Improvements in Electrolysis in General, and Particularly in Electrolysis of Metals.
Year: 1890

page_text: Date of Application, 27th Nov., 1890
Complete Specification Left, 26th Aug., 1891-Accepted, 26th Sept.. 1891
PROVISIONAL SPECIFICATION.
Improvements in Electrolysis in General, and Particularly in
Electrolysis of Metals.
We EMILE PLACET and JOSEPH BONNET, both of 95 Boulevard Beaumarchais,
Paris in the Republic of France, Chemists, do hereby declare the nature of this
invention to be as follows:---
Numerous experiments have proved to us that when an electrolyte is subjected
to more or less considerable pressure, a much more complete decomposition is
effected, and that frequently products are obtained of a totally different nature from
those obtained at the atmospheric pressure.
In this case, the electricity acts in a much more efficient manner upon the
molecules of the liquid.
Let us take, for example, the salts of iron. Hitherto, galvanic iron has only
been obtained in the form of exceedingly thin pellicules, which only serve to harden
the surface of engraved plates under the name of "steeling." On attempting to
thicken these pellicules, they break and come off in scales.
It is true that several clever experts have obtained some medals & some
moulds of works of art in galvanic iron, but the processes employed for obtaining
this iron were so defective and impractical, that the authors themselves of these
processes have abandoned them, and given up the pursuit of their researches.
Thus, the few reproductions of works of art obtained by these skilful operators
remain the only objects which have hitherto been produced in galvanic iron, and
are to this day cited and admired as great feats and unique museum specimens, and
as objects of curiosity, constituting a difficulty overcome from a scientific point of
view, but not from an industrial point of view.
Therefore, galvanic iron hitherto does not exist as an industrial product. In
reality, it would be impossible to actually procure a given quantity for industrial
use.
The impossibility of depositing industrially any thickness of galvanic iron, is, by
reason of the salts of iron, under the influence of electricity, having great tendency
to evolve bubbles of gas. .In this case, decomposition of the metallic salts is
incomplete, and the deposit on the negative pole is impure, pulverulent, and of an
inferior nature.
.
It will be understood that the molecules thus deposited and surrounded on all
sides by the nascent gas bubbles are not sufficiently in contact to constitute a
pure, coherent, and malleable metal.
All experimentalists have recommended the use of a very feeble electric current
to prevent the liberation of these gas bubbles. But this means is practically
impossible, because a very feeble electric current will cause the deposit in a given
time (say 24 hours), when operating on salts of iron, of but a very small quantity
of galvanic iron, quite insufficient to serve as a base to any industrial product.
On the contrary, we have endeavoured to employ strong electric currents, so as to
be able to obtain, in a given time, large quantities of deposited metal, which is
the only way of practically working.
The point is, therefore, (1) to use strong electric currents, in order to obtain
a yield (in metallic deposits) which shall be useful and marketable; (2) to prevent
the liberation of gas bubbles generated by strong currents, in order to obtain a
deposit of metal which shall be pure and of good quality.
We have succeeded in obtaining these two objects, in submitting (as above
stated) the electrolyte to a pressure more or less great.
To exert this pressure on the electrolyte. various
means may be employed.

page_text: Sometimes we augment the pressure by means of a column of liquid, a simple
system of pumps and valves introduced on one side the fresh liquid to be electrolysed,
and remove from the other side the spent liquor which has been decomposed.
Sometimes we augment the pressure by forcing into the receptacles containing the
liquor, air, or, better, a gas having no action on the liquor, or better still, a gas
which will assist the reaction we desire to produce.
Sometimes we augment the pressure by means of steam, or by heating the
electrolyte in a closed vessel to the desired temperature, in order to give it the
desired pressure. Finally, in certain cases, we increase the pressure by increasing
the density of the electrolyte. Indeed, it is evident, that, in a very dense liquid,
the gas bubbles will meet with the same resistance in their formation and in
their liberation, as in a liquid under pressure.
We also obtain very considerable changes in the nature of the products formed
by electrolysis, by varying the conductor power of one of the electrodes with
respect to the other. For instance, we use a copper wire to lead. the electric
current into the decomposing bath, and on the other side we use an iron, lead, zinc,
or platinum electrode, of much less conductivity, for leading off the current.
arrive at the same result by using the same metal for the two electrodes, such as
copper, but making the negative electrode of a smaller section than the positive
electrode.
We
By reason of this arrangement, it seems that the electricity is resisted, and
accumulates in the bath. There results from this accumulation, and from tbis
resistance, a more complete decomposition of the electrolyte, and a more perfect
deposit upon the negative pole. Indeed, given a solution of a metallic salt which
only produces, at the negative pole (with the two electrodes of copper), a deposit
of a pulverulent, brittle and inferior nature, it will often be sufficient to change the
conductivity of the negative electrode, and to use, for instance, an iron or lead
wire, or simply use a smaller negative copper wire, in order to obtain a deposit
of pure ductile and malleable metal on the negative pole.
In some cases, this effect, produced by the difference of conductivity of the two
electrodes, may be combined with the variations of pressure, and truly remarkable
effects of decomposition may thus be obtained. By the help of the improvements
herein described, we have been able to deposit galvanic iron in a practical, and
merchantable manner, in plates as large and as thick as required.
It is not merely electrotype reproductions of works of art and the like which
we obtain, but blocks of pure iron of all sizes and all weights. In reality, we
obtain a new commercial product, a new metallurgical product which is destined,
by reason of its special and exceptional properties, to replace not only iron, but
many other metals in numerous and very important applications.
All we have said referring to galvanic iron, applies equally well to aluminium,
chrome, magnesium, tungsten, molybdium, uranium, etc.
It has not been possible hitherto to obtain all these metals commercially by
means of electrolysis, but thanks to our processes, we have been able to obtain them
with the greatest facility.
In fact, our processes enable us to obtain all metals by means of electrolysis.
We have said that in order to be able to pass a strong electric current through
a liquid to be decomposed (the only means of obtaining a commercial product), and
to obtain at the same time a deposit of metal of good quality, we submit the
electrolyte to a more or less high pressure. We have said that this pressure may
be produced either by the use of known physical or mechanical means, or what
comes to the same thing, in certain cases, by simply increasing the density of the
electrolyte.
It is useless for us to describe here the physical and mechanical means for
producing pressure. These means are well known, and, moreover, vary greatly
according to circumstances, but we may increase the density of the electrolyte
liquids (still using, for example, the salts of iron), by dissolving at the same time
two, three, or even a larger number of salts, which may be dissolved at once, and

page_text: which are not decomposable by electricity under conditions which allow of iron
being perfectly decomposed.
An important fact to observe is, that it is not by dissolving a large quantity of
salts of iron, that the density of the bath is increased. The salt of iron used
should only form about one third or one half of the saturation of the bath. But
it is by dissolving the salts of metals other than iron, that the density of the bath
is increased.
Generally, the density of a bath may be increased by dissolving, indifferently, all
salts of metals which are more electro-positive than the metal which is sought to be
deposited. And the proof that it is simply a question of increasing the density of
the bath, is, that these salts may be, so to speak, of any kind, provided they are
soluble, and do not decompose one another.
In baths thus composed of several metals in solution, only one metal is deposited
on the negative pole, and this is always the most electro-negative metal, when a
suitable and uniform electric current is passed through the bath, which is easily
obtained by dynamo-electric machines or other sources of electricity.
Further, when a more uniform current (such as a battery current), and of greater
intensity than is necessary to cause the most electro-negative metal to deposit, is
used, other metals are deposited at the same time, which unite with the first metal,
and alter more or less its purity. This is even a means of directly producing alloys
by electrolysis, when it is desired to do so.
Dated this 27th day of November 1890.
NEWTON & SON,
Agents for the Applicants.
COMPLETE SPECIFICATION.
Improvements in Electrolysis in General, and Particularly in
Electrolysis of Metals.
We EMILE PLACET and JOSEPH BONNET, both of 95 Boulevard Beaumarchais,
Paris, in the Republic. of France, Chemists, do hereby declare the nature of this
invention, and in what manner the same is to be performed, to be particularly
described and ascertained in and by the following statement :-
Numerous experiments have proved to us that when an electrolyte is subjected
to more or less considerable pressure, a much more complete decomposition is
effected, and that frequently products are obtained of a totally different nature
from those obtained at the atmospheric pressure.
In this case, the electricity acts in a much more efficient manner upon the
molecules of the liquid.
Let us take, for example, the salts of iron.-Hitherto, galvanic iron has only
been obtained in the form of exceedingly thin pellicles, which only serve to harden
the surface of engraved plates under the name of "steeling."-On attempting to
thicken these pellicles, they break and come off in scales.
It is true that several clever experts have obtained some medals and some moulds
of works of art in galvanic iron, but the processes employed for obtaining this iron
were so defective and unpractical, that the authors themselves of these processes
have abandoned them, and given up the pursuit of their researches.
Thus, the few reproductions of works of art obtained by these skilful operators,
remain the only objects which have hitherto been produced in galvanic iron, and
are to this day cited and admired as great feats and unique museum specimens, and
as objects of curiosity, constituting a difficulty overcome from a scientific point of
view, but not from an industrial point of view.
Therefore, galvanic iron hitherto does not exist as an industrial product. In
reality, it would be impossible to actually procure a given quantity for indus-
trial use.
The impossibility of depositing industrially any thickness of galvanic iron, is by

page_text: reason of the salts of iron, under the influence of electricity, having great tendency
to evolve bubbles of gas. Consequently, decomposition of the metallic salts is
incomplete, and the deposit on the negative pole is impure, pulverulent, and of an
inferior nature.
It will be understood that the molecules thus deposited, and surrounded on all
sides by the nascent gas bubbles, are not sufficiently in contact to constitute a pure,
coherent, and malleable metal.
All experimentalists have recommended the use of a very feeble electric current
to prevent the liberation of these gas bubbles. But this means is practically
impossible, because a very feeble electric current will cause the deposit in a given
time (say, 24 hours), when operating on salts of iron, of but a very small quantity
of galvanic iron, quite insufficient to serve as a base to any industrial product. On
the contrary, we have endeavoured to employ strong electric currents, so as to be
able to obtain, in a given time, large quantities of deposited metal, which is the
only way of practically working.
The point is, therefore, (1) to use strong electric currents, in order to obtain a
yield (in metallic deposits) which shall be useful and marketable; (2) to prevent
the liberation of gas bubbles generated by strong currents, in order to obtain a
deposit of metal which shall be pure and of good quality.
We have succeeded in obtaining these two objects, by submitting (as above
stated) the electrolyte to a pressure more or less great.
To exert this pressure on the electrolyte, various means may be employed.
Sometimes we augment the pressure by means of a column of liquid, a simple
system of pumps and valves introduced on one side the fresh liquid to be electro-
lysed, and remove from the other side the spent liquor which has been decomposed.
Sometimes we augment the pressure by forcing into the receptacles containing the
liquor, air; or, better, a gas, having no action on the liquor; or, better still, a gas
which will assist the re-action we desire to produce.
Sometimes we augment the pressure by means of steam, or by heating the
electrolyte in a closed vessel to the desired temperature, in order to give it
the desired pressure. Finally, in certain cases, we increase the pressure by increasing
the density of the electrolyte. Indeed, it is evident, that, in a very dense liquid, the
gas bubbles will meet with the same resistance in their formation. and in their
liberation, as in a liquid under pressure.
We also obtain very considerable changes in the nature of the products formed
by electrolysis, by varying the conductor power of one of the electrodes with
respect to the other. For instance, we use a copper wire to lead the electric
current into the decomposing bath, and on the other side we use an iron, lead, zinc,
or platinum electrode of much less conductivity, for leading off the current.
arrive at the same result by using the same metal for the two electrodes, such as
copper, but making the negative electrode of a smaller section than the positive
electrode.
We
By reason of this arrangement, it seems that the electricity is resisted, and
accumulates in the bath. There results from this accumulation, and from this
resistance, a more complete decomposition of the electrolyte, and a more perfect
deposit upon the negative pole. Indeed, given a solution of a metallic salt which
only produces, at the negative pole (with the two electrodes of copper), a deposit of
a pulverulent, brittle, and inferior nature, it will often be sufficient to change the
conductivity of the negative electrode, and to use, for instance, an iron or lead
wire, or simply use a smaller negative copper wire, in order to obtain a deposit of
pure, ductile, and malleable metal on the negative pole.
In some cases, this effect, produced by the difference of conductivity of the two
electrodes, may be combined with the variations of pressure, and truly remarkable
effects of decomposition may thus be obtained. By the help of the improvements
herein described, we have been able to deposit galvanic iron in a practical and
merchantable manner, in plates as large and as thick as required.
It is not merely electrotype reproductions of works of art, and the like, which

page_text: we obtain, but blocks of pure iron, of all sizes and all weights. In reality we
obtain a new commercial product, a new metallurgical product which is destined,
by reason of its special and exceptional properties, to replace not only iron, but
many other metals in numerous and very important applications.
All we have said referring to galvanic iron, applies equally well to aluminium,
chrome, magnesium, tungsten, molybdenum, uranium, etc.
It has not been possible hitherto to obtain all these metals commercially by
means of electrolysis, but thanks to our process, we have been able to obtain them
with the greatest facility.
In fact, our process enables us to obtain all metals by means of electrolysis.
We have said that in order to be able to pass a strong electric current through a
liquid to be decomposed (the only means of obtaining a commercial product), and
to obtain, at the same time, a deposit of metal of good quality, we submit the
electrolyte to a more or less high pressure. We have said that this pressure may
be produced either by the use of known physical or mechanical means, or, what
comes to the same thing, in certain cases, by simply increasing the density of the
electrolyte.
It is useless for us to describe here the physical and mechanical means for
producing pressure. These means are well known, and, moreover, vary greatly
according to circumstances, but we may increase the density of the electrolyte
liquids (still using, for example, the salts of iron), by dissolving at the same time
two, three, or even a larger number of salts, which may be dissolved at once, and
which are not decomposable by electricity under conditions which allow of iron
being perfectly decomposed.
An important fact to observe is, that it is not by dissolving a large quantity of
salts of iron that the density of the bath is increased. The salt of iron used should
only form about one third or one half of the saturation of the bath. But it is by
dissolving the salts of metals other than iron, that the density of the bath is
increased.
Generally, the density of a bath may be increased by dissolving, indifferently, all
salts of metals which are more electro-positive than the metal which is sought to be
deposited. And the proof that it is simply a question of increasing the density of
the bath, is, that these salts may be, so to speak, of any kind, provided they are
soluble, and do not decompose one another.
In baths thus composed of several metals in solution, only one metal is deposited
on the negative pole, and this is always the most electro-negative metal, when a
suitable and uniform electric current is passed through the bath, which is easily
obtained by dynamo-electric machines or other sources of electricity.
Further when a more uniform current (such as a battery current), and of greater
intensity than is necessary to cause the most electro-negative metal to deposit, is
used, other metals are deposited at the same time, which unite with the first metal,
and alter more or less its purity. This is even a means of directly producing alloys
by electrolysis, when it is desired to do so.
a
In order to prevent the inconvenience arising from the variable intensity of the
electric current, the following is the means we have adopted for communicating
suitable density to the baths, and for obtaining a metal perfectly pure, without
alloy of other metals.
The three following solutions are made in water :-
1st saturated solution of
sulphate of potash
sulphate of soda, and

page_text: 3rd saturated solution of
sulphate or chloride of the metal to be deposited, of sulphate of iron, for
example, or of chloride of iron.
We take a litre of each of these solutions, and mix them together; this produces
immediately a bath which will give the deposits of pure iron as thick as desired.
This composition is general. In the same manner, baths have been prepared
which have served to produce aluminium, chromium, magnesium, tungsten,
molybdenum, uranium, etc., by substituting for the sulphate or the chloride of iron,
the sulphates or the chlorides of these various metals. Moreover, this same com-
position of bath allows of all metals being obtained by electrolysis, by dissolving
therein the sulphate or the chloride of the metal desired to be deposited. The
same bath may be used to obtain successively all the metals, either by dipping in
one after the other anodes of the different metals, or by successively charging the
bath with sulphates or chlorides of different metals, that is to say, that a bath of
this description, giving deposits of a certain metal, may easily be transformed into
another bath, giving deposits of another metal. We use either the sulphate or the
chloride of the metals which are to be deposited, and why we have adopted these
two salts is, that they are generally easier to obtain, and are cheaper.
All ores, all salts of metals, may be converted into sulphates or chlorides with
the greatest ease.
If we have adopted the combination of the three alkaline sulphates of potash, of
soda, and of ammonia, as well as the combining of the three alkaline chlorides of
potassium, sodium, and ammonium, it is because these salts combined, dissolve in
larger quantities than when separate.
They mutually help each other to dissolve, by forming double, triple, etc. salts;
further, the combining of these salts answers in all cases, which would not be the
case had we used other salts.
Really, the solutions of alkaline sulphates alone, or chlorides alone, do not give
good results in the presence of the solutions of certain metals. It is therefore
necessary to add one, two, or three alkaline chlorides to the sulphates, or one,
two, or three sulphates to the chlorides. To avoid this complication, we use a
solution of the three sulphates, and a solution of the three chlorides.. Bv this
means, we have a general method which permits of any metal being obtained.
Moreover, our object being simply to increase or diminish the density of the
baths, we reserve to ourselves the right to increase or diminish the number of salts
to be dissolved.
Instead of using saturated solutions, which are frequently difficult to determine,
the degree of saturation being variable, the bath may equally well be composed in
the following manner :-

page_text: 1st. One litre of the saturated solution of the three alkaline sulphates above
described.
2nd. One litre of the saturated solution of the three alkaline chlorides.
3rd. One litre of water, acidulated by sulphuric acid or hydrochloric acid.
These three solutions are mixed together, and using two plates of the metal to be
deposited as positive and negative poles, an electric current is passed through, until
the metal begins to deposit upon the negative pole.
Modifications in the composition of the baths-The alkaline sulphates and
chlorides may be replaced in the bath by phosphates, nitrates, chlorates, carbonates,
borates, fluor hydrates, acetates, citrates, tartrates, oxalates, cyanhydrates, sulphites
of potash, soda, ammonia, lime, magnesia, manganese, barytes, strontium,
aluminium, etc.
It is thus, by way of example, that solutions of phosphates or sulphites succeed
very well, when it is wished to obtain chromium. These baths, according to what
metal is to be deposited, may be alkaline, neutral, or acid.
They may be slightly acid for iron magnesium, tungsten, etc. They may be
strongly acidulated for chromium, uranium etc.
The baths may be acidulated by sulphuric, hydrochloric, nitric, phosphoric, &
boric acids, and by means of organic acids such as tartaric, oxalic, acetic, citric,
benzoic, salicilic, tannic, gallic, etc.
These acids, and, amongst others, oxalic acid, generally give great purity to the
film of metal deposited in dissolving the sub-oxides, which often are deposited at
the same time as the metal.
Our process allows of the work being carried ou cold, but heat considerably
facilitates the decomposition, by increasing the conductivity of the baths, permitting
of a greater concentration of the liquids, and, in consequence, ensures more rapid
and more abundant deposits.
It would therefore be of great advantage to utilize the waste heat from machinery
to heat the baths, by circulating around the clectrolytic baths the waters of
condensation.
Sometimes we use soluble anodes, sometimes insoluble anodes.
a
When insoluble anodes are used, we find it advantageous (in order to prevent
polarization caused by the nascent bubbles of oxygen) to place these anodes in
separate compartments with porous partitions, and in contact with a liquid which
favors the disengagement or the absorbtion of the oxygen.
In the accompanying drawings,
Figs. 1, 2, 3, 4, 5 represent, in sectional elevation, arrangements which show, by
way of example, how the impurities of the anode are prevented from mixing with
the bath. In these drawings, A represents the liquid to be decomposed, B the
depolarizing liquid, C impurities, R reservoir for salts in a solid state.
The liquids which we use for the above object, are sulphuric and hydrochloric
acids, chlorides of sodium, of calcium, and all bodies having an affinity for oxygen,
such as sulphurous acid, the sulphites, the protošulphates, the protochlorides etc.
The nascent oxygen transforms these last named salts into bi-sulphates or
bi-chlorides, salts which may be directly utilized for the composition of the baths,
or which may be very easily returned to the state of sulphites or prochlorides.
This means of preventing the polarization of the positive pole is therefore very
advantageous, and costs nothing to speak of.
When we use soluble anodes of impure metal, or of metal other than that which
is contained in the bath (anodes of zinc, iron, etc.), we find it equally advantageous
to place these anodes in separate compartments with porous sides, in order to
prevent the fouling of the bath by the impurities of these anodes, or of the salts
which they produce by their dissolution, and we have been careful to provide an
easy escape out of the bath for these impurities, and for the salts formed, as may
be seen on reference to Figs. 1, 2, 3, 4, 5.
The impurities collect below the vessel containing the decomposing bath, so that
these impurities are-evacuated before they are able to mix with the bath and alter

page_text: its purity. As shown in Figs. 2, 3, 4, the liquid B, in passing through the
apparatus, carries out with it all the impurities.
The salts run off with the impurities are not lost; we separate the zinc, iron, or
other metal therein contained, by means of electrolysis.
When we use insoluble anodes, we make their surface as rugged as possible,
in order to prevent polarization, for each inequality considerably favors the
disengagement from the liquid of the bubbles of nascent oxygen.
When zinc is used as a soluble anode the salt of zinc formed may be prevented
from entering the bath through the porous partition, by placing in the bath oxalic
acid or an alkaline oxalate.
An oxalate of zinc is thus formed, which is insoluble, and is precipitated to the
bottom of the vessel.
The zinc cannot therefore alter the purity of the deposited metal.
When we do not use soluble anodes made of the same metal as that to be
deposited, we maintain the baths by dissolving in them a sulphate, a chloride, an
oxide, or a carbonate of this metal.
By arranging a series of 3, 4, 5-10-20 or more baths, coupled in tension, all
the metals may be obtained at an exceedingly low price.
We considerably improve the quality of the different metals deposited, by adding
to the baths very small quantities (1 to 2 grammes per 10 litres of liquid in the
bath) of one or more of the following substances:-
Gelatine, gum, dextrine, cascine, sugar, glucose, glycerine, ether, and alcohol,
hydrocarbons, chlorides of sulphur, sulphurets, hyposulphites of soda, iodine,
arsenical acid, gallic acid, pyrogallic acid, etc. etc.
For refining iron and other metals, our process may be used.
For refining iron, we use, as anodes, waste wrought iron, steel, or cast iron.
We have found by experience that the deposition of iron is much facilitated
by adding to an iron electrolytic bath, from 12 to 15 per cent. of sulphate of
magnesia.
Our process may be employed to extract the tin contained in waste "tins," such
as preserved meat tins.
To this end the waste "tins " are used as anodes in our iron electrolytic bath ;
the tin not being acted upon falls to the bottom of the bath, where it may be
collected without any expense.
The electrolytic baths, the density of which has been increased by dissolving
therein, two, three, or a greater number of inert metallic salts, so to speak, with
the sole object of being able to pass a strong electric current through them (the
only way to obtain a commercial result), these very dense baths, we repeat, permit
of alloys being directly obtained by means of electrolysis.
To this end we operate as follows:-We begin by making a very dense bath,
by dissolving together one, two, or three sulphates, and one, two, or three alkaline
chlorides of potash, soda, and ammonia (or any other alkaline salts which do not
decompose one another, as we have above explained), so that the liquid shall be
about half or two thirds saturated.
In this we place the soluble anodes of the different metals it is desired to alloy;
or we dissolve (as much as is possible to dissolve) the salts of the different
metals it is desired to alloy (these salts being sulphates, chlorides, phosphates,
sulphites, or other salts of the different metals as we have above indicated).
In this state a feeble electric current is caused to pass; and this current is
increased little by little until a metal begins to deposit upon the negative pole.
Here are two cases.
If the bath is acid, the first metal to deposit is always the most electro-negative
with respect to all the other metals dissolved in the bath.
If the bath is alkaline, it is the contrary; in this case, the metal which is first.
deposited is always the most electro-positive. Having caused a sufficient electric
current to pass for depositing sometimes the most electro-negative metal, sometimes
the most electro-positive metal, it is only necessary to obtain alloys of the different

page_text: metals introduced into the bath, to progressively increase the intensity of the
electric current; for example, by means of a variable transformer, when the
deposition of the more and more electro positive metals in the acid bath, and
the deposition of the more and more electro negative metals in the alkali bath,
takes place at the same time as the deposition of the first metal, thus forming
alloys of two, three, or a larger number of metals. When the desired alloy is
obtained, it is only necessary to note at this time the intensity of the current used,
and by continuing this same intensity of current in the baths composed of, and
maintained with the same elements, the same alloy is always produced.
In order to vary the proportion of the various metals, it is necessary to vary
the surface of the soluble anodes of the metals; or to vary the proportions of the
different salts used, by causing the salts of such and such metal to vary with
respect to any other metal.
In this manner, we have obtained very malleable alloys, by alloying directly
zinc and tin or copper with aluminium, chromium, tungsten, and molybdenum.
We have obtained very white and beautiful alloys, by alloying silver with
molybdenum and uranium."
It is thus we have obtained very hard and tough alloys, in alloying chromium
with tungsten, iron, and molybdenum.
Finally, we have produced alloys remarkable for their lightness, while being as
tough as aluminium. bronze, by alloying with aluminium a small quantity of
chromium, tungsten, iron, and molybdenum.
These alloys, composed of a large quantity of aluminium, retain nearly the
lightness of aluminium, which is not the case with aluminium bronze, in the
composition of which aluminium enters but in a very small proportion.
By our process we are enabled to use directly the ores of the various metals.
When these ores are sufficient electric conductors, they may be used at once as
anodes in the bath.
When they are not suitable for use as anodes, they may be transformed into
soluble salts, either by roasting or exposure to the air; or by contact with suitable
salts or acids.
The solutions resulting from the washing of the transformed ores, are treated
in such a manner as to extract from them the precious metals or other useful
products which are often found in them.
Our process, therefore, allows of the precious metals and other bye-products
being extracted which have been lost in the ordinary metallurgical operations.
Our process gives pure metals even from the most impure ores, thus allowing
of the use of many ores which have had to be abandoned, because the ordinary
method (dry process) produced metals which were too impure to be used or
economically refined.
By increasing the pressure, an electric current may be passed having practically
an illimitable power.
Under these conditions, a composite body does not exist which may not be
decomposed.
Having now particularly described and ascertained the nature of our said
invention and in what manner the same is to be performed, we declare that what
we claim is :-
1st. In electrolysis, the method of increasing the effects due to the action of an
electric current, consisting in subjecting the liquid, cold or hot, through which the
electric current passes, to a given pressure, either by physical means, gas under
pressure, liquids under pressure, etc., or by increasing the density of the electrolysed
liquid; either by dissolving therein inert substances, non-decomposable by the
current, or by means of conductors of different section or of different co-efficients
of conductivity, which will have the effect of impeding the current in its passage,
and thus constitute an artificial pressure.
2nd. The use of pressure acting upon the hot or cold electrolytic bath containing
B

page_text: the compound of the metal to be deposited, or in which is immersed an anode of
the metal to be obtained; such pressure being obtained by physical means (such
as gas under pressure or a column of liquid), combined with the use of currents of
a relatively high intensity with a view to obtaining pure metal.
3rd. The use of pressure acting upon the hot or cold electrolytic bath, containing
several compounds of two, three, or more metals, or in which the anodes of these
metals are immersed, such pressure being obtained by physical means, such as gas
under pressure or a column of liquid,-combined with the use of currents, the electro
motive force and the intensity of which may be regulated at will, in order to obtain
the deposition of the metals which should constitute the alloy.
4th. The use of anodes of different section and different conducting power,
constituting a means of causing an artificial pressure in the current, combined with
a current of relatively high intensity acting upon the hot or cold electrolytic bath
containing the metal or metals to be precipitated.
5th. The use of hot or cold electrolytic baths, the density and consequently the
pressure of which has been increased by dissolving therein inert salts, such as
sulphates, sulphites, phosphates, & oxalates, with alkaline or earthy alkaline bases,
and generally all compositions the bases of which are more electro-positive or
negative than the metal to be precipitated, according to whether the bath be acid
or alkaline; whether the baths contain in solution the compounds of the metal
to be precipitated; or whether the pure or impure soluble anodes of the metal to be
obtained are immersed in these baths, combined with the use of currents of a
relatively high intensity.
6th. The use of hot or cold electrolytic baths, the density of which has been
increased by their being constituted of the three saturated solutions of (a) three
alkaline sulphates; (b) three alkaline chlorides; (e) one sulphate or one chloride,
or soluble compound of the metal to be precipitated, combined with the use of
currents of relatively high intensity.
7th. The use of coild or warmed electrolytic baths, the density of which has
been increased by makng them of the two saturated solutions of (a) three alkaline
sulphates; (b) three alkaline chlorides, and in which are immersed the soluble
anodes of the metal to be precipitated, combined with the use of currents of
relatively high intensity.
8th. The use of electrolytic baths, the density of which is increased by making
them either of a saturated solution of three alkaline chlorides, or of a saturated
solution of three alkaline sulphates, and by pouring into one of these solutions, a
saturated solution of chloride or sulphate, or soluble salt of the metal to be
precipitated, or by immersing therein smooth or rough soluble anodes of the
metal, combined with the use of currents of relatively high intensity.
9th. The use of electrolytic baths, the density of which has been increased as
above indicated, and in which the insoluble anodes are placed in porous pots
containing one of the following:-sulphuric acid, hydrochloric acid, chloride of
sodium, chloride of calcium, sulphurous acids, or sulphites, with a view to prevent
polarization, combined with the use of currents of a relatively high intensity.
10th. The use of electrolytic baths, the density of which is increased as above
described, and in which the soluble anodes are rough, in order to prevent polariza-
tion, and are placed in porous pots arranged as shown in the accompanying
drawings, in order to prevent the impurities of these anodes fouling the bath, in
combination with the use of currents of a relatively high intensity.
11th. The use of electrolytic baths the density of which has been increased as
above indicated, in which the rough soluble or unsoluble anodes are placed in
porous pots arranged as indicated in the accompanying drawing, containing the
depolarizing liquids, when insoluble anodes are used, and in which the depolarizing
liquid, or the decomposing liquid, or the two liquids at once, are automatically
renewed, in combination with the use of currents of a relatively high intensity.
12th. The use of electrolytic baths the density of which has been increased as
above indicated, in which the soluble anode is of zinc, placed in the porous pot,

page_text: containing oxalic acid or alkaline oxalate, in order to prevent the salts of zinc
formed, from penetrating into the decomposing bath, in combination with the use
of currents of a relatively high intensity.
13th. The use of electrolytic baths the d nsity of which has been increased
as above described, in which a soluble or insoluble anode is immersed, and in
which is dissolved 1 to 2 grammes, per litre of the bath, of gelatine, gum,
dextrine, or similar material, with a view to improve the quality of the metal,
in combination with the use of currents of a relatively high intensity.
14th. The use of electrolytic baths the density of which has been increased as
above described, for refining iron, in which a soluble anode is immersed, and in
which is dissolved from 12 to 15% of sulphate of magnesia, with the view of
facilitating the deposition, combined with the use of currents of a relatively high
intensity.
15th. The use of electrolytic baths the density of which has been increased as
above described, and in which tin boxes are used as soluble anodes, to extract the
iron and the tin therefrom, combined with the use of currents of a relatively high
intensity.
16th. The use of electrolytic baths the density of which has been increased as
above described, and in which are immersed the soluble anodes, (which anodes may
be ores, when these last are conductors), or in which is dissolved the compounds
of metals to be alloyed (these compounds may be ores of the metals, when these
ores are soluble), the surface of the anodes and the proportions of the compounds
to be dissolved varying according to the proportion of the alloys to be obtained
in combination with a current the electro-motive force and intensity of which
may be regulated at will, in order to obtain the deposition of the metals which
should form the alloy.
17th. The alloys
(a) of aluminium, zinc, tin, or copper; chromium, zinc, tin, or copper; of
tungsten, zinc, tin or copper; of molybdenum, zinc, tin or copper, etc.
(b) of molybdenum and silver; of uranium and silver.
(c) of chromium and tungsten, of iron and chromium, of nickel and chromium, of
nickel and molybdenum, etc.
(d) of aluminium and chromium, of aluminium and tungsten, of aluminium and
iron, of aluminium and molybdenum etc.
These alloys may be alloyed with each other.
18th. The use of electrolytic baths, the density of which has been increased as
above indicated, and in which good conducting ores are used as soluble anodes for
extracting the metal therefrom, in combination with the use of currents of
relatively high intensity, suitable for effecting the precipitation of the metal.
19th. The use of electrolytic baths, the density of which has been increased as
above indicated, in which are dissolved bad conducting ores, which have been
previously transformed into soluble sulphates, chlorides, etc., in combination with
the use of currents of relatively high intensity, and suitable for effecting the
precipitation of the metal.
20th. The use of electrolytic baths, the density of which has been increased as
above indicated, and in which are dissolved the alloys of precious metals, when
these alloys are soluble, or capable of being converted into soluble compounds,
in combination with the use of a current, the intensity of which is varied at certain
times with a view of obtaining the successive precipitation of each metal composing
the alloy.
21st. The use of the electrolytic baths, the density of which has been increased
as above indicated, and in which are immersed the alloys of the precious metals,
when these alloys are capable of serving as soluble anodes, in combination with
the use of a current, the intensity of which is caused to vary at certain times,
with a view to obtain the successive precipitation of each metal composing
the alloy.
22nd. The use of several electrolytic baths coupled in tension, the density of

page_text: which is increased, or which are submitted to a high pressure, as above indicated,
and in which one or more compounds of metals are dissolved, or in which one or
more soluble anodes of metals are immersed, whether a single metal or alloys
are to be produced, in combination with the use of currents of a relatively high
intensity, currents of which the intensity and the electro-motive force may be
varied when alloys are to be produced.
Dated this 24th day of August 1891
NEWTON & SON,
Agents for the Applicants.