You-iggy

3Na2HPO4 + 3NH3 🔥→ 2Na3PO4 + (NH4)3PO4

The reaction of sodium hydrogenphosphate and ammonia yields sodium phosphate and ammonium phosphate. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

General equation

Reaction of acid salt and base
Acid saltBrønsted acid + BaseBrønsted base
SaltConjugate base + (H2O)
Reaction of acid salt and non hydroxide base
Acid saltBrønsted acid + Non hydroxide baseBrønsted base
SaltConjugate acid base

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na2HPO4Sodium hydrogenphosphate3
Brønsted acid
Acid salt
NH3Ammonia3
Brønsted base
Base
Non hydroxide base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na3PO4Sodium phosphate2
Conjugate base
Conjugate acid base
Salt
(NH4)3PO4Ammonium phosphate1
Conjugate base
Conjugate acid base
Salt

Thermodynamic changes

Changes in standard condition

Reaction of sodium hydrogenphosphate and ammonia
3Na2HPO4Crystalline solid + 3NH3Gas
🔥
2Na3PO4Crystalline solid + (NH4)3PO4Crystalline solid
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−124.1
−41.37
per 1 mol of
−41.37
per 1 mol of
−62.05
per 1 mol of
−124.1

Changes in aqueous solution

Reaction of sodium hydrogenphosphate and ammonia
ΔrG52.8 kJ/mol
K0.56 × 10−9
pK9.25
3Na2HPO4Ionized aqueous solution + 3NH3Un-ionized aqueous solution
🔥
2Na3PO4Ionized aqueous solution + (NH4)3PO4Ionized aqueous solution
Standard enthalpy
of reaction
ΔrH°
kJ · mol−1
Standard
Gibbs energy
of reaction
ΔrG°
kJ · mol−1
Standard entropy
of reaction
ΔrS°
J · K−1 · mol−1
Standard heat
capacity of reaction
at constant pressure
ΔrCp°
J · K−1 · mol−1
per 1 mol of
Equation
−112.752.8−557
−37.5717.6−186
per 1 mol of
−37.5717.6−186
per 1 mol of
−56.3526.4−279
per 1 mol of
−112.752.8−557

Thermodynamic data of reactants

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Na2HPO4 (cr)-1748.1[1]-1608.2[1]150.50[1]135.31[1]
Na2HPO4 (ai)-1772.38[1]-1612.98[1]84.5[1]
Na2HPO4 (cr)
2 hydrate
-2346.0[1]-2088.5[1]221.3[1]
Na2HPO4 (cr)
7 hydrate
-3821.7[1]-3279.8[1]434.59[1]
Na2HPO4 (cr)
12 hydrate
-5297.8[1]-4467.8[1]633.83[1]
NH3 (g)-46.11[1]-16.45[1]192.45[1]35.06[1]
NH3 (ao)-80.29[1]-26.50[1]111.3[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas, (ao):Un-ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard enthalpy
of formation
ΔfH°
kJ · mol−1
Standard Gibbs
energy of
formation
ΔfG°
kJ · mol−1
Standard
molar entropy
S°
J · K−1 · mol−1
Standard molar
heat capacity at
constant pressure
Cp°
J · K−1 · mol−1
Na3PO4 (cr)-1917.40[1]-1788.80[1]173.80[1]153.47[1]
Na3PO4 (ai)-1997.9[1]-1804.5[1]-43.3[1]
(NH4)3PO4 (cr)-1671.9[1]
(NH4)3PO4 (ai)-1674.9[1]-1256.6[1]117[1]
(NH4)3PO4 (cr)
3 hydrate
-2555.6[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution

References

List of references

  1. 1