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3SrCl2 + 2K3PO4 💧→ Sr3(PO4)2↓ + 6KCl

The reaction of strontium chloride and potassium phosphate yields strontium phosphate and potassium chloride. 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

Oxidation state of each atom

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
SrCl2Strontium chloride3
Lewis acid
Very soluble in water
K3PO4Potassium phosphate2
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Sr3(PO4)2Strontium phosphate1
Lewis conjugate
Insoluble in water
KClPotassium chloride6
Non-redox product

Thermodynamic changes

Changes in standard condition

Reaction of strontium chloride and potassium phosphate
3SrCl2Crystalline solidα + 2K3PO4Crystalline solid
💧
Sr3(PO4)2Crystalline solid + 6KClCrystalline 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
3354.3
per 1 mol of
1118.1
1677.2
3354.3
per 1 mol of
559.05

Changes in aqueous solution

Reaction of strontium chloride and potassium phosphate
3SrCl2Ionized aqueous solution + 2K3PO4Ionized aqueous solution
💧
Sr3(PO4)2Crystalline solid + 6KClIonized 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
3780.2
per 1 mol of
1260.1
1890.1
3780.2
per 1 mol of
630.03

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
SrCl2 (cr)
α
-828.9[1]-781.1[1]114.85[1]75.60[1]
SrCl2 (g)-485.8[1]-496.2[1]310.81[1]55.77[1]
SrCl2 (ai)-880.10[1]-821.91[1]80.3[1]
SrCl2 (cr)
1 hydrate
-1136.8[1]-1036.3[1]172[1]120.1[1]
SrCl2 (cr)
2 hydrate
-1438.0[1]-1281.8[1]218[1]160.2[1]
SrCl2 (cr)
6 hydrate
-2623.8[1]-2240.92[1]390.8[1]
K3PO4 (cr)-1950.2[1]
K3PO4 (ai)-2034.7[1]-1868.7[1]87.2[1]
* (cr):Crystalline solid, (g):Gas, (ai):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
Sr3(PO4)2 (cr)-412.29[1]
KCl (cr)-436.747[1]-409.14[1]82.59[1]51.30[1]
KCl (g)-214.14[1]-233.0[1]239.10[1]36.48[1]
KCl (ai)-419.53[1]-414.49[1]159.0[1]-114.6[1]
* (cr):Crystalline solid, (g):Gas, (ai):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)