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therefore, in all probability the maximum crops capable of being produced by the addition of manure had been produced. If this is true then t h e increase in yield due t o activated sludge over ordinary barnyard manure is very striking and a t once places a high monetary value on this material, for t h e value of fertilizers must be directly proportional t o t h e crop returns yielded by them.
Vol.
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respect t o glaserite, Glauber's salt, potassium chloride and sodium chloride at a temperature of 3.7", and t h a t therefore this temperature represents t h e "transition temperature" for t h e equilibrium 3KC1
+ 2NazS04.1oH~O
+
+
KsNa(SO& 3NaC1 20 HzO, in which all t h e formulae, except t h a t of water, represent solid phases. A consequence of this fact is t h a t one of t h e two pairs of salts (in this case potassium chloDEPARTMENT OF PUBLIC HSALTH DIVISIONOF LABORATORIES rideand Glauber's salt) can exist assolidphasesinequilibTORONTO, CANADA rium with solutions of the four salts at temperatures below 3 . 7 ' only, whereas the other pair, i. e., glaserite EQUILIBRIA IN SOLUTIONS CONTAINING MlXTURES OF and sodium chloride, can exist as solid phases in equilibSALTS rium with such solutions only above this temperature. I-THE SYSTEM WATER AND THE SULFATES AND If the temperature of the system is limited t o t h e interCHLORIDES OF SODIUM AND POTASSIUM' val between 0" and IOO", which represents the limits By WALTERC. BLASDALE of practical importance, so t h a t ice is eliminated, Received March 20, 1918 The various processes suggested for increasing t h e nine different univariant systems in which three solid production of potassium-containing compounds involve phases are present are theoretically possible. T h e the separation of t h a t element from associated salts univariant systems which can be actually realized exb y fractional crystallization. The only satisfactory perimentally were first studied by Meyerhoff er and method of obtaining a clear understanding of the possi- Saunders,' who fixed t h e transition temperature disbilities of making such separations is a study of t h e covered by van't Hoff a t 4.4' instead of 3.7",and worked phase-rule diagrams representing the equilibria which out the phase-rule diagrams for t h e system a t temperaexist in aqueous solutions between the salts t o be sepa- tures of o", 4.4", 16" and 2 5 " . In taking up t h e work rated. Unfortunately much of t h e data necessary for at this point it was thought desirable t o repeat t h e det h e preparation of such diagrams is lacking, and t h e terminations upon which t h e diagrams for o o and 2 5 " present paper represents the first of a series which have were based, and t o obtain data necessary for t h e prepabeen planned by members of the Department of Chem- ration of similar diagrams a t temperatures of soo, 75' istry of the University of California for t h e purpose and 100'. EXPERIMENTAL METHODS USED of supplying what is believed t o be much-needed information. I n carrying out t h e work here reported assisSaturation of solutions with respect t o the different tance in t h e large amount of analytical work involved salts was effected by stirring in an apparatus similar has been rendered by students of the Department, t o t h a t used by Meyerhoffer until its composition reand special acknowledgment should be made t o Messrs. mained constant, which required from one t o 4 R. D. Elliott, A. H. Foster, D. Ehrenfeld and K. V. days. The tubes for t h e determinations made at King. 0" were kept in a large thermostat capable of holding PREVIOUS W O R K O N THE SUBJECT sufficient ice t o last for 5 days. For saturation a t t h e The system designated in the sub-title consists of four other temperatures t h e necessary heat was supfour components, namely, water and any three of t h e plied t o t h e thermostats b y electric lamps immersed four salts concerned, which constitute a "reciprocal salt in the water or oil of the bath; a large mercury regulator pair." I n addition t o t h e four simple anhydrous salts kept t h e temperature of the 2 5 ' and t h e 50' baths the only solid phases t o be considered are ice, t h e constant t o within 0 . 2 " , and of t h e 7 5 O and 100" baths decahydrate of sodium sulfate, which will be called t o within 1 . 0 ~ . The composition of t h e saturated solution was ascerGlauber's salt, and t h e double sulfate of sodium and potassium generally known as glaserite. This name was tained by removing portions of i t in a weight pipette first used by Penny t o represent a compound corre- previously heated t o the temperature of the bath, sponding t o t h e formula K3Na(S04)2, but double sul- weighing and analyzing t h e solution. The chlorine fates containing somewhat different proportions of t h e ion was determined by titrating a fractional part of constituent salts were subsequently reported by other the solution with a standard solution of silver nitrate, investigators and different names applied t o them. the SO1 ion by precipitating and weighing as BaS04, Van't Hoff2 was able t o show t h a t it was possible t o and the potassium ion by separating and weighing as prepare a series of solid solutions in which the per- K2P t Cle. As it seemed probable t h a t the control of any procentages of potassium sulfate varied between 78.6 and 61.8, which justifies treating all of these compounds as cesses based on these diagrams could be most easily effected by means of a hydrometer t h e specific gravities a single solid phase. It was also shown by van't Hoff and Reichera t h a t of most of t h e solutions were also determined. T h e it was possible t o prepare a solution saturated with method consisted in removing and weighing, by means of a pipette which had been drawn out t o a capillary 1 This work has been supported by the Council of Defense of the State of California. a t t h e mark on its stem,a definite volume of t h e solution, 2
"Unters.
a
Z.fihysik. Chem., 3
U.
Bildung der ozeanischen Salzablagerung," p. 22G. (1889), 482.
12.physik.
Chem. 28 (18991, 453.
T H E J O U R N A L OF I N D U S T R I A L A N D E N G I N E E R I N G C H E M I S T R Y
May, 19x8
measured at the temperature of t h e bath, and comparing the weight with t h a t of the water delivered by t h e same pipette at a temperature of z o o . The results are probably accurate t o within two units in t h e third decimal place. No corrections were made for changes in t h e capacity of t h e pipette due t o varying temperature nor for variations in t h e volume delivered by it owing to changes in the viscosity of the solution. THE D I A G R A M FOR
25O
The composition of the solutions saturated with one o r more salts a t this temperature expressed in grams of t h e various salts per I O O grams of water is given in Table 1.' I n order t o represent these results graphically t h e corresponding values, when expressed in terms of mols of t h e various salts which have equal replacing power per 1000 mols of water, were calculated. These data are given in Table 11; they are plotted in Fig. I \&i
w W & ? S O ,1. 0
FIG.I-THE EQUILIBRIUM DIAGRAMAT
25'
with respect t o four axes, representing N a ~ S 0 4 ,KzS04, KzClzand NazClz,respectively, and the various points are connected by straight lines, although i t is probable TABLEI-COMPOSITION,
IN
GRAMSPER 100 G.,oF WATER, OF SOLUTIONS SATURATED AT 25 NaCl KCl NazSO4 KzSO4 Sp. Gr. 27.93 1.212 1202 1.088 36166 1.187 35.63 1.199 36167 9.31 1.282 6.69 13.24 1.149 3k:83 1.53 1.190 29:88 16.28 1.237 32.16 i:Sl 1.239
Saturated with Ai] NazSO4.. BI &SO4 CI KCl DI NaCl El NaBOt and glaserite.. FI &So4 and glaserite.. GI RzSOn and RCl.. HI KC1 and NaCI.. 11 NaCl and NazSO4.. JI NazSO4 and Glauber's salt 18.82 21.68 PI NazSO4 Glauber's salt, gladrite.. 14.28 22.28 7.32 L.1 KCl, RzSO4, glaserite.. 6.78 24:i8 ... 2.23 MI KC1 NaCl glaserite.. 27.96 16.37 3.51 N I Nadl, NazQO,, glaserite 34.90 2.25 ii:o3 .BLE 11-COMPOSITION, IN MOLS PRR 1000 M ~ OFs WATER,OF TA TIONS SATURATED A T 25 Saturated with NazClz KzClz &SO4 NazSO4 35.41 Ai NazSO4. li:46 BI KZS04... 4k 62 c1 KCl.. 54:90 DI NaCl. 39:i7 9.63 E1 NazSOi and glaserite.. 13.69 8.48 Fi KZs04 and glaserite.. 1.50 44: ii GI KZSO4 and KCl 46:04 19.66 Hi KCl and NaCl. li:44 49.56 11 NaCl and NazSOa.. J I NazSO4 and Glauber's 27.5 salt. 29.00 Kl NazSO4, Glauber's salt, 28.25 glaserite.. 21.92 7.57 2.30 3i:i9 Ll KCl. RzSOa, glaZerite 10.45 4.45 43.08 19.78 M1i KC1, NaCl, glaserite.. 2.85 ii:ko N1 NaCI, NazS04, glaserite 53.75
............... .................. .................... ................ ... ...... . . . ...... ...
..............
...
... ...
... ...
...
...
...
... ...
... ...
...
.........
...
............. ............ ............... ............... ... ....... ... ....... ... ............. ..........
... : ... ...
... ...
...
...
...
...
... ...
ferent composition, but if perpendiculars are erected a t t h e limiting points and given lengths proportional t o t h e total number of mols present in the saturated solutions t o which these points correspond, and if the ends of these perpendiculars are properly connected, any point which appears on the planes which limit the resulting solid figure can have a single definite value only. The diagram agrees in all essential features with t h a t given by Meyerhoffer, with the exception of the position of t h e point J representing the composition of a solution containing sodium chloride and sodium sulfate in equilibrium with solid sodium sulfate and Glauber's salt. His determination places t h e position of this point as W. That this is in error was clearly shown by duplicate determinations and also by determining the points a, b, c and d on the line I J , and e on the line AJ, t h a t is, the composition of solutions containing sodium chloride and sodium sulfate, and saturated with either sodium sulfate or Glauber's salt. The diagram indicates t h e composition of all possible solutions which can be in equilibrium with t h e six different solid phases: v i z . , glaserite, Glauber's salt, sodium chloride, sodium sulfate, potassium chloride and potassium sulfate. Since t h e composition of glaserite may vary between certain limits, the position of all points representing solutions saturated with respect t o it may show slight variations. I n determining the composition of such solutions care was taken t o add only sufficient of the prepared salt t o inoculate t h e solution, t h a t is, t o cause the greater part of the solid glaserite present t o separate from t h e solution itself. This insured t h e presence of solid glaserite of a composition corresponding t o t h e limiting value of t h e salt which could exist in t h e particular portion of the diagram concerned. No difficulty was experienced in inducing t h e salt t o separate under favorable conditions, even without inoculation. It invariably appeared in t h e form of coarse, granular crystals sometimes 2 t o 3 mm. in diameter, which showed under t h e microscope a well-defined hexagonal symmetry, and were uniaxial.
1.243 1.273 1.200 1.250 1.266 SOLU-
Sum 35.41 12.46 44,62 54.90 48.90 22.17 45.61 65.70 62.00 56.50 57.74 48.24 67.31 68.00
t h a t most of these are curved slightly. It should not be forgotten t h a t this kind of a diagram actually represents the horizontal projection of a solid figure. Any point on it may represent a number of solutions of difIn the tables in this article t h e subscripts of A, B, C, etc., indicate t h e figure on which the points are t o be found. 1
345
A FIG. 2-CRYSTALS OF GLASBRITE
The typical habit, which makes it easy t o distinguish the salt from either potassium or sodium sulfates, is represented in Fig. 2, of which A represents a specimen prepared a t 100' and B a specimen prepared a t joo from the two simple sulfates. THE D I A G R A M F O R
0'
The d a t a for this diagram are given in Tables I11 and IV. The graphical representation given in Fig. 3 differs from t h a t given by Meyerhoffer in two funda-
'
.
T H E J O U R N A L OF I N D U S T R I A L A N D E N G I N E E R I N G C H E M I S T R Y
346
Vol.
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No. 5
mental respects. First, t h e position of t h e point I, representing t h e composition of solutions in equilibrium with solid sodium chloride and solid Glauber’s salt, is located by Meyerhoffer a t t h e point marked W. That t h e point I represents t h e correct composition of the solution was shown by t h e preparation of ‘two different solutions whose analyses gave closely agreeing results. The second difference relates t o t h e location and size of t h e glaserite field. The Meyerhoffer diagram shows t h a t t h e glaserite field includes t h e point F and exFro. J-THE EQUILIBRIUM tends over an interval between D ~ A G R AATM0’ t h e points marked X and Y. I t also makes t h e glaserite field extend between lines joining the points Y and L and t h e points X and 0.
t h e glaserite field gave more difficulty. By starting with solutions containing varying amounts of sodium chloride and saturating- with both Glauber’s salt and potassium sulfate, solutions represented by t h e points a, b, c and d , evidently in t h e line FP, were obtained. By starting with solutions containing both sodium and potassium chlorides and saturating with Glauber’s salt and glaserite, solutions represented by t h e points e and f,evidently on t h e line O P , were obtained, and b y saturating a solution of sodium chloride with potassium sulfate and glaserite t h e point g was obtained. These make it possible t o fix with apparent accuracy t h e position of t h e point P. The points h and i on t h e line OL were fixed by a similar method. The other parts of t h e diagram differ but slightly from those found by Meyerhoffer. The complete diagram differs from t h a t for 2 5 ’ in t h e disappearance of sodium sulfate as a solid phase and t h e very much reduced area occupied by t h e glaserite field. TABLE 111-COMPOSITION, IN GRAMSPER 100 G. OR WATER, OB SOLUTIONS THE DIAGRAMS F O R SOo, 75’ A N D 1 0 0 ’ SATURATED AT Oo Saturated with NaCl KC1 NaaS01 KzSO4 SP. Gr. Since Glauber’s salt loses its water of crystallization a t Aa NaaSO4.. . . . . . . . . . . . . . . . ... 4.62 ... 1.043 33O, even when in contact with a saturated solution Bs KzSOi . . . . . . . . . . . . . . . . . . ... 7.23 1.063 Cs KCl ................. 28:iO ... ... of sodium sulfate, it cannot exist as a solid phase above Do NaCI.. .............. 34:95 ... ... ... 1.153 1.206 and Fa Glauber’s salt ._ _ this temperature in equilibrium with aqueous solutions KzSO4.. . . . . . . . . . . . . . 6.30 9.00 1.118 Ga K&Oi and KC1.. ..... 2?:88 ... 1.21 ... of any of t h e salts here considered, and t h e only solid Ha NaCl and KC1. ....... 3 i : j 3 10.55 ... ... Io NaClandGlauber’ssalt 34.48 1.70 ... i : i k phases t o be considered a t temperatures of joo, 7 5 O La KtS04, KC1, glaserite.. 13.38 1 i :$8 ... 2.78 1.188 Ns NaCI, Glauber’s salt, and 100’ are Na2S04, KzS04, KC1, NaCl and glaserite. KCl. ............. 32.08 7.81 ... 3.62 1.240 The composition of t h e saturated solutions which Oa KCl, Glauber’s salt, glaserite.. ......... 27.07 10.06 ... 3 . 2 4 1.232 determine t h e equilibrium diagrams for these temperaPs KzS04, Glauber’s salt, glaserite............ 7.46 13.24 4.73 ... ... tures are given in Tables V, V I , VII, V I I I , I X and X, TABLE IV-COMPOSITION, IN Mobs PER 1000 M*OLSOF WATER, OF SOLUand t h e corresponding diagrams (Figs. 4,5 and 6). If t h e TIONS SATURATED AT 0 &SOL Sum NazSOk Saturated with NatCle KzCla diagram for 2 5 O be compared with those for s o o , 75 and ... 5.85 As NazSOa .............. ... 5.85 7.47 7.47 IOOO it will be seen t h a t t h e progressive changes in t h e Ba KzSOk ............... ... ... .,. 34.05 Ca KC1................. ... positions of t h e points C , H, I , L, M and N are such as ... 53.84 Ds NaCl ................ 5 i : a 4 ...
Fa Glauber’s
salt and .......... ..... 4 ... i:h ...... NaCland Glauber’ssalt 53.28 KzSO4. KCl, glaserite . 19.41 NaCl, Glauber’s salt,
Is
La
Na
............ .........
49.44 KCl.. Os KCl, Glauber’s salt, 41.71 glaserite., Ps KzSOn, Glauber’s salt, glaserite., . . . . . . . . . 11.50
9.30 1.25
2.32 2.87
... ...., .
17.29 34.91 61.33 55.60 43.76
...
7.99
KZS04..
... ...
Ga KaSOa and KCl.. Ha NaCl and KC1..
3.75
62.62
12.15
..
3.35
57.21
16.00
6.0
...
33.50
9.43
Several attempts t o prepare a solution whose composition corresponded t o t h a t represented by t h e point X failed. All such attempts resulted in t h e formation of a solution whose composition was represented by t h e point F, when made either from Glauber’s salt and glaserite or by t h e use of potassium sulfate and a large excess of Glauber’s salt and inoculating with glaserite. Although glaserite seems t o be unstable a t this temperature in contact with any possible solution made from t h e constituent salts, it might be expected t o exist as a solid phase in contact with solutions which also contain sodium and potassium chlorides, since t h e reaction by which it is formed involves the dehydration of Glauber’s salt. N o difficulty was experienced in showing t h a t glaserite was stable in contact with solutions whose composition was represented by points slightly t o t h e left of t h e line LO, and t h e locations of t h e points L and 0, both of which represent solutions saturated with glaserite, were found t o agree with those fixed by t h e work of Meyerhoffer. The determination of t h e third point which establishes the form and size of
FIG. $-THE
E Q U I L I B ~ ~DIAGRAM UM AT 50‘
might be predicted from t h e changes in t h e solubilities The changes in t h e points of t h e four simple salts. E and F depend in part upon t h e specific properties of glaserite, b u t it is easy t o correlate t h e change of Elt o E4 with t h e very great increase in t h e solubility of sodium sulfate between 2.5’ and 5 0 ° , and t h e changes from E4 t o E6 and EB with t h e slight decrease in t h e solubility of this salt between 50 O and 7 5 ’. Similarly t h e successive changes from F1 t o F4, Fs and FR are correlated with t h e increase in t h e solubility of potassium sulfate between 2 5 O and 100’. The striking feature of these diagrams is t h e great increase in t h e size of t h e fields representing t h e composition of solutions
M a y , 191.8
T H E JOURATAL OF I N D U S T R I A L A N D ENGINEERING C H E M I S T R Y
347
KSZ.
FIG. 5-THE
EQUILIBRIUM DIAGRAMA T 75O
TABLE~V-COMPOSITION, IN GRAMSPER 100 SATURATED AT 50 Saturated with NaCl KCl A: NasSOa B4 KzSO4 4i:iz 6 KC1 D4 NaCl 36: 50 E4 NazSO: and glaserite.. F: &SO4 and glaserite.. ... 45: i 4 G4 KC1 and KzS04.. H4 KCl and NaC1.. 29: 09 22.03 14 NaCl and NazS04.. 33.70 35:66 4.68 L4 KzS04. KCI, glaserite. M4 KCl, NaC1, glaserite.. 26.84 22.43 N4 NaC1, NazSOa, glase1-ite 40.15 14.58
.............. ............... ................. ...............
. ...
...
...
...
..... ......
...............
g. OF
FIG. 6-THE
WATER,OF SOLUTIONSTABLE X-COMPOSITION, KzSOa
SP. Gr.
... ...
1.301 1.110 1,198
As
1i:09
45:i3 6.79
9.40 17.36 1.84
Ea
... ... 2.59 ...
1.351 1.307 1.212 1.246 1.223 1.203 1.254
...
1.248
NazSOa 44.84
... ...
7.34
...
3.15 11.74
...
...
1.188
TABLE VI-COMPOSITION, IN MOLS PER 1000 M ~ L OF S WATER,OF SOLUA4 B4 C4 D4 E4 F 4
G4 H4 14
L4 M4 N4
TIONS SATURATED AT 50 NazClz KzCla NazSO: 56.86
Saturated with NazSOn KzS04 KCI NaCl NazSOa and glaserite.. KzS04 and glaserite.. KCl and KzSOa.. KC1 and NaCl. NaCl and NazS04.. KzSOa, KCl, glaserite KCl, NaCl, glaserite.. NaCI, NazSO4, glaserite
.............. ... ............... ... ................. ................ si:i 4 .. ... ... ..... ....... 44:82 .... 51.93 7.21 41.36 40.15
... 52: io ... ...
5i:03 26.61 4i:k 27.01 14.58
EQUILIBRIUM DIAGRAMAT 100’
... ...
58100 8.61
KzSO4
1i:io
... ...
...
2.67
4.00 11.74
Fa
Gs He Is
L6 Me
Ne
...
.................. .................. .................
...
.......
...
.. ...
with which solid glaserite is in equilibrium. Some further details of these diagrams will be described in the following paper. UNIVERSITY O F CALIFORNIA BERKELEY
... ... 9.72
17.95 1.90
9.26
Sum
Be Ce De
MOLSPER 1000 MOLSOF WATER, OF SOLUTIONS SATURATEDAT 100° Saturated with NazClz KzClz NazSOa KzSO4 Sum NazSO4 52.86 52,86 &SO4 ... 2i:07 24.07 KC1 6j:90 ... 67.90 NaCl ................ 60:81 ... 60.81 NazSOa and glaserite.. ... ... 52:88 14:68 66.96 KnSOa and glaserite.. . . . . 17.21 21.21 38.42 KzSOa and KC1 . . . . . 65:?6 ... 2.93 68.69 NaCl and KCI. 42:ZO 42.48 ... ... 84.68 NaCl and NazSOa.. 56.33 8.12 ... 64.45 K ~ S OKCI ~ glaserite. 4.91 60:41 , 3.24 68.56 KCl, NaC1,’glaserite.. 38.25 43.65 4.78 86.68 NaC1, NazS04, glaserite 55.22 12.31 li:37 78.90 IN
~
THE SEPARATION OF THE CHLORIDES AND SULFATES OF SODIUM AND POTASSIUM BY FRACTIONAL CRYSTALLIZATION
... ... ... ...
By WALTERC. BLASDALE Received March 20, 1918
TABLEVII-COMPOSITION, IN GRAMSPBR 100oG. OF WATER, O F SOLUTIONS SATURATED AT 75 Saturated with NaCl KC1 NazSOa KzSOa Sp. Gr. As NazSO4 43.41 1 286 Bs KZSO4 20:io 1:120 Cs KCl 49:jo 1,204 Dr NaCl.. 3;:j5 1.183 Es NazSO4 and glaserite.. 4i:06 ii:?7 11332 Fs KzS04 and glaserite.. 10.09 18.60 1.183 48:;s 2.12 Gs KCI and KzS04.. Hs KCl and NaCl. 2?:87 29.06 1:i49 Ir NaCl and NazSO4.. 35.46 6.67 1.210 LI KzSOa, KC1, glaserite . 5.71 42:;s , , 2.83 1.223 MI KCl NaCl, glaserite. 25.45 29.38 3.33 1.257 Ns N a d l , NazSO4, glaserite 28.28 15.72 8.88 1.253
Relatively little use has been made in the industries of d a t a similar t o t h a t presented in t h e preceding article, ................. ... although the possibility of doing SO was indicated by ................. ... ................. ... ... van% Hoff’ and has recently been discussed by Hilde.............. ... ... ... brand2 as applied t o the utilization of t h e bittern of . . . . ..... ... sea water. I n this paper the d a t a referred t o will be ....... ... ... utilized in suggesting and testing t h e efficiencies of ... ... . methods for t h e separation of certain pairs of salts . ... ... which yield a common ion, and for the recovery of TABLE VIII-COMPOSITION, I N MOLS PER 1000 %OLS OF WATER, OF SOLUpotassium salts from two classes of materials which TIONS SATURATED AT 75 are of special importance t o the states of t h e Pacific Saturated with NazClz KzClz NazS04 KzSO4 Sum As NazS0: . . . . . . . . . . . . . . . . . ... 55.03 55.03 Coast. The first is the ash of kelp, which is already Bs KzS04 . . . . . . . . . . . . . . . . . . ... 2i:io 21.50 ... ... 60.02 Cn KCl. ................ 66102 produced on a large scale in t h e state of California; DS NaCl ............... 58: i 7 ... ... 58.17 Es NazSO4 and glaserite.. ,.. ... 5i:i4 12.17 65.51 the second includes certain natural brines found in t h e F r KzSOa and glaserite. . . . . . 12.80 19.23 32.03 desert regions of California, Nevada and Utah. Many Gs KC1 and KzS04 ...... 58’90 ... 2.19 61.09 Hs KC1 and NaCI ........ 42194 35: 11 ... ... 78.05 of the latter contain small amounts of carbonates, I 6 NaCl and NazSO4.. ... 54.64 8.48 ... 63.12 Ls KzSO:, KCl, glaserite.. 8.80 51145 ... 2.93 63.18 bicarbonates and borates which would make i t necesM6 KC1 NaCl glaserite.. 39.23 35.50 4.23 ... 78.96 ... 73.82 N6 N a d l , NarS‘04, glaserite 43.57 18.99 11.26 sary t o modify t o some extent any process based upon TABLEIX-COMPOSITION, IN GRAMSPER 100 G. 2” WATER,OF SOLUTIONSthese d a t a ; others contain such large proportions of SATURATED AT 100 these substances as t o make a n entirely new set of d a t a Saturated with NaCl KC1 NazSO4 KzSO4 Sp. Gr. A6 NazSO4 .............. ... ... 41.68 1.264 necessary. Be &SO4 ............... ... 1.134 ... 2i 44
................. ..............
Cs KC1 De NaCI.. NazS04 and glaserite.. . KzSO: and glaserite.. Ge KzSOa and KCl He NaCl and KC1.. ...... I e NaCl and NazSOd.. Le KzSO4, KC1, glaserite Me KCl, NaC1, glaserite.,.. NE NaCI, NazSO4, glaserite E6 F 6
39: 40
...
. ...... 2;:...39 .... 36.56 3.19 24.82 35.84
56:i0
...
...
...
4 i .’io 13.57
1i:fiz 20.51 2.83
...
5i:i3 35.16 50:Ol 36.13 10.18
... ...
6.41
...
...
...
3.24
...
ii:0o
3.77
1.217 1.175 1.326 1.213 1.225 1.253 1.204 1.233 1.269 1.256
I-SEPARATION
O F POTASSIUM CHLORIDE F R O M SODIUM CHLORIDE
The behavior upon evaporation of solutions containing different proportions of these salts can be easily 1 2
“Zur Bildung der ozeanischen Salzablagerung,” 1906. THIS JOURNAL, 10 (1918). 96.
