BaS + NaHSO4 💧→ BaSO4↓ + NaHS
Last updated:
The reaction of barium sulfide and sodium hydrogensulfate yields barium sulfate and sodium hydrogensulfide. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of barium sulfide and sodium hydrogensulfate
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 barium sulfide and sodium hydrogensulfate
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaS | Barium sulfide | 1 | Lewis acid | Soluble in water |
| NaHSO4 | Sodium hydrogensulfate | 1 | Lewis base | Very soluble in water |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaSO4 | Barium sulfate | 1 | Lewis conjugate | Insoluble in water |
| NaHS | Sodium hydrogensulfide | 1 | Non-redox product | – |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of barium sulfide and sodium hydrogensulfate
| 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 | −125 | – | – | – |
per 1 mol of | −125 | – | – | – |
per 1 mol of | −125 | – | – | – |
per 1 mol of | −125 | – | – | – |
per 1 mol of | −125 | – | – | – |
Changes in standard condition (2)
- Reaction of barium sulfide and sodium hydrogensulfate
| 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 | −118 | – | – | – |
per 1 mol of | −118 | – | – | – |
per 1 mol of | −118 | – | – | – |
per 1 mol of | −118 | – | – | – |
per 1 mol of | −118 | – | – | – |
Changes in aqueous solution
- Reaction of barium sulfide and sodium hydrogensulfate
| 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 | 1218.3 | – | – | – |
per 1 mol of | 1218.3 | – | – | – |
per 1 mol of | 1218.3 | – | – | – |
per 1 mol of | 1218.3 | – | – | – |
per 1 mol of | 1218.3 | – | – | – |
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 |
|---|---|---|---|---|
| BaS (cr) | -460[1] | -456[1] | 78.2[1] | 49.37[1] |
| BaS (g) | 50[1] | – | – | – |
| BaS (aq) | -493.3[1] | – | – | – |
| NaHSO4 (cr) | -1125.5[1] | -992.8[1] | 113.0[1] | – |
| NaHSO4 (ai) | -1127.46[1] | -1017.80[1] | 190.8[1] | -38[1] |
| NaHSO4 (cr) 1 hydrate | -1421.7[1] | -1231.6[1] | 155[1] | – |
* (cr):Crystalline solid, (g):Gas, (aq):Aqueous solution, (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 |
|---|---|---|---|---|
| BaSO4 (cr) | -1473.2[1] | -1362.2[1] | 132.2[1] | 101.75[1] |
| BaSO4 (cr) precipitated | -1466.5[1] | – | – | – |
| BaSO4 (ai) | -144.691[1] | -1305.30[1] | 29.7[1] | – |
| NaHS (cr) | -237.23[1] | – | – | – |
| NaHS (ai) | -257.73[1] | -249.81[1] | 121.8[1] | – |
| NaHS (cr) 2 hydrate | -838.47[1] | – | – | – |
* (cr):Crystalline solid, (ai):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°, -460. kJ · mol−1
- ^ ΔfG°, -456. kJ · mol−1
- ^ S°, 78.2 J · K−1 · mol−1
- ^ Cp°, 49.37 J · K−1 · mol−1
- ^ ΔfH°, 50. kJ · mol−1
- ^ ΔfH°, -493.3 kJ · mol−1
- ^ ΔfH°, -1125.5 kJ · mol−1
- ^ ΔfG°, -992.8 kJ · mol−1
- ^ S°, 113.0 J · K−1 · mol−1
- ^ ΔfH°, -1127.46 kJ · mol−1
- ^ ΔfG°, -1017.80 kJ · mol−1
- ^ S°, 190.8 J · K−1 · mol−1
- ^ Cp°, -38. J · K−1 · mol−1
- ^ ΔfH°, -1421.7 kJ · mol−1
- ^ ΔfG°, -1231.6 kJ · mol−1
- ^ S°, 155. J · K−1 · mol−1
- ^ ΔfH°, -1473.2 kJ · mol−1
- ^ ΔfG°, -1362.2 kJ · mol−1
- ^ S°, 132.2 J · K−1 · mol−1
- ^ Cp°, 101.75 J · K−1 · mol−1
- ^ ΔfH°, -1466.5 kJ · mol−1
- ^ ΔfH°, -144.691 kJ · mol−1
- ^ ΔfG°, -1305.30 kJ · mol−1
- ^ S°, 29.7 J · K−1 · mol−1
- ^ ΔfH°, -237.23 kJ · mol−1
- ^ ΔfH°, -257.73 kJ · mol−1
- ^ ΔfG°, -249.81 kJ · mol−1
- ^ S°, 121.8 J · K−1 · mol−1
- ^ ΔfH°, -838.47 kJ · mol−1