Co(NO3)2 + 2KOH → 2KNO3 + Co(OH)2↓
Last updated:
The reaction of cobalt(II) nitrate and potassium hydroxide yields potassium nitrate and cobalt(II) hydroxide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of cobalt(II) nitrate and potassium hydroxide
General equation
- Reaction of salt of weak base and strong base
- Salt of weak baseBrønsted acid + Strong baseBrønsted base ⟶ Salt of strong baseConjugate acid + Weak baseConjugate base + (H2O)
- 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 cobalt(II) nitrate and potassium hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Co(NO3)2 | Cobalt(II) nitrate | 1 | Brønsted acid Lewis acid | Salt of weak base Very soluble in water |
| KOH | Potassium hydroxide | 2 | Brønsted base Lewis base | Strong base Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KNO3 | Potassium nitrate | 2 | Conjugate acid Non-redox product | Salt of strong base – |
| Co(OH)2 | Cobalt(II) hydroxide | 1 | Conjugate base Lewis conjugate | Weak base Insoluble in water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of cobalt(II) nitrate and potassium hydroxide
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (2)
- Reaction of cobalt(II) nitrate and potassium hydroxide
| 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 | −258.9 | – | – | – |
per 1 mol of | −258.9 | – | – | – |
per 1 mol of | −129.4 | – | – | – |
per 1 mol of | −129.4 | – | – | – |
per 1 mol of | −258.9 | – | – | – |
Changes in standard condition (3)
- Reaction of cobalt(II) nitrate and potassium hydroxide
| 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in aqueous solution (1)
- Reaction of cobalt(II) nitrate and potassium hydroxide◆
ΔrG −52.9 kJ/mol K 1.85 × 109 pK −9.27
| 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 | – | −52.9 | – | – |
per 1 mol of | – | −52.9 | – | – |
per 1 mol of | – | −26.4 | – | – |
per 1 mol of | – | −26.4 | – | – |
per 1 mol of | – | −52.9 | – | – |
Changes in aqueous solution (2)
- Reaction of cobalt(II) nitrate and potassium hydroxide◆
ΔrG −81.3 kJ/mol K 1.75 × 1014 pK −14.24
| 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 | – | −81.3 | – | – |
per 1 mol of | – | −81.3 | – | – |
per 1 mol of | – | −40.6 | – | – |
per 1 mol of | – | −40.6 | – | – |
per 1 mol of | – | −81.3 | – | – |
Changes in aqueous solution (3)
- Reaction of cobalt(II) nitrate and potassium hydroxide◆
ΔrG −85.5 kJ/mol K 9.53 × 1014 pK −14.98
| 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 | −21.6 | −85.5 | 214 | – |
per 1 mol of | −21.6 | −85.5 | 214 | – |
per 1 mol of | −10.8 | −42.8 | 107 | – |
per 1 mol of | −10.8 | −42.8 | 107 | – |
per 1 mol of | −21.6 | −85.5 | 214 | – |
Changes in aqueous solution (4)
- Reaction of cobalt(II) nitrate and potassium hydroxide◆
ΔrG −89.3 kJ/mol K 4.41 × 1015 pK −15.64
| 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 | – | −89.3 | – | – |
per 1 mol of | – | −89.3 | – | – |
per 1 mol of | – | −44.6 | – | – |
per 1 mol of | – | −44.6 | – | – |
per 1 mol of | – | −89.3 | – | – |
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 |
|---|---|---|---|---|
| Co(NO3)2 (cr) | -420.5[1] | – | – | – |
| Co(NO3)2 (ai) | -472.8[1] | -276.9[1] | 180[1] | – |
| Co(NO3)2 (cr) 2 hydrate | -1021.7[1] | – | – | – |
| Co(NO3)2 (cr) 3 hydrate | -1325.9[1] | – | – | – |
| Co(NO3)2 (cr) 4 hydrate | -1630.5[1] | – | – | – |
| Co(NO3)2 (cr) 6 hydrate | -2211.20[1] | – | – | 452[1] |
| KOH (cr) | -424.764[1] | -379.08[1] | 78.9[1] | 64.9[1] |
| KOH (g) | -231.0[1] | -232.6[1] | 238.3[1] | 49.20[1] |
| KOH (ai) | -482.37[1] | -440.50[1] | 91.6[1] | -126.8[1] |
| KOH (cr) 1 hydrate | -748.9[1] | -645.1[1] | 117.2[1] | – |
| KOH (cr) 2 hydrate | -1051.0[1] | -887.3[1] | 150.6[1] | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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 |
|---|---|---|---|---|
| KNO3 (cr) | -494.63[1] | -394.86[1] | 133.05[1] | 96.40[1] |
| KNO3 (ai) | -459.74[1] | -394.53[1] | 248.9[1] | -64.9[1] |
| Co(OH)2 (cr) blue, precipitated | – | -450.1[1] | – | – |
| Co(OH)2 (cr) pink, precipitated | -539.7[1] | -454.3[1] | 79[1] | – |
| Co(OH)2 (cr) pink, precipitated, aged | – | -458.1[1] | – | – |
| Co(OH)2 (ai) | -518.0[1] | -369.0[1] | -134[1] | – |
| Co(OH)2 (ao) | – | -421.7[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°, -420.5 kJ · mol−1
- ^ ΔfH°, -472.8 kJ · mol−1
- ^ ΔfG°, -276.9 kJ · mol−1
- ^ S°, 180. J · K−1 · mol−1
- ^ ΔfH°, -1021.7 kJ · mol−1
- ^ ΔfH°, -1325.9 kJ · mol−1
- ^ ΔfH°, -1630.5 kJ · mol−1
- ^ ΔfH°, -2211.20 kJ · mol−1
- ^ Cp°, 452. J · K−1 · mol−1
- ^ ΔfH°, -424.764 kJ · mol−1
- ^ ΔfG°, -379.08 kJ · mol−1
- ^ S°, 78.9 J · K−1 · mol−1
- ^ Cp°, 64.9 J · K−1 · mol−1
- ^ ΔfH°, -231.0 kJ · mol−1
- ^ ΔfG°, -232.6 kJ · mol−1
- ^ S°, 238.3 J · K−1 · mol−1
- ^ Cp°, 49.20 J · K−1 · mol−1
- ^ ΔfH°, -482.37 kJ · mol−1
- ^ ΔfG°, -440.50 kJ · mol−1
- ^ S°, 91.6 J · K−1 · mol−1
- ^ Cp°, -126.8 J · K−1 · mol−1
- ^ ΔfH°, -748.9 kJ · mol−1
- ^ ΔfG°, -645.1 kJ · mol−1
- ^ S°, 117.2 J · K−1 · mol−1
- ^ ΔfH°, -1051.0 kJ · mol−1
- ^ ΔfG°, -887.3 kJ · mol−1
- ^ S°, 150.6 J · K−1 · mol−1
- ^ ΔfH°, -494.63 kJ · mol−1
- ^ ΔfG°, -394.86 kJ · mol−1
- ^ S°, 133.05 J · K−1 · mol−1
- ^ Cp°, 96.40 J · K−1 · mol−1
- ^ ΔfH°, -459.74 kJ · mol−1
- ^ ΔfG°, -394.53 kJ · mol−1
- ^ S°, 248.9 J · K−1 · mol−1
- ^ Cp°, -64.9 J · K−1 · mol−1
- ^ ΔfG°, -450.1 kJ · mol−1
- ^ ΔfH°, -539.7 kJ · mol−1
- ^ ΔfG°, -454.3 kJ · mol−1
- ^ S°, 79. J · K−1 · mol−1
- ^ ΔfG°, -458.1 kJ · mol−1
- ^ ΔfH°, -518.0 kJ · mol−1
- ^ ΔfG°, -369.0 kJ · mol−1
- ^ S°, -134. J · K−1 · mol−1
- ^ ΔfG°, -421.7 kJ · mol−1