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H3PO4 + 2NaOH → Na2HPO4 + 2H2O

The reaction of phosphoric acid and sodium hydroxide yields sodium hydrogenphosphate and water (Other reactions are here). 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 reactions
  5. 5Related categories

Reaction data

Chemical equation

General equation

Reaction of acid and base
AcidBrønsted acid + BaseBrønsted base
SaltConjugate base + (H2O)(Conjugate acid)
Reaction of acid and hydroxide base
AcidBrønsted acid + Hydroxide baseBrønsted base
SaltConjugate base + H2OConjugate acid
Reaction of weak acid and strong base
Weak acidBrønsted acid + Strong baseBrønsted base
Salt of weak acid and strong baseConjugate base + (H2O)(Conjugate acid)

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
H3PO4Phosphoric acid1
Brønsted acid
Acid
Weak acid
NaOHSodium hydroxide2
Brønsted base
Base
Hydroxide base
Strong base

Products

Chemical formulaNameCoefficientTypeType in general
equation
Na2HPO4Sodium hydrogenphosphate1
Conjugate base
Salt
Salt of weak acid and strong base
H2OWater2
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition

Reaction of phosphoric acid and sodium hydroxide
ΔrG−204.4 kJ/mol
K6.45 × 1035
pK−35.81
H3PO4Crystalline solid + 2NaOHCrystalline solid
Na2HPO4Crystalline solid + 2H2OLiquid
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
−189.5−204.450.9160.75
per 1 mol of
−189.5−204.450.9160.75
per 1 mol of
−94.75−102.225.4530.38
−189.5−204.450.9160.75
per 1 mol of
−94.75−102.225.4530.38

Changes in aqueous solution (1)

Reaction of phosphoric acid and sodium hydroxide
ΔrG−106.40 kJ/mol
K4.37 × 1018
pK−18.64
H3PO4Un-ionized aqueous solution + 2NaOHIonized aqueous solution
Na2HPO4Ionized aqueous solution + 2H2OLiquid
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
−115.47−106.40−30.1
per 1 mol of
−115.47−106.40−30.1
per 1 mol of
−57.735−53.200−15.1
−115.47−106.40−30.1
per 1 mol of
−57.735−53.200−15.1

Changes in aqueous solution (2)

Reaction of phosphoric acid and sodium hydroxide
ΔrG−230.2 kJ/mol
K2.13 × 1040
pK−40.33
H3PO4Ionized aqueous solution + 2NaOHIonized aqueous solution
Na2HPO4Ionized aqueous solution + 2H2OLiquid
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
−126.4−230.2348.4
per 1 mol of
−126.4−230.2348.4
per 1 mol of
−63.20−115.1174.2
−126.4−230.2348.4
per 1 mol of
−63.20−115.1174.2

Changes in aqueous solution (3)

Reaction of phosphoric acid and sodium hydroxide
ΔrG−106.40 kJ/mol
K4.37 × 1018
pK−18.64
H3PO4Un-ionized aqueous solution + 2NaOHIonized aqueous solution
Na2HPO4Ionized aqueous solution + 2H2OLiquid
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
−115.47−106.40−30.1
per 1 mol of
−115.47−106.40−30.1
per 1 mol of
−57.735−53.200−15.1
−115.47−106.40−30.1
per 1 mol of
−57.735−53.200−15.1

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
H3PO4 (cr)-1279.0[1]-1119.1[1]110.50[1]106.06[1]
H3PO4 (l)-1266.9[1]
H3PO4 (ai)-1277.4[1]-1018.7[1]-220.3[1]
H3PO4 (ao)-1288.34[1]-1142.54[1]158.2[1]
H3PO4 (cr)
0.5 hydrate
-1431.3[1]-1242.1[1]129.16[1]126.02[1]
H3PO4 (cr)
1 hydrate
-1568.83[1]
NaOH (cr)-425.609[1]-379.494[1]64.455[1]59.54[1]
NaOH (g)-207.1[1]-210.0[1]228.43[1]48.37[1]
NaOH (ai)-470.114[1]-419.150[1]48.1[1]-102.1[1]
NaOH (cr)
1 hydrate
-734.543[1]-629.338[1]99.50[1]90.17[1]
NaOH (l)
2 hydrate
-1019.076[1]-873.091[1]195.979[1]239.41[1]
NaOH (l)
3.5 hydrate
-1459.798[1]-1236.356[1]286.089[1]354.43[1]
NaOH (l)
4 hydrate
-1605.15[1]-1356.64[1]318.70[1]
NaOH (l)
5 hydrate
-1894.31[1]-1596.34[1]386.06[1]
NaOH (l)
7 hydrate
-2469.02[1]-2073.80[1]526.31[1]
* (cr):Crystalline solid, (l):Liquid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (g):Gas

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
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]
H2O (cr)
H2O (l)-285.830[1]-237.129[1]69.91[1]75.291[1]
H2O (g)-241.818[1]-228.572[1]188.825[1]33.577[1]
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas

References

List of references

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)