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Na3PO4 + 3HClO4 → 3NaClO4 + H3PO4

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Reaction of sodium phosphate and perchloric acid
Na3PO4Sodium phosphate + 3HClO4Perchloric acid
⟶
3NaClO4Sodium perchlorate + H3PO4Phosphoric acid

The reaction of sodium phosphate and perchloric acid yields sodium perchlorate and phosphoric acid (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

Reaction of sodium phosphate and perchloric acid
Na3PO4Sodium phosphate + 3HClO4Perchloric acid
⟶
3NaClO4Sodium perchlorate + H3PO4Phosphoric acid

General equation

Reaction of salt of weak acid and strong acid with generating weak acid
Salt of weak acidBrønsted base + Strong acidBrønsted acid
⟶
Salt of strong acidConjugate base + Weak acidConjugate acid

Oxidation state of each atom

Reaction of sodium phosphate and perchloric acid

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
Na3PO4Sodium phosphate1
Brønsted base
Salt of weak acid
HClO4Perchloric acid3
Brønsted acid
Strong acid

Products

Chemical formulaNameCoefficientTypeType in general
equation
NaClO4Sodium perchlorate3
Conjugate base
Salt of strong acid
H3PO4Phosphoric acid1
Conjugate acid
Weak acid

Thermodynamic changes

Changes in standard condition

Reaction of sodium phosphate and perchloric acid
Na3PO4Crystalline solid + 3HClO4Liquid
⟶
3NaClO4Crystalline solid + H3PO4Crystalline 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
−389.8–––
per 1 mol of
−389.8–––
per 1 mol of
−129.9–––
per 1 mol of
−129.9–––
per 1 mol of
−389.8–––

Changes in aqueous solution (1)

Reaction of sodium phosphate and perchloric acid
◆
ΔrG−123.7 kJ/mol
K4.69 × 1021
pK−21.67
Na3PO4Ionized aqueous solution + 3HClO4Ionized aqueous solution
⟶
3NaClO4Ionized aqueous solution + H3PO4Un-ionized 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
−10.8−123.7378.5–
per 1 mol of
−10.8−123.7378.5–
per 1 mol of
−3.60−41.23126.2–
per 1 mol of
−3.60−41.23126.2–
per 1 mol of
−10.8−123.7378.5–

Changes in aqueous solution (2)

Reaction of sodium phosphate and perchloric acid
◆
ΔrG−123.7 kJ/mol
K4.69 × 1021
pK−21.67
Na3PO4Ionized aqueous solution + 3HClO4Ionized aqueous solution
⟶
3NaClO4Ionized aqueous solution + H3PO4Un-ionized 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
−10.8−123.7378.5–
per 1 mol of
−10.8−123.7378.5–
per 1 mol of
−3.60−41.23126.2–
per 1 mol of
−3.60−41.23126.2–
per 1 mol of
−10.8−123.7378.5–

Changes in aqueous solution (3)

Reaction of sodium phosphate and perchloric acid
◆
ΔrG0.1 kJ/mol
K0.96 × 100
pK0.02
Na3PO4Ionized aqueous solution + 3HClO4Ionized aqueous solution
⟶
3NaClO4Ionized aqueous solution + H3PO4Ionized 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
0.10.10.0–
per 1 mol of
0.100.100.0–
per 1 mol of
0.0330.0330.0–
per 1 mol of
0.0330.0330.0–
per 1 mol of
0.100.100.0–

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
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]–
HClO4 (l)-40.58[1]–––
HClO4 (ai)-129.33[1]-8.52[1]182.0[1]–
HClO4 (cr)
1 hydrate
-382.21[1]–––
HClO4 (l)
2 hydrate
-677.98[1]–––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid

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
NaClO4 (cr)-383.30[1]-254.85[1]142.3[1]–
NaClO4 (ai)-369.45[1]-270.41[1]241.0[1]–
NaClO4 (cr)
1 hydrate
-677.77[1]-494.29[1]190.8[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]–––
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (ao):Un-ionized aqueous solution

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)