Ca(ClO)2 + 2KHCO3 💧→ CaCO3↓ + 2KClO + H2CO3
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The reaction of calcium hypochlorite and potassium hydrogencarbonate yields calcium carbonate, potassium hypochlorite, and carbonic acid (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of calcium hypochlorite and potassium hydrogencarbonate
General equation
- Precipitation reaction
- Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base💧⟶ Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)
Oxidation state of each atom
- Reaction of calcium hypochlorite and potassium hydrogencarbonate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ca(ClO)2 | Calcium hypochlorite | 1 | Lewis acid | Soluble in water |
| KHCO3 | Potassium hydrogencarbonate | 2 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaCO3 | Calcium carbonate | 1 | Lewis conjugate | Insoluble in water |
| KClO | Potassium hypochlorite | 2 | Non-redox product | – |
| H2CO3 | Carbonic acid | 1 | Non-redox product | – |
Thermodynamic changes
Changes in aqueous solution
- Reaction of calcium hypochlorite and potassium hydrogencarbonate
| 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 | 17.6 | – | – | – |
per 1 mol of | 17.6 | – | – | – |
per 1 mol of | 8.80 | – | – | – |
per 1 mol of | 17.6 | – | – | – |
per 1 mol of | 8.80 | – | – | – |
per 1 mol of | 17.6 | – | – | – |
Thermodynamic data of reactants
| Chemical formula | Standard 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 |
|---|---|---|---|---|
| Ca(ClO)2 (aq) | -754.4[1] | – | – | – |
| KHCO3 (cr) | -963.2[1] | -863.5[1] | 115.5[1] | – |
| KHCO3 (ai) | -944.37[1] | -870.04[1] | 193.7[1] | – |
* (aq):Aqueous solution, (cr):Crystalline solid, (ai):Ionized aqueous solution
Thermodynamic data of products
| Chemical formula | Standard 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 |
|---|---|---|---|---|
| CaCO3 (cr) | -1207.13[1] | -1127.75[1] | 88.7[1] | 81.25[1] |
| CaCO3 (ai) | -1219.97[1] | -1081.39[1] | -110.0[1] | – |
| KClO (ai) | -359.4[1] | -320.0[1] | 146[1] | – |
| H2CO3 (ao) | -699.65[1] | -623.08[1] | 187.4[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution
References
List of references
- 1Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -754.4 kJ · mol−1
- ^ ΔfH°, -963.2 kJ · mol−1
- ^ ΔfG°, -863.5 kJ · mol−1
- ^ S°, 115.5 J · K−1 · mol−1
- ^ ΔfH°, -944.37 kJ · mol−1
- ^ ΔfG°, -870.04 kJ · mol−1
- ^ S°, 193.7 J · K−1 · mol−1
- ^ ΔfH°, -1207.13 kJ · mol−1
- ^ ΔfG°, -1127.75 kJ · mol−1
- ^ S°, 88.7 J · K−1 · mol−1
- ^ Cp°, 81.25 J · K−1 · mol−1
- ^ ΔfH°, -1219.97 kJ · mol−1
- ^ ΔfG°, -1081.39 kJ · mol−1
- ^ S°, -110.0 J · K−1 · mol−1
- ^ ΔfH°, -359.4 kJ · mol−1
- ^ ΔfG°, -320.0 kJ · mol−1
- ^ S°, 146. J · K−1 · mol−1
- ^ ΔfH°, -699.65 kJ · mol−1
- ^ ΔfG°, -623.08 kJ · mol−1
- ^ S°, 187.4 J · K−1 · mol−1