NaH₂PO₄

Formula : NaH₂PO₄

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Dernière mise à jour le 25.01.2021

Individual properties (298.15 K)

M g·mol^-1	V° cm³·mol^-1	ΔGº_f J·mol^-1	ΔHº_f J·mol^-1	Sº J·mol^-1·k^-1	C_P J·mol^-1·K^-1
119.977		-1385974 (Ref.: Internal calculation)	-1536800 (Ref.: 82wag/eva) Wagman D.D., Evans W.H., Parker V.B., Schumm R.H., Halow I., Bailey S.M., Churney K.L., and Nutall R.L., 1982. The NBS Tables of Chemical Thermodynamic Properties. J. Phys. Chem. Ref. Data, 11, Suppl. 2.	127.500 (Ref.: 67and/cou) Andon R.J.L., Counsell J.F., Martin J.F., and Mash C.J., 1967. Thermodynamic properties of phosphorus compounds: II. Low temperature heat capacity and entropy of sodium mono-, di-, and triphosphates. J. Appl. Chem., 17, 65-70	116.86 (Ref.: 67and/cou) Andon R.J.L., Counsell J.F., Martin J.F., and Mash C.J., 1967. Thermodynamic properties of phosphorus compounds: II. Low temperature heat capacity and entropy of sodium mono-, di-, and triphosphates. J. Appl. Chem., 17, 65-70

C_P(T) = a + b·T + ·c·T^-2 (T in Kelvin)

a J·mol^-1·K^-1	*b 10³** J·mol^-1·K^-2	*c 10^-5** J·K·mol^-1	Maier Kelley Ref.
116.86	0.00	0.00	(Ref.: 67and/cou) Andon R.J.L., Counsell J.F., Martin J.F., and Mash C.J., 1967. Thermodynamic properties of phosphorus compounds: II. Low temperature heat capacity and entropy of sodium mono-, di-, and triphosphates. J. Appl. Chem., 17, 65-70

Reaction properties

NaH₂PO₄ ⇌ Na⁺ + H₂PO₄^-

298.15 K, 1 bar log₁₀K: 2.30 ΔH°_r:-6140 J·mol^-1

T(°C)	0	25	60	100	150	200	250	300
log₁₀K	2.37	2.30	2.16	1.98	1.72	1.42	1.05	0.53

log₁₀K(T) = A + B·T + C·T^-1 + D·log₁₀(T) + E·T⁻² (T in Kelvin)

A	B	C	D	E
-739.243221	-0.116134	40935.496523	269.084655	-2396714.773607