Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°. II. Effect of Sodium Hydroxide and Sodium Carbonate<sup>1</sup>

Schroeder, W. C.; Berk, A. A.; Gabriel, Alton

doi:10.1021/ja01296a047

Cited by 15 publications

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“…Other solid species that can form from this system at temperatures above 100 °C include sodium carbonate, sodium carbonate monohydrate, and sodium sulfate. 2,3 It is interesting to note that the experimental procedures followed by the researchers cited above achieved apparent equilibrium by adding excess amounts of sodium carbonate and sodium sulfate crystals to solutions of these solutes. The primary concern with this approach is that it might have extended the domains of sodium carbonate and sodium sulfate if the system had not reached equilibrium.…”

Section: Introductionmentioning

confidence: 99%

Structure of Burkeite and a New Crystalline Species Obtained from Solutions of Sodium Carbonate and Sodium Sulfate

and

Rousseau

2003

J. Phys. Chem. B

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It has long been recognized that crystallization from solutions of sodium carbonate and sodium sulfate can produce anhydrous or hydrated forms of the pure species or, in certain composition ranges, burkeitea crystalline double salt of sodium carbonate and sodium sulfate having the nominal stoichiometry Na2CO3·2Na2SO4. The present work examines and explains the observed variation of burkeite composition and identifies a new double-salt species whose composition has been determined to contain approximately 2 moles of sodium carbonate per mole of sodium sulfate. The new species was formed at 115 °C from solutions whose compositions range from approximately 5 moles of sodium carbonate per mole of sodium sulfate to 7 moles of sodium carbonate per mole of sodium sulfate.

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Section: Introductionmentioning

confidence: 99%

Structure of Burkeite and a New Crystalline Species Obtained from Solutions of Sodium Carbonate and Sodium Sulfate

and

Rousseau

2003

J. Phys. Chem. B

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“…The first three papers of this series have presented data for the solubility of sodium sulfate in solutions containing sodium hydroxide, sodium chloride, sodium carbonate and sodium phosphate at temperatures above 100°. [6][7] The utility of this information should be increased materially by the determination of the degree of accuracy with which the equilibrium values can be applied to a system undergoing evaporation. In this paper comparison is made between the amount of sodium sulfate in a solution from which steam is being removed, and the amount of sodium sulfate present in the same solution at equilibrium.…”

Section: Effect Of Sodium Hydroxide On the Systemmentioning

confidence: 99%

“…The operation of the bomb was essentially as described in the first paper of this series. 6 Solubility of Sodium Phosphate in Water and Sodium Hydroxide Solutions Mulder7 and Apfel8 have shown that the solubility of trisodium phosphate in water increases rapidly with temperature from 0 to above 100°. Above 25°Mulder's values as shown in Fig.…”

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Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°.¹ III. Effect of Sodium Hydroxide and Sodium Phosphate

Schroeder¹,

Berk²,

Gabriel³

1937

J. Am. Chem. Soc.

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The present paper is the third in a series presenting the results of an investigation carried out in coiiperation with the Joint Research Committee on Boiler Feedwater Studies dealing with the solubility of sodium sulfate in various solutions in the temperature range from 150 to 350". The first paper5 gave solubility data for sodium SUIfate, in sodium hydroxide-sodium chloride solutions, and the secondfi for sodium sulfate in SOdium hydroxide-sodium carbonate solutions. This paper presents data for (1) a design for a new high temperature solubility bomb, ( 2 ) the solubility of trisodium phosphate in water and in sodium hydroxide solutions, (3) data for the system sodium sulfate-trisodium phosphate-water, (4) the solid phases in this system, and (5) the effect of sodium hydroxide on the system. These studies involving the phosphate are the most complicated, and perhaps the most interesting, of the three solubility investigations. High Temperature Solubility BombThe bomb originally used in the study of the high temperature solubility equilibria of sodium sulfate has been described in the first paper5 of this series. As the investigation proceeded several disadvantageous features were found in this equipment. It has been redesigned and the difficulties have been corrected in the bomb shown in Fig. 1. The body is open a t both ends to make for easy machining] with the sampler as well as the bottom held in place by studs. The necessary seals are formed by metal-to-metal contact between seats machined a t 60" so that no gaskets or material other than the bomb metal comes in contact with the solution. The valve (I) Published by permission of the Director, U. S. Bureau of Mines. (Not subject to copyright.) (2) Research chemical engineer, Joint Research Committee on Boiler Feed-Water Studies, attached to Eastern Experiment Station, stem is large enough to eliminate sticking and danger of twisting off. SQUARE FOR WRENCH ~ PACKING Fig. l.-Solubility bomb (dimensions in inches) : firessure, 200 atmospheres or 3000 lb. per sq. in.; volume, L U L~I W I L U saiiryicr 111 p a c e YJU CC., UCIUW aamyirr IYW CF., above sampler 110 cc., sampler 18 cc.The sampler is enclosed in the bomb to ensure sampling a t the operating temperature, and the end may be equipped with a filter of carbon or 843-849 (1936) ' fine wire screen if this is desirable. Crane pack-

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“…Some studies have been done on the solubility for the subsystems of the five-component system Na 2 CO 3 + NaHCO 3 + Na 2 SO 4 + NaCl + H 2 O at 150 °C (Eddy and Menzies, 1940;Itkina and Kohova, 1955;Palkova and Ahumov, 1962;Schroeder et al, 1935Schroeder et al, , 1936Stephen and Stephen, 1979;Waldeck et al, 1934;Zhang et al, 1991), but the studies of the phase equilibria for the ternary systems NaHCO 3 + NaCl + H 2 O and NaHCO 3 + Na 2 SO 4 + H 2 O, the quaternary systems Na 2 CO 3 + NaHCO 3 + Na 2 SO 4 + H 2 O, Na 2 CO 3 + NaHCO 3 + NaCl + H 2 O, and NaHCO 3 + Na 2 SO 4 + NaCl + H 2 O, and the five-component system Na 2 CO 3 + NaHCO 3 + Na 2 SO 4 + NaCl + H 2 O at 150 °C have not been reported so far.…”

Section: Introductionmentioning

confidence: 99%

Solubility in the Na₂CO₃ + NaHCO₃ + Na₂SO₄ + NaCl + H₂O System and Its Subsystems at 150 °C

Zhang²,

Wu³

et al. 1999

J. Chem. Eng. Data

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Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°. II. Effect of Sodium Hydroxide and Sodium Carbonate¹

Cited by 15 publications

References 0 publications

Structure of Burkeite and a New Crystalline Species Obtained from Solutions of Sodium Carbonate and Sodium Sulfate

Structure of Burkeite and a New Crystalline Species Obtained from Solutions of Sodium Carbonate and Sodium Sulfate

Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°.¹ III. Effect of Sodium Hydroxide and Sodium Phosphate

Solubility in the Na₂CO₃ + NaHCO₃ + Na₂SO₄ + NaCl + H₂O System and Its Subsystems at 150 °C

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Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°. II. Effect of Sodium Hydroxide and Sodium Carbonate1

Cited by 15 publications

References 0 publications

Structure of Burkeite and a New Crystalline Species Obtained from Solutions of Sodium Carbonate and Sodium Sulfate

Structure of Burkeite and a New Crystalline Species Obtained from Solutions of Sodium Carbonate and Sodium Sulfate

Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°.1 III. Effect of Sodium Hydroxide and Sodium Phosphate

Solubility in the Na2CO3 + NaHCO3 + Na2SO4 + NaCl + H2O System and Its Subsystems at 150 °C

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Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°. II. Effect of Sodium Hydroxide and Sodium Carbonate¹

Solubility Equilibria of Sodium Sulfate at Temperatures from 150 to 350°.¹ III. Effect of Sodium Hydroxide and Sodium Phosphate

Solubility in the Na₂CO₃ + NaHCO₃ + Na₂SO₄ + NaCl + H₂O System and Its Subsystems at 150 °C