Table shows dissociation constants of selected chemical substances in temperature 298K (25°C).

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other inorganic#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
ammonia	NH₃	0.000026	-	-

gases#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
ammonia	NH₃	0.000026	-	-
hydrogen chloride	HCl	100000000	-	-
hydrogen cyanide	HCN	7.5×10^-10	-	-
hydrogen fluoride	HF	0.00063	-	-
hydrogen jodide	HI	10000000000	-	-
hydrogen sulfuride	H₂S	6×10^-8	1×10^-14	-
dimethylamine	(CH₃)₂NH	0.00051	-	-
trimethylamine	(CH₃)₃N	0.0063	-	-
ethylamine	C₂H₅NH₂	0.00047	-	-

inorganic acids#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
hydrogen bromide	HBr	3000000000	-	-
hydrogen chloride	HCl	100000000	-	-
hydrogen cyanide	HCN	7.5×10^-10	-	-
hydrogen fluoride	HF	0.00063	-	-
hydrogen jodide	HI	10000000000	-	-
hydrogen sulfuride	H₂S	6×10^-8	1×10^-14	-
arsenous (III) acid	H₃AsO₃	6×10^-10	1.7×10^-14	-
arsenous (V) acid	H₃AsO₄	0.0056	1.1×10^-7	3.9×10^-12
boric acid	H₃BO₃	5.8×10^-10	1.8×10^-13	1.6×10^-14
hypobromous acid	HBrO	2×10^-9	-	-
bromic (V) acid	HBrO₃	0.2	-	-
fulminic acid	HCNO	0.00012	-	-
carbonic acid	H₂CO₃	4.5×10^-7	4.7×10^-11	-
chloric (V) acid	HClO₃	6.3	-	-
chloric (I) acid	HClO	3.2×10^-8	-	-
chloric (III) acid	HClO₂	0.01	-	-
hypoiodous acid	HIO	1×10^-10	-	-
iodic (V) acid	HIO₃	0.16	-	-
iodic (VII) acid	HIO₄	0.023	-	-
nitrous (III) acid	HNO₂	0.0002	-	-
nitrous (V) acid	HNO₃	25	-	-
phosphoric (V) acid	H₃PO₄	0.0075	6.3×10^-8	1.3×10^-12
sulfurous (IV) acid	H₂SO₃	0.016	6.3×10^-8	-
sulfurous (VI) acid	H₂SO₄	1000	0.012	-

phenols#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
phenol	C₆H₅OH	1×10^-10	-	-

liquids#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
phenol	C₆H₅OH	1×10^-10	-	-
formic acid	HCOOH	0.00018	-	-
lactic acid	CH₃CH(OH)COOH	0.00014	-	-
acetate acid	CH₃COOH	0.000018	-	-
propionic acid	CH₃CH₂COOH	0.000013	-	-
methylamine	CH₃NH₂	0.00044	-	-
phenylamine (aniline)	C₆H₅NH₂	3.8×10^-10	-	-
hypobromous acid	HBrO	2×10^-9	-	-

carboxylic acids#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
formic acid	HCOOH	0.00018	-	-
lactic acid	CH₃CH(OH)COOH	0.00014	-	-
oxalic acid	(COOH)₂	0.054	0.000054	-
acetate acid	CH₃COOH	0.000018	-	-
propionic acid	CH₃CH₂COOH	0.000013	-	-
salicylic acid	OHC₆H₄COOH	0.0013	1.5×10^-14	-
benzoic acid	C₆H₅COOH	0.0066	-	-

solids#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
oxalic acid	(COOH)₂	0.054	0.000054	-
salicylic acid	OHC₆H₄COOH	0.0013	1.5×10^-14	-
benzoic acid	C₆H₅COOH	0.0066	-	-

amines#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
methylamine	CH₃NH₂	0.00044	-	-
dimethylamine	(CH₃)₂NH	0.00051	-	-
trimethylamine	(CH₃)₃N	0.0063	-	-
ethylamine	C₂H₅NH₂	0.00047	-	-
diethylamine	(C₂H₅)₂NH	0.00085	-	-
triethylamine	(C₂H₅)₃N	0.00074	-	-
phenylamine (aniline)	C₆H₅NH₂	3.8×10^-10	-	-

hydroxides#

Substance	Molecular formula	First dissociation constant K₁	Second dissociation constant K₂	Third dissociation constant K₃
zinc hydroxide	Zn(OH)₂	-	0.00004	-
copper (II) hydroxide	Cu(OH)₂	-	0.00013	-
iron (II) hydroxide	Fe(OH)₂	-	0.00013	-
iron (III) hydroxide	Fe(OH)₃	-	0.0025	-
aluminium hydroxide	Al(OH)₃	-	-	1.4×10^-9
silver (I) hydroxide	AgOH	0.00011	-	-

Some facts#

Dissociation constant is equilibrium constant written for the dissociation reaction.
If some acid dissociates in the aqueous solution proceeds according to the reaction:

$HA + H_2O \iff H_3O^+ + A^-$
then we can write the following dissociation constant for it:

$K=\dfrac{[H_{3}O^{+}][A^{-}]}{[HA][H_{2}O]}$
where:
- $K$ - dissociation constant of $HA$ acid,
- $[HA]$ - molar concentration of not dissociated acid $HA$ in an equilibrium state,
- $[H_2O]$ - molar concentration of water (solvent) in an equilibrium state,
- $[H_3O^+]$ - molar concentration of hydronium ions $H_3O^+$ in an equilibrium state,
- $[A^-]$ - molar concentration of acid anions in equilibrium.
Analogously if some alkali dissociates according to the reaction:

$BOH + H_2O \iff BH^+ + OH^-$
then we can write following dissociation constant:

$K=\dfrac{[BH^+][OH^{-}]}{[BOH][H_{2}O]}$
where:
- $K$ - dissociation constant of $BOH$ alkali,
- $[BOH]$ - molar concentration of not dissociated $BOH$ alkali in equlibrium state,
- $[H_2O]$ - molar concentration of water (solvent) in an equlibrium state,
- $[BH^+]$ - molar concentration of $BH^+$ cations in equlibrium state,
- $[OH^-]$ - molar concentartion of hydroxyl ions $OH^-$ in equlibrium state.
Other name for dissociation constant is ionization constant.
Dissociation constant is specific for given substance.
The dissociation constant (just like the equilibrium constant of other chemical reactions) depends on the temperature. Chemical tables usually give values for 278K (25°C) i.e. room temperature.

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