Section: 5 | Aqueous Solubility of Inorganic Compounds at Various Temperatures |

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AQUEOUS SOLUBILITY OF INORGANIC COMPOUNDS AT VARIOUS TEMPERATURES

The solubility of over 300 common inorganic compounds in water is tabulated here as a function of temperature. Solubility is defined as the concentration of the compound in a solution that is in equilibrium with a solid phase at the specified temperature. In this table the solid phase is generally the most stable crystalline phase at the temperature in question. An asterisk * on solubility values in adjacent columns indicates that the solid phase changes between those two temperatures (usually from one hydrated phase to another or from a hydrate to the anhydrous solid). In such cases the slope of the solubility vs. temperature curve may show a discontinuity.

All solubility values are expressed as mass percent of solute, 100 × w₂, where

w₂ = m₂/(m₁ + m₂)

and m₂ is the mass of solute and m₁ the mass of water. This quantity is related to other common measures of solubility as follows:

Molarity: c₂ = 1000ρw₂/M₂
Molality: m₂ = 1000w₂/M₂(1-w₂)
Mole fraction: x₂ = (w₂/M₂)/{(w₂/M₂) + (1-w₂)/M₁}
Mass of solute per 100 g of H₂O: r₂ = 100w₂/(1-w₂)

Here M₂ is the molar mass of the solute and M₁ = 18.015 g/mol is the molar mass of water; ρ is the density of the solution in g cm^-3.

The data in the table have been derived from the references indicated; in many cases the data have been refitted or interpolated in order to present solubility at rounded values of temperature. Where available, values were taken from the IUPAC Solubility Data Series (Ref. 1) or related papers in the Journal of Physical and Chemical Reference Data (Refs. 2 to 5), which present carefully evaluated data.

The solubility of sparingly soluble compounds that do not appear in this table may be calculated from the data in the table “Solubility Product Constants of Inorganic Salts.” Solubility of inorganic gases may be found in the table “Solubility of Selected Gases in Water.” Both tables are in this section.

Compounds are listed alphabetically by formula.

References

Solubility Data Series, International Union of Pure and Applied Chemistry. Volumes 1 to 53 were published by Pergamon Press, Oxford, from 1979 to 1994; subsequent volumes were published by Oxford University Press, Oxford. The number following the colon is the volume number in the series. Current reports in the series appear in the Journal of Physical and Chemical Reference Data.
Clever, H. L., and Johnston, F. J., J. Phys. Chem. Ref. Data, 9, 751, 1980. [https://doi.org/10.1063/1.555628]
Marcus, Y., J. Phys. Chem. Ref. Data, 9, 1307, 1980. [https://doi.org/10.1063/1.555633]
Clever, H. L., Johnson, S. A., and Derrick, M. E., J. Phys. Chem. Ref. Data, 14, 631, 1985. [https://doi.org/10.1063/1.555732]
Clever, H. L., Johnson, S. A., and Derrick, M. E., J. Phys. Chem. Ref. Data, 21, 941, 1992. [https://doi.org/10.1063/1.555909]
Söhnel, O., and Novotny, P., Densities of Aqueous Solutions of Inorganic Substances, Elsevier, Amsterdam, 1985.
Krumgalz, B.S., Mineral Solubility in Water at Various Temperatures, Israel Oceanographic and Limnological Research Ltd., Haifa, 1994.
Potter, R. W., and Clynne, M. A., J. Research U.S. Geological Survey, 6, 701, 1978; Clynne, M. A., and Potter, R. W., J. Chem. Eng. Data, 24, 338, 1979.
Marshal, W. L., and Slusher, R., J. Phys. Chem., 70, 4015, 1966; Knacke, O., and Gans, W., Zeit. Phys. Chem., NF, 104, 41, 1977. [https://doi.org/10.1021/j100884a044]
Stephen, H., and Stephen, T., Solubilities of Inorganic and Organic Compounds, Vol. 1, Macmillan, New York, 1963.

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Aqueous Solubility of Inorganic Compounds in Mass% as a Function of Temperature

Mol. form.	Name	CAS Reg. No.	Mol. Wt.	0 °C	10 °C	20 °C	25 °C	30 °C	40 °C	50 °C	60 °C	70 °C	80 °C	90 °C	100 °C	Ref.
Continued on next page...
AgBrO₃	Silver(I) bromate	7783-89-3	235.770				0.193							1.32		7
AgClO₂	Silver(I) chlorite	7783-91-7	175.320	0.17	0.31	0.47	0.55	0.64	0.82	1.02	1.22	1.44	1.66	1.88	2.11	7
AgClO₃	Silver(I) chlorate	7783-92-8	191.319				15									7
AgClO₄	Silver(I) perchlorate	7783-93-9	207.319	81.6	83.0	84.2	84.8	85.3	86.3	86.9	87.5	87.9	88.3	88.6	88.8	6
AgNO₂	Silver(I) nitrite	7783-99-5	153.874	0.155			0.413									7
AgNO₃	Silver(I) nitrate	7761-88-8	169.873	55.9	62.3	67.8	70.1	72.3	76.1	79.2	81.7	83.8	85.4	86.7	87.8	6
Ag₂SO₄	Silver(I) sulfate	10294-26-5	311.799	0.56	0.67	0.78	0.83	0.88	0.97	1.05	1.13	1.20	1.26	1.32	1.39	7
AlCl₃	Aluminum chloride	7446-70-0	133.341	30.84	30.91	31.03	31.10	31.18	31.37	31.60	31.87	32.17	32.51	32.90	33.32	7
Al(ClO₄)₃	Aluminum perchlorate	14452-39-2	325.334	54.9										64.4		7
AlF₃	Aluminum fluoride	7784-18-1	83.977	0.25	0.34	0.44	0.50	0.56	0.68	0.81	0.96	1.11	1.28	1.45	1.64	7
Al(NO₃)₃	Aluminum nitrate	13473-90-0	212.997	37.0	38.2	39.9	40.8	42.0	44.5	47.3	50.4	53.8^*			61.5^*	6
Al₂(SO₄)₃	Aluminum sulfate	10043-01-3	342.151	27.5			27.8	28.2	29.2	30.7	32.6	34.9	37.6	40.7	44.2	7
As₂O₃	Arsenic(III) oxide (arsenolite)	1327-53-3	197.841	1.19	1.48	1.80	2.01	2.27	2.86	3.43	4.11	4.89	5.77	6.72	7.71	10
BaBr₂	Barium bromide	10553-31-8	297.135	47.6	48.5	49.5	50.0	50.4	51.4	52.5	53.5	54.5	55.5	56.6	57.6	6
Ba(BrO₃)₂	Barium bromate	13967-90-3	393.131	0.285	0.442	0.656	0.788	0.935	1.30	1.74	2.27	2.90	3.61	4.40	5.25	1:14
Ba(C₂H₃O₂)₂	Barium acetate	543-80-6	255.416	37.0			44.2									7
BaCl₂	Barium chloride	10361-37-2	208.233	23.30	24.88	26.33	27.03	27.70	29.00	30.27	31.53	32.81	34.14	35.54	37.05	8
Ba(ClO₂)₂	Barium chlorite	14674-74-9	272.231	30.5			31.3								44.7	7
Ba(ClO₃)₂	Barium chlorate	13477-00-4	304.229	16.90	21.23	23.66	27.50	29.43	33.16	36.69	40.05	43.04	45.90	48.70	51.17	1:14

^*Solid phase changes between these temperatures

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