. 0057

0. 2028

Trace

0. 0840 

0.0250 a

0. 0025

0. 0127

0. 0038

0. 0741

0. 1595

0. 0009

0.00106

0. OC46

1. 22236

Percent, of total material 

in solution.

17.83

34.38

0.61

0.47

16.59

6.87

2.04

0.20

1.04

0.31

6.06

13.05

0.08

0.09

0.38

100. 00

Determinations.

2

2

2

2

2

2

1

2

2

2

2

2

2

2

1

Grams of water 

employed in 

each determination.

200

200

200

500

500

200

100

200

200

200

200

200

200

200

50

Albuminoid ammonia (not in summation), 0.00010 gram per kilo.

a All in ferric condition.

Hypothetical combination.

Constituents.

NH4C1.......

T ^f1!

KC1..........

KBr. ........

ZsSCh. ......

NasS04 ...... 

MgSC-4.......

CaSO-i .......

A12(S04)3 .... 

Fe2(S04)3 -... 

SiOa. ........

BsOa.. .......

COa. ...... ...

HC1.... ......

Grams per kilo 

of water.

0. 0031

0. 0055

0. 0669

0. 0872

0. 4924 

0. 0190

0. 0432

0.0158 

0. 0893 

0. 2180

0. 0057

0. 0075

0. 1688

1. 2224

Per cent, of total material 

in solution,

0.26

0.45

5.47

7 13

40.29 

1.55

3.53

1.29 

7.31 

17.83

0.47

0.61

13.81

100. 00

(75)
76 WATEES OP YELLOWSTOtfE NATIONAL PARK. (BULL. 4?.

CHROME SPRING.

(Locality, Crater Hill; date of collection, September 19, 1884; temperature, 92° C.; 

reaction, neutral; specific gravity, 1.00231.)

The water was filtered from suspended matter before analyzing and the latter was 

examined by itself.

Constituents.

SiOz .........

SOa..........

COi.... ......

BiO, - 

AssOs........

Cl ...........

Br...........

HjS.... ......

O (basic)..... 

-Fe. ........ I

Al <

Ca...........

Mg ..........

K.... ........

TZa.

Li...........

NH4 .........

4

Grams per kilo 

of water.

0. 3750

0. 3618

0. 0147

0. 0842

O flfl79

1. 0207

0. 0801

0. 0043

0. 0140

0. 0020

0. 1603

0. 7320

0. 0064

0. 0106

2. 8733

Percent, of total material 

in solution.

13.04

19 <WJ

0.51

2.93

6 9^

35.52

2.78

0.14

0.48

0.06

5.66

25. 47

0.21

0.36

100. 00

peterminations.

2

2

2

2

2

2

2

2

2

2

2

2

2

Grama of water' 

employed in 

each determination.

200

100

200

250

9^ft

200

200

200

200

100

100

100

40

a As received in the laboratory. 

Albuminoid ammonia (not in summation), 0.00107 grams per kilo.

Material in 

suspension in 

a kilo of water

SiOz ..............0.4791 gram.

S .................0.0757 gram.

Other J 

insoluble> .......0.0503 gram.

matter )

0.6051 gram.

(76)
OOOCH AND WH1TFIELD.J KESULTS OF ANALYSIS. 77

Hypothetical combination.

Constituents.

N.H4CI.......

 Lid.........

KC1... .......

KBr .........

NaCl ........

Na2S04 ...... 

MgSO*. ...... 

CaS04 .......

KaaBdOr..... 

A1203 -. ......

SiO« .........

B20S .........

As203 ........

C02 ..........

Grams.per'kilo 

of water.

0.0315

0. 3062

1. 353G

0. 5804 

0. 0100 

0. 0476

0. 0516 

0. 0082

0. 3750

0. 0485

0. 0072

0. 0147

2. 8733

Per cent, of total material 

in solution.

1.10

I

qe

10.66

47.11

21.46 

0.34 

0 45

1.74 

0.29

13.05

1.69

0.25

0.51

100. 00

A preliminary sample of 600 cm3., taken September 18,1883, yielded, when filtered 

from suspended material, the following figures signifying grams-of material per kilogram of water:

SiOs, 0.2380; S03, 0.3516; 01,1.0442; Fe and Al,.0.0080; 

Ca, 0.0185; Mg, 0.0024 ; K, 0.1438; Na, 0.6269; Li, 0.0041. 

The reaction was acid.

(77)
78 WATERS OF YELLOWSTONE NATIONAL PAEK. [BULL. 47.

MUSH POT SPRING,

(Locality, Pelican Creek; elate of collection, October 1, 1886; temperature, 85° C.; 

reaction, acid; specific gravity, 1.00088.)

The water was filtered from suspended material before the analysis.

Constituents.

SiOz .........

SOs..........

COa. ......

B203- ........

AszOs. .......

Cl. ..........

HsS..........

Fe. ..........

Al. ..........

Mg ..........

K...... ......

"Wo

Li ...........

NH4 .. .......

H(inHCl)...

Grams per kilo 

of water.

0. 2270

0. 5375

0. 0045

0. 0056

0. 0047

0. 0929

0. 0045

0. 0632

0. 0214

0. 0195

0. 1175

0. 0100

0. 0001

1.1084

Percent, of total material 

in solution.

Determinations.

2

2

2

2

2

2

2

2

2

2

2

2

2

Grams of water 

employed in 

each determination.

200

200

200

500

500

100

200

200

200

200

200

200

200

50

a As received in the laboratory. 

Albuminoid ammonia (not in summation), 0.00060 gram per kilo.

(78)
ooocn ASD WH:TFIELD.] RESULTS OF ANALYSIS. 79

Hypothetical combination.

Constituents.

(NE4)aS04 . . . 

Na8S04 ...... 

K2S04 .......

MgS04. ......

CaS04 ....'-..

Al2 (S04)s..... 

Fe»(SQ4)s.... 

SiOz.. ........

BaOs. ........

80s ..........

COz. .........

HC1.... ......

Grams per kilo 

of water.

0. 0366 

0. 3627 

0. 0435

0. 1070

0. 2149

0. 0285

Trace

0. 2270

0. 0056

0. 0733

0. 0045

0. 0048

1. 1084

Percent, of total material 

in solution.

3.30 

32.72 

3.93

9.66

19.39

2.57 

20.48

0.50

6.61

0.41

0.43

100. 00

The water carried in suspension 0.5551 gram of insoluble matter per kilogram of 

 water. This material dried at 104°; lost 7.33 per cent, of its weight on ignition. 

The partial analysis of 3.4972 grams of the ignited material resulted as follows:

SiOz .........

S03..........

AlsOs........

FesCh........

MnO. ........

CaO .........

MgO. ........

J&O.... ......

NasO ........

Per cent. 

61.30

0.63

24.24

6.53

1.74

2.18

0 17

0.84

98.03

(79)
80 WATERS OF YELLOWSTONE NATIONAL PARK.

PEVII/S JXK POT,

(Locality, Moant Washburn; date of collection, July, 8, 1886; temperature, 92° C. 

reaction, acid; specific gravity, 1.00221.)

Constituents.

SiOa . ........

SOs..........

COa.... ......

BaOs--. ......

AsaOs .......

Cl. ..........

H2S. .........

0 (basic) ..... 

Fa. ..........

Al. .........

Ca. ..........

Mg. .........

K.... ........

"No,

u. ..........

NH4- ........

H(inHCl)...

Gram s per kilo 

of water.

0. 0897

1

QOOA

0. 0647

0. 0518

0. 0058

0. 0051

0. 3795

0. 0037

0. 0396

0. 0121

0.0083

O.C245

0. 0004

0. 7687

0. 0002

3. 3871

Per cent, of total material 

in solution.

2.65

K<7 f\rj

1 91

1 PiQ

0.17

n 11

11.20

0.11

1.17

0.36

0.25

0.72

0.01

22.69

0.01

100. 00

Determinations.

9

2

o

2

2

2

2

2

2

g

-

Grams of water 

employed in 

each determination.

200

200

200

500

500

200

200

200

200

200

200

200

200

200

100

Hypothetical combination.

Constituents.

(NEthSOt... 

LijSCh. ......

NaaSO* ...... 

KaSCh .......

MgSO«.......

CaSOa .......

Alj(S04)s.... 

SiOa. ........

BsOs---......

S08 ..........

CO*..........

HC1. .........

HjS..........

Grams per kilo 

of water.

2. 8185 

0. 0031

0. 0756 

0.0185

0. 0605

n I<MR

0. 0234. 

0. 0897

0. 0518

0. 0356

0.0647

0. 0060

0. 0051

3. 387i

Per cent, of total material 

in solution.

83. 21 

0.11

2.23

0

*A

1.78

3 97

0.69 

2.65

I

eq

1.05

1 91

0.18

0.15

100. 00

(80)
OOOCH AKD WHITFIELD.] RESULTS OF ANALYSIS.

SODA BUTTE SPRING.

81

(Locality, Soda Butte; date of collection, September 17, 1885; temperature, 18° C.; 

reaction, alkaline; specific gravity, 1.00138.)

The water was filtered before bottling.

Constituents.

SiOa. ........

crv.

COn... .......

BaOs. ........

Cl ...........

Br ...........

HzS... .......

0 (basic)..... 

Pe Al t1 

Ca.. .........

Mg ..........

K. ...........

"Wo.

Li. ..........

NH4 - ........

Grams per kilo 

of water.

0. 0335

0. 0614

1. 2490 a

0. 0150

0. 0315

0.0042&

0. 1618 

0. 0069 .

0. 2325

0. 0632

0. 0238

0. 0575

0. 0057

1. 9460

Per cent, of total material 

in solution.

1.72

3.15

64.18

0.77

1.62

0.22

8.32 

0.36

11.95

3.25

1.22

2.95

0.29

100. 00

Determinations.

2

2

2

2

2

2

2

0

2

2

2

. 2

2

1

Grams of water 

employed in 

each determination.

200

200

200

500

500

200

100

200

200

200

200

200

200

200

50

ffl Cuprio sulphate was used to hold back HzS in the determination of COa. 

o'As received in the laboratory. (

Albuminoid ammonia (not in summation), 0.00140 gram per kilo.

Hypothetical combination.

Constituents.

NHaCl.......

LiCl.........

KC1.. ........

NajS04 ...... 

NajB<0, ..... 

NasCOs...... 

MgC03 .......

CaCOa. ......

A1203 ---.----

SiOa.........

C0a ..........

H2S..........

'

Grams per kilo 

of water.

0. 0169

0. 0425

0. 0034

0. 1062 

0. 0216 

0. 0419 

0. 2212

0. 5813

0. 0131

0. 0335

0. 8602

0. 0042

1.9460

Per cent, of total material 

in solution.

0.87

0 10

0.17

5.46 

1.11 

2.15

n VT

90 R7

0.67

1.72

44.20

0.22 ,

100. 00

Bull. 47 6

(81)
Summary of Analyses. 

[The amounts of substances are stated in grams per kilogram, f

Fearless eyse

Firehole River above Upper Basin. 

Gardiner River above Hot River . . 

Gardiner River below Hot River . . 

Water Supply at Mam. Hot Springs

Date of 

collection.

Oct. 11,1883 

July 28, 1884 

July 28, 1884 

Oct. 11,1883 

Oct. 5, 1884 

Sept. 17, 1885 

Aug. 18, 1884 

Sept. 27, 1883 

Aug. 20, 1884 

Sept. 13, 1885 

Aug. 20, 1884 

Oct. 11, 1886 

Aug. 20, 1884 

Aug. 20, 1884 

Aug. 24, 1884 

....do .......

Sept. 11, 1885 

....do .......

Aug. 25, 1884 

Aug. 29, 1883 

Sept. 1, 1884 

Sept. 10, 1885 

Aug. 28, 1884 

Aug. 29, 1884 

Aug. 28, 1883 

Sept. 1, 1884 

Aug. 28, 1884 

Sept. 1,1887 

....do .......

July 20, 1884 

Sept. 16, 1884 

Sept. 2,1884 

Sept. 19, 1884 

Sept. 18, 1883 

Sept. 19, 1884 

Oct. 1, 1886 

July 8, 1886 

Aug. 24, 1884 

Aug. 27, 1884 

Oct. 12,1883 

Sept. 26, 1884 

July 28, 1884 

1887

Sept. 18, 1884

Temperature.

Degrees G. 

71 

67 

44 

63 

58 

18 

88 

92 

84 

92 

73 

72 

91 

91 

82 

82-93 c 

43 

60 

92 

92 

84-88 d 

93 

93 

93 

93 

' 93 

93 

91 

89 

92 

84 . 

88 

92 

92

85 

92 

8 

12 

8 

13

6

Reaction.

....do .... .... 

....do .........

....do 

....do ......... 

....do .........

Neutral .......

..do .........

....do ......... 

Acid ......... 

....do ... ..... 

Faintly acid . .

....do .........

Alkaline...... 

....do .........

....do ........I

....do .........

....do ......... 

....do ......... 

....do ........

... do ......... 

....do ......... 

....do .........

....do ........

...do .........

....do .........

....do .........

....do ......... 

....do......... 

... do .........

....do .........

....do .........

....do .........

Slightly alk...

...............

Acid

Specific 

gravity.

1.00205

1. 00157 

1. 00138 

1. 00110

1. 00110 

1. 00115 

1. 00130 

1. 00124 

1. 00071 

1. 00130 

1. 00100 

1. 00104 

1. 00107 

1. 00100 

1. 00110

1. 00096 

1. 00132 

1. 00127 

1. 00100

1. 00095 

1. 00120 

1. 00108 

1. 00121 

1. 00105

1. 00231

1. 00105 

1. 00088

1. 00031 

1. 00015

.........

1. 00041 

1.00014

SiO»

0. 0517

0. 0502 

0. 0500 

0. 0335 

0. 4180

0 4636 

0. 4685 

0. 6070 

0. 5805 

0. 2532 

0. 4577 

0. 3315 

0. 3182 

0.2477 

0. 1507 

0. 2214 

0.2727 

0. 3828 

0. 2964 

0. 3000 

0. 3917

O QQJQ

0. 3042 

0. 2590 

0. 3035 

0. 2737 

0. 2926 

0. 1650 

0. 2400

0. 3750

O OOQA

0.2180 

0. 2270

0. 0965 

0. 0407 

0 0469

0. 0272

0. 0184 

0. 0420

TiOi

.......

none.

none.

none.

none.

none, 

none.

........

.......

........

......

.......

SOa

0. 4254

0. 4395 

0. 4573 

0. 4407 

0. 4230 

0. 0614 

0. 0367 

0.6501

0. 0228 

0. 0923 

0. 0264 

0. 0280 

0. 1929 

0. 1012 

0. 0195 

0. 0187 

0. 0196 

0. 0123 

0. 0146 

0. 0107 

0. 0152 

0.0158 

0. 0158 

0. 0167. 

0. 0144

0. 0271 

0. 0148 

0. 0218 

0. 0127 

0. 0385 

0. 0324 

0. 1151

0. 3618 

0. 3516

0. 4202 

0. 5375 

1. 9330 

0. 0084

0. 0117 

0. 0802

0. 0390 

0. 0070

CO,

0. 5071

0. 6287 

0. 3866 

0. 3378 

0. 4270 

1. 2490 

0. 0046

0. 0075 

0. 0155 

0. 0425 

0. 0262 

0.0250 

0. 0175 

0.2307 

0. 2107 

0. 2907 

0. 6140 

0. 3825

0. 0894 

0. 4225 

0. 4042 

0. 1055

0. 0920 

0. 3155 

0. 1950 

0. 3607 

0. 3210 

0. 1800

0. 0147

0. 0075 

0. 0045 

0. 0647 

0. 1040

0. 0710 

0. 1725

0. 6735 

0. 0725

K,0.

.......

none.

none.

none.

none, 

none.

........

........

........

PiOs

4,

none.

none.

0. 00004

trace.

none. 

0. 00012

.........

........

........

«H

0. 0226

present. 

0. 0128 

0. 0150 

0. 0223

0. 0317 

0. 0328 

0. 0368 

0/0173 

0. 0390 

0. 0138 

0. 0100 

0. 0239 

0. 0130 

0. 0161 

present. 

0. 0148 

0. 0234 

0. 0240 

0. 0233

0. 0145 

0. 0290 

0. 0243 

0. 0177 

0. 0149 

trace, 

none. 

0. 0842

0. 0057 

0. 0056 

0. 0513 

0. 0060 

trace.

........

none.

As2O3

0. 0031

0. 0004 

none. 

0. 0022

0. 0038 

0. 0018 

0. 0007 

0. 0009 

0.0016 

none. 

0. 0027 

0. 0017 

0. 0034 

trace. 

0. 0026

0. 0021 

0. 0019 

0. 0010 

0. 0006

0. 0011 

0. 0003 

0. 0011 

0. 0014 

0. 0007 

undet.

0. 0072

none, 

none, 

none, 

none, 

none.

.......

none.

Cl

0. 1749

0. 1623 

O.\604 

0. 0315 

0. 6705 

0. 6476

0. 6520 

0.5740 

0. 7087 

0. 6701 

0. 1207 

0. 6391 

0. 3337 

0. 3508 

0. 2487 

0. 0698 

0. 2793 

0. 2765 

0. 4391 

0. 3227 

0. 3181 

0. 4408 

0. 4384

0. 3894 

0. 3045 

0. 3767 

0. 2996 

0. 1935 

0. 0947

1. 0207 

1. 0442

0. 2028 

0. 0047 

0. 0058 

0. 0737 

0. 0105 

0. 0049

0. 0301 

0. 0022

0. 0044 

0. 0094

Br

trace.

trace, 

none, 

none. 

0. 0026

trace.

trace, 

trace. 

0. 0004

tracti. 

none, 

trace.

0.0034 

none, 

none, 

trace.

trace, 

trace, 

trace, 

trace, 

none, 

none.

trace.

........

I

none.

none.

none.

none, 

none.

.......

Fl

*

none.

none.

none.

none.

none, 

none.

........

HjS

trace.

none, 

none. 

0. 0042 

trace.

trace, 

none, a 

none, 

none.

trace, 

trace, 

trace, 

none, 

none a 

none a 

trace.

0. 0002 

none a 

none, 

trace.

none, 

none, 

trace, 

none, 

none, 

none, 

none, 

none.jr

none, 

none.o. 

0. 0051 

none.

none.

........

none, 

none.

Basic O

0.1954

0. 1796 

0. 1682 

0. 1618 

0. 0113

0. 0185 

0. 0053 

0. 0175

0. 0386 

0. 0202 

0. 0654 

0. 0472 

0. 0504 

0. 1062 

0. 0955

0. 0419 

0. 0897 

0. 0866 

0. 0411

0. 0364 

0. 0807 

0. 0596 

0. 0903 

0. 0781 

0. 0392 

0. 0350 

0. 0801

0.0840 

0. 0929 

0. 3795 

0. 0265

0. 0103 

0. 0216 

0. 0487 

0. 0248 

0. 0432 

0. 0100

Fe

0.0

0.0 

- 0.0 

0.0 

0. 0006 

0.0

trace, 

trace, 

trace, 

trace.

none. 

0.0 

0. 0002 

trace, 

none, 

none. 

0. 0018 

0.0 

trace. 

0. 00008 

trace, 

trace. 

0.0 

trace. '' 

trace, 

trace, 

trace, 

trace. 

0.0 

0.0 

0.0 

0.0 

0. 0250 

trace, 

trace, 

trace.

trace. 

0. ( 

0.0 

0. ( 

0. 0053 

none.

Al

149

>12 

051 

069 

0. 0002 

1)21

0. 0031 

0. 0048 

0. 0029 

0. 0077

0. 0027 

)S1 

0. 0057 

0. 0021 

0. 0036 

none. 

0. 0012 

309 

0. 0009 

0. 0027 

0. 0034 

0. 0049 

)30 

0. 0029 

0. 0036 

0. 0032 

0. 0079 

0. 0040 

059 

L45 

)43 

)80 

0. 0025 

0. 0045 

0. 0037 

0. 0031

0. 0029 

042 

010 

Oil 

0. 0004 

0. 0021

Mn

none.

trace.Ti

trace, b

trace.

trace, e 

none.

........

.......

.......

.......

........

Ba

none.

none.

none.

none.

none, 

none.

.......

.......

........

........

........

Sr

none.

none.

none.

none.

none, 

none.

......:.

.......

........

.......

........

Ca

0. 3006

0. 3076 

0. 2504 

0. 2821 

0. 2360 

0. 2325 

0. 0092 

. 0..0098

0. 0064 

0. 0146 

0. 0102 

0. 0071

0. 0115

0. 0078 

0. 0014 

0. 0017 

0. 0064 

0. 0255 

0. 0022 

0. 0055

0.0015 

0. 0030 

0. 0034 

0. 0007 

0. 0058 

0. 0039 

0. 0039 

0. 0028 

0. 0014

0. 0118 

trace. 

0.0140 

0. 0185 

0. 0127 

0. 0632 

0. 0396 

0. 0066 

0. 00o2 

0. 0250 

0. 0749 

0.0316 

0. 0808 

0. 0086

Mg

0. 0729 

0. 0797 

0. 0659 

0. 0631 

0. 0632 

0. 0001

0. 0009 

0. 0018 

0. 0022

0. 0003 

0. 0010 

0. 0023 

0. 0022 

0. 0017 

0. 0022

0. 0006 

0. 0005 

0. 0015 

0. 0012 

0. 0002 

0. 0002 

0. 0010 

none, 

none.

0. 0010 

trace. 

0. 0020 

0. 0024 

0. 0038 

0. 0214 

0. 0121 

0. 0007 

0. 0011 

0. 0005 

0. 0175 

0. 0089 

0. 0106 

0. 0003

Cs

trace.

none.

none.

trace, 

none.

.......

.......

......

........

 ;:;:;:

........

Rb

trace.

none.

none:

trace, 

none.

.......

.......

..'......

........

.......

.......

K

0. 0511

0. 0610 

0. 0462 

0. 0238 

0. 0415 

0,0443 

0. 0544 

0. 0745 

0. 0729 

0. 0815 

0. 0395 

0. 0254 

0. 0379 

0. 0145 

0.0154 

0. 03S5 

0. 0225

0. 0267 

0. 0121 

0. 0152 

0. 041,0

0. 0213 

0. 0249 

0. 0167 

0. 0163 

0. 0235 

0.0116 

0. 0097 

0. 1603 

0. 1438 

0. 0741 

0.0195 

0. 0083 

0. 0170 

0. 0094 

0. 0079 

0. 0105 

0. 0031 

0.0027 

0. 0047

Na

0. 1299

0. 1233 

0. 1506 

0. 0575 

0. 4046 

0.3931 

0. 4046 

0. 3190 

0. 3936 

0. 3925 

0. 1265 

0. 3654 

0.6522 

0. 3351 

0. 2654 

0. 2930 

0. 4186

0. 3666 

0. 4407 

0. 4179 

0. 3451

0. 3118 

0. 3853 

0. 3818 

0. 3988 

0. 3202 

0.1340 

0. 0574 

0. 7320 

0. 6269 

0. 1595 

0. 1175 

0. 0245 

0. 0930 

0.0151 

0. 0200 

0. 0311 

0. 0145 

0. 0039 

0. 0156

Li

0. 0023

0. 0016 

0. 0011 

trace. 

0. 0081 

0. 0042 

0. 0022 

0. 0030 

0. 0020 

0. 0040 

trace. 

0. 0029 

0. 0035 

.0. 0025 

0. 0032 

" 0. 0004 

0. 0020 

present. 

0. 0056 

0. 0023 

0. 0037 

0. 0057 

0. 0043 

0.0061 

0. 0041 

0. 0036 

0. 0070 

0. 0009 

0. 0008 

trace. 

0. 0064 

0. 0041 

0. 0009 

none. 

0. 0004 

0. 0011 

trace, 

trace, 

trace, 

none, 

none, 

trace.

 .

-

0. 00063

0. 00011 

0. 00570 

0. 00025

0.00021 

0. 00127 

0. 00042 

0. 00030 

0. 00106 

0. 00633 

0. 00015

0. 00021 . 

0. 00080 

0. 00001

0. 00001 

0. 00008 

0. 00042

0. 00021 

0. 00023 

0. 00042 

0. 00021 

0. 0010

0. 0106

0. 00106 

0. 0100 

0. 7687

0. 00002

0. 000022 

0. 0005 

- 0.00042

In HC1° 

H

........

0. 0008 

0. 0032

0. 0007 

0.0019

0. 0046 

0. 0001 

0. 0002

.........

.........

Total.

2. 08523

1. 74401 

1. 9460 

1. 63275

1. 62207 

1. 91082 

1. 8545 

0. 83126 

1. 69283 

1. 39979 

1. 3155

1 1 £091

1. 32590 

1. 47251

1.39081 

1. 63398 

1. 59522

1. 21111 

1. 42683 

1. 39052 

1. 48771 

1. 2898 

0. 6764

0. 4717

2. 8733

1. 22236 

1.1084 

3. 3871 

0. 4366 

0. 13192

0. 4937 

0. 2757 

0. 8827 

0. 17262

Albuminoid 

ammonia.

0. 00020

trace. 

0. 00140 

0. 00001

0. 00001 

none. 

0. 00010 

0. 00060 

none. 

0. 00040 

0. 00038

0. 00020 

0. 00002

0. 00002 

0. 00002 

0. 00020

none. 

0. 00010 

0. 00020 

trace. 

0. 0002

0. 00107

0. 00010 

0. 00060

0. 00015

. 000028 

trace. 

0. 00022

a As received in laboratory. It 0. 000003. c Usual temperature between eruptions. d Temperature in pools about crater after eruption. e 0.000005. Total Na and K as chlorides, 0. 9559. g As received in the laboratory ; sulphur in suspension, 0.0757. AC. 000038

Bull. 47 Page 82.
INDEX.

	Page. 

Alkalies, correction of.................... 23

Determination of..................... 22, 31

Alum Creek, analysis of.................. 75

Aluminum, determination of....---...... 21

Ammonia, determination of .............. 25

Albuminoid, determination of......... 25

Amyl alcohol, use of ..................... 22

Analysis, statement of results............ 33

Anthracene filter, use of................. 31

Antimony, determination of.............. 31

Aqueous solution, treatment of .......... 29

Arsenic, determination of................ 31

Arsenious acid, determination of......... 17

Sulphide, precipitatiop of............ 17

Artemisia Spring, analysis of............ 69

Asbestos filter ........................... 27

Asta Spring, analysis of.................. 71

Barium, determination of................. 20

Bath,paraffine ........................... 14,19

Beehive Geyser, analysis of .............. 60

Bench Spring, analysis of................ 72

Benzol,useof .'........................... 31

Berzelius, method for fluorine ............ 26

Boric acid, apparatus for determining .... 18

Determination of.. ................ 17,33

Bromine, determination of ............... 20,29

Ccesium, determination of................ 31

Calcium, determination of................ 21

Carbonic acid, apparatus for determining. 15

Quantity of water used.............. 16

Total, determination of .............. 15

Chlorine, determination of............... 20

Chrome Spring, analysis of............... 76, 77

Cleopatra Spring, analyses of............. 36,37

Concentrated waters, treatment of....... 25

Strength of .......................... 25

Constant Geyser, analy sis of............. 48

Copper, test for.......................... 31

Sulphate, use of...................... 17

Coral Spring, analyses of ................ 49,50

Crucible, perforated, use of.... .13, ]7,21,24,27, 32

Devil's Ink Pot, analysis of.............. 80

Echinus Spring, analysis of.............. 51

Elements, combination of................ 34

Excelsior Geyser, analy sis of............. 58, 59

Fearless Geyser, analysis of.............. 44,45

Filter, anthracene........................ 31

Asbestos............................. 27

Firehole River, analyses of .............. 57,73

Fluorine, test for......................... 26

Page.

Fountain Geyser, analyses of............. 53

Gardiner Rivev, analyses of.......... 40,41

Grand and Turban Geysers, analyses of.. 68

Giantess Geyser, analysis of............. 65

Great Fountain Geyser, analysis of...... 54

Grotto Geyser, analysis of ............... 67

HotKiver, analysis of ................... 39

Hydrogen sulphide, determination of.... .13

Teat for.............................. 10

Precipitation by ..................... . 17

Hygeia Spring, analysis of............... 55

Hypothetical combinations, why assumed 34

Indigo solution, use of.................... 14

Introduction.............................. 9

Iodine, determination of................. 20,29

Iron, determination of ................... 21,27

Lead, test for ............................ 31,32

Lithium, determination of ...............22,30,31

Madison Spring, analysis of.............. 56

Magnesium, determination of ............. 21

Mammoth Hot Springs, analysis of water

supply of........................... 42

Manganese, determination of............. 27

Marignac, method for boric acid ......... 33

Mayor, method for lithium............... 30

Methyl alcohol, use of.........i.......... 18

Mush Pot Spring, analysis of............ 78,79

Natural waters, treatment of............. 12

Nessler's re-agent, use of................. 25

Nitric acid, determination of............. 14

Nitrous acid, determination of........... 14

Old Faith f ul Geyser, analy sis of.......... 60, 61

Operations in the field......;............. 10

Operations in the laboratory ............. n

Orange Spring, analysis of............... 38

Oxygen, basic............................ 33

Pearl Geyser, analysis of................. 46,47

Phosphoric acid, determination of........ 27

Potassium, determination of ............. ' 22°

Permanganate, useof................ 28,29

Residue, total............................ 11

Treatment of, in concentrated waters. 26

Rubidium, determination of............;. 31

Samples, method of taking............... 10

Number of........................... 9

Size of ............................... 10

Scblammkessel, analysis ot............... 52

Silica, determination of.................. 21

Free, action of........................ 31

.Soda Butte Spring, analysis of........... 81

(83)
INDEX.

Page. 

Soda Spring, analysis of.................. 43

Sodium, determination of............. 22

Specific gravity, accuracy of determination of.............................. 13

Apparatus for determining........... 12

Splendid Geyser, analyses of .............62,63,64

Strontium, determination of.............. 26

Sulphur, free, determination of........... 13

Sulphuric acid, determination of......... 13

Sulphurous acid, test for................. 13

Page. 

Summary of analyses.................... 82

Tartaiic acid, useof...................... 28

Taurus Geyser, analysis of............... 70

Thallium, test for........................ 31

Tin, testfor.............................. 31

Titanic acid, determination of............ 28

Turban and Grand Geysers, analysis of.. 68 

"Warrington, E., determination of nitric 

acid.................................... 14

Yellowatone Lake, analysis of............ 74

(84)