Table shows solubility of various substances under different temperature given in grams of dissoluted substance per 100g of water.

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other inorganic#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
ammonia	NH₃	90	53	31	-	-	-

gases#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
ammonia	NH₃	90	53	31	-	-	-
nitrogen	N₂	0.2914	0.1922	0.1463	0.1265	0.119	0.1178
carbon dioxide	CO₂	0.3346	0.1688	0.0973	0.0576	-	-
hydrogen chloride	HCl	82.3	72	63.3	56.1	-	-
hydrogen sulfuride	H₂S	-	0.385	-	-	-	-
ethyne	C₂H₂	-	0.117	-	-	-	-
nitrogen (II) oxide	NO	-	0.0056	-	-	-	-
nitrogen (I) oxide	N₂O	-	0.112	-	-	-	-
chlorine	Cl₂	4.61	2.23	1.44	1.02	0.68	-
hydrogen	H₂	0.0192	0.0162	0.0146	0.0143	0.0143	0.0143
oxygen	O₂	0.6993	0.4433	0.3303	0.2789	0.2517	0.246

oxides#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
carbon dioxide	CO₂	0.3346	0.1688	0.0973	0.0576	-	-
carbon monoxide	CO	0.035	0.023	0.018	0.015	0.014	0.014
nitrogen (II) oxide	NO	-	0.0056	-	-	-	-
nitrogen (I) oxide	N₂O	-	0.112	-	-	-	-

salts#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
potassium bromide	KBr	53.5	65.2	75.5	85.5	95	104
potassium chloride	KCl	27.6	34	40	45.5	51.1	56.7
potassium jodide	KI	127.5	144	160	176	192	208
silver chloride	AgCl	-	0.00015	-	-	-	-
potassium chromate	K₂CrO₄	58.2	61.7	65.2	68.6	72.1	75.6
silver iodide	AgI	-	-	-	0.000003	-	-
silver (I) sulfate (VI)	Ag₂SO₄	0.57	0.79	0.97	1.14	1.28	1.39
barium chromate (VI)	BaCrO₄	0.0002	0.00037	-	-	-	-
barium sulfate (VI)	BaSO₄	0.000115	0.00024	-	-	-	0.000413
mercury (I) chloride	Hg₂Cl₂	0.00014	0.0002	-	-	-	-
mercury (II) chloride	HgCl₂	3.5	6.1	9.3	14	23.1	38
silver nitrate (V)	AgNO₃	122	222	376	525	669	952
aluminium sulfate (VI)	Al₂(SO₄)₃	23.8	26.7	31.4	37.2	42.2	47.1
barium chloride	BaCl₂	31.6	35.7	40.7	46.4	52.4	58.8
barium nitrate (III)	Ba(NO₃)₂	5	9.2	14.2	20.3	27	34.2
potassium thiocyanate	KSCN	63.9	68.5	-	-	-	-
potassium nitrate (III)	KNO₂	73.6	74.9	77	-	-	80.5
potassium nitrate (V)	KNO₃	13.3	31.6	63.9	110	169	246
sodium nitrate (V)	NaNO₃	73	88	104	124	148	180
potassium sulfate (VI)	K₂SO₄	7.35	11.11	14.76	18.17	21.75	24.1
ammonium thiocyanate	NH₄SCN	54.5	63	-	-	-	-
ammonium oxalate	(NH₄)₂C₂O₄	2.1	4.2	9.3	-	-	-
ammonium chloride	NH₄Cl	29.4	37.2	45.8	55.2	65.6	77.3
ammonium magnesium phosphate	NH₄MgPO₄	0.023	0.052	0.036	0.04	0.019	-
ammonium nitrate (V)	NH₄NO₃	118.3	192	297	421	580	871
lead (II) nitrate (V)	Pb(NO₃)₂	38.8	56.3	75	96	115	138.8
ammonium sulfate (VI)	(NH₄)₂SO₄	70.6	75.4	81	88	95.3	103.3
sodium chloride	NaCl	35.7	36	36.6	37.3	38.4	39.8

inorganic acids#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
hydrogen chloride	HCl	82.3	72	63.3	56.1	-	-
hydrogen sulfuride	H₂S	-	0.385	-	-	-	-

hydrocarbons#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
ethyne	C₂H₂	-	0.117	-	-	-	-

hydroxides#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
calcium hydroxide	Ca(OH)₂	0.185	0.165	0.141	0.116	0.094	0.077
barium hydroxide	Ba(OH)₂	1.67	3.89	8.22	20.94	101.4	-

halogens#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
chlorine	Cl₂	4.61	2.23	1.44	1.02	0.68	-
bromine	Br₂	4.22	3.2	-	-	-	-
jodine	I₂	-	0.029	0.056	-	-	-

liquids#

Substance	Molecular formula	0 °C	20 °C	40 °C	60 °C	80 °C	100 °C
bromine	Br₂	4.22	3.2	-	-	-	-

Some facts#

Solubility is the ability of one chemical substance to dissolve in another one called solvent.
As a result of dissolution, a homogeneous solution is formed.
Depending on the needs, many different units of solubility are used, e.g.:
- grams per 100 grams of solvent (g / 100 g),
- grams per 1 kilogram of solvent (g / 1 kg),
- grams per 100 cm³ of solvent (g / 100 cm³),
- grams per litre of solvent, (g/l),
- moles per litre of solvent (n/l),
- etc.
The solubility for a specific substances pair (solvent and dissoluted substance) depends on many factors. Among others, these are:
- kind of dissolved substance,
- kind of solvent,
- temperature,
- pressure,
- concentration of common ions in solution,
- complexation,
- the ion strength of the solution,
- crystal size,
- etc.
The solubility of gases is inversely proportional to temperature, i.e. it decreases with temperature.
At a constant temperature, the solubility of gases is met by Henry's law:

$c = k \times p$
where:
- c - gas concentration in the liquid,
- k - proportionality coefficient specific for selected gas, solubility and temperature,
- p - partial pressure of gas.

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