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2KHSO4 + Ca(OH)2 → K2SO4 + CaSO4 + 2H2O

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Reaction of potassium hydrogensulfate and calcium hydroxide
2KHSO4Potassium hydrogensulfate + Ca(OH)2Calcium hydroxide
⟶
K2SO4Potassium sulfate + CaSO4Calcium sulfate + 2H2OWater

The reaction of potassium hydrogensulfate and calcium hydroxide yields potassium sulfate, calcium sulfate, 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

Reaction of potassium hydrogensulfate and calcium hydroxide
2KHSO4Potassium hydrogensulfate + Ca(OH)2Calcium hydroxide
⟶
K2SO4Potassium sulfate + CaSO4Calcium sulfate + 2H2OWater

General equation

Reaction of acid salt and base
Acid saltBrønsted acid + BaseBrønsted base
⟶
SaltConjugate base + (H2O)
Reaction of acid salt and hydroxide base
Acid saltBrønsted acid + Hydroxide baseBrønsted base
⟶
SaltConjugate base + H2OConjugate acid

Oxidation state of each atom

Reaction of potassium hydrogensulfate and calcium hydroxide

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
KHSO4Potassium hydrogensulfate2
Brønsted acid
Acid salt
Ca(OH)2Calcium hydroxide1
Brønsted base
Base
Hydroxide base

Products

Chemical formulaNameCoefficientTypeType in general
equation
K2SO4Potassium sulfate1
Conjugate base
Salt
CaSO4Calcium sulfate1
Conjugate base
Salt
H2OWater2
–
Conjugate acid
Water

Thermodynamic changes

Changes in standard condition (1)

Reaction of potassium hydrogensulfate and calcium hydroxide
◆
ΔrG−156.3 kJ/mol
K2.41 × 1027
pK−27.38
2KHSO4Crystalline solid + Ca(OH)2Crystalline solid
⟶
K2SO4Crystalline solid + CaSO4Crystalline solidinsoluble, anhydrite + 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
−136.3−156.362.5–
−68.15−78.1531.3–
per 1 mol of
−136.3−156.362.5–
per 1 mol of
−136.3−156.362.5–
per 1 mol of
−136.3−156.362.5–
per 1 mol of
−68.15−78.1531.3–

Changes in standard condition (2)

Reaction of potassium hydrogensulfate and calcium hydroxide
◆
ΔrG−148.0 kJ/mol
K8.48 × 1025
pK−25.93
2KHSO4Crystalline solid + Ca(OH)2Crystalline solid
⟶
K2SO4Crystalline solid + CaSO4Crystalline solidsoluble, α + 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
−127.4−148.064.2–
−63.70−74.0032.1–
per 1 mol of
−127.4−148.064.2–
per 1 mol of
−127.4−148.064.2–
per 1 mol of
−127.4−148.064.2–
per 1 mol of
−63.70−74.0032.1–

Changes in standard condition (3)

Reaction of potassium hydrogensulfate and calcium hydroxide
◆
ΔrG−143.5 kJ/mol
K1.38 × 1025
pK−25.14
2KHSO4Crystalline solid + Ca(OH)2Crystalline solid
⟶
K2SO4Crystalline solid + CaSO4Crystalline solidsoluble, β + 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
−123.0−143.564.2–
−61.50−71.7532.1–
per 1 mol of
−123.0−143.564.2–
per 1 mol of
−123.0−143.564.2–
per 1 mol of
−123.0−143.564.2–
per 1 mol of
−61.50−71.7532.1–

Changes in aqueous solution (1)

Reaction of potassium hydrogensulfate and calcium hydroxide
◆
ΔrG−130.27 kJ/mol
K6.64 × 1022
pK−22.82
2KHSO4Ionized aqueous solution + Ca(OH)2Crystalline solid
⟶
K2SO4Ionized aqueous solution + CaSO4Crystalline solidinsoluble, anhydrite + 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
−154.26−130.27−80.438
−77.130−65.135−40.219
per 1 mol of
−154.26−130.27−80.438
per 1 mol of
−154.26−130.27−80.438
per 1 mol of
−154.26−130.27−80.438
per 1 mol of
−77.130−65.135−40.219

Changes in aqueous solution (2)

Reaction of potassium hydrogensulfate and calcium hydroxide
◆
ΔrG−121.90 kJ/mol
K2.27 × 1021
pK−21.36
2KHSO4Ionized aqueous solution + Ca(OH)2Crystalline solid
⟶
K2SO4Ionized aqueous solution + CaSO4Crystalline solidsoluble, α + 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
−145.39−121.90−78.738
−72.695−60.950−39.419
per 1 mol of
−145.39−121.90−78.738
per 1 mol of
−145.39−121.90−78.738
per 1 mol of
−145.39−121.90−78.738
per 1 mol of
−72.695−60.950−39.419

Changes in aqueous solution (3)

Reaction of potassium hydrogensulfate and calcium hydroxide
◆
ΔrG−117.46 kJ/mol
K3.79 × 1020
pK−20.58
2KHSO4Ionized aqueous solution + Ca(OH)2Crystalline solid
⟶
K2SO4Ionized aqueous solution + CaSO4Crystalline solidsoluble, β + 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
−140.95−117.46−78.737
−70.475−58.730−39.419
per 1 mol of
−140.95−117.46−78.737
per 1 mol of
−140.95−117.46−78.737
per 1 mol of
−140.95−117.46−78.737
per 1 mol of
−70.475−58.730−39.419

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
KHSO4 (cr)-1160.6[1]-1031.3[1]138.1[1]–
KHSO4 (ai)-1139.72[1]-1039.18[1]234.3[1]-63[1]
Ca(OH)2 (cr)-986.09[1]-898.49[1]83.39[1]87.49[1]
Ca(OH)2 (g)-544[1]–––
Ca(OH)2 (ai)-1002.82[1]-868.07[1]-74.5[1]–
Ca(OH)2 (cr)
2 hydrate
-1218.4[1]–––
* (cr):Crystalline solid, (ai):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
K2SO4 (cr)-1437.79[1]-1321.37[1]175.56[1]131.46[1]
K2SO4 (g)-1096[1]-1033[1]364[1]108.8[1]
K2SO4 (ai)-1414.02[1]-1311.07[1]225.1[1]-251[1]
CaSO4 (cr)
insoluble, anhydrite
-1434.11[1]-1321.79[1]106.7[1]99.66[1]
CaSO4 (cr)
soluble, α
-1425.24[1]-1313.42[1]108.4[1]100.21[1]
CaSO4 (cr)
soluble, β
-1420.80[1]-1308.98[1]108.4[1]99.04[1]
CaSO4 (ai)-1452.10[1]-1298.10[1]-33.1[1]–
CaSO4 (cr)
0.5 hydrate
macrocrystalline, α
-1576.74[1]-1436.74[1]130.5[1]119.41[1]
CaSO4 (cr)
0.5 hydrate
microcrystalline, β
-1574.65[1]-1435.78[1]134.3[1]124.22[1]
CaSO4 (cr)
2 hydrate
selenite
-2022.63[1]-1797.28[1]194.1[1]186.02[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, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid

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)