Ca3(AsO4)2 + 3H2SeO4 → 3CaSeO4 + 2H3AsO4
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The reaction of calcium arsenate and selenic acid yields calcium selenate and arsenic 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 arsenate and selenic acid
General equation
- Salt of weak acidBrønsted base + Strong acidBrønsted acid ⟶ Salt of strong acidConjugate base + Weak acidConjugate acid
Oxidation state of each atom
- Reaction of calcium arsenate and selenic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ca3(AsO4)2 | Calcium arsenate | 1 | Brønsted base | Salt of weak acid |
| H2SeO4 | Selenic acid | 3 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaSeO4 | Calcium selenate | 3 | Conjugate base | Salt of strong acid |
| H3AsO4 | Arsenic acid | 2 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of calcium arsenate and selenic acid
- Ca3(AsO4)2Crystalline solid + 3H2SeO4Crystalline solid3CaSeO4Crystalline solid + 2H3AsO4Un-ionized 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 | −245.4 | – | – | – |
per 1 mol of | −245.4 | – | – | – |
per 1 mol of | −81.80 | – | – | – |
per 1 mol of | −81.80 | – | – | – |
per 1 mol of | −122.7 | – | – | – |
Changes in aqueous solution (2)
- Reaction of calcium arsenate and selenic acid
- Ca3(AsO4)2Crystalline solid + 3H2SeO4Crystalline solid3CaSeO4Crystalline solid + 2H3AsO4Aqueous 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 | −249.6 | – | – | – |
per 1 mol of | −249.6 | – | – | – |
per 1 mol of | −83.20 | – | – | – |
per 1 mol of | −83.20 | – | – | – |
per 1 mol of | −124.8 | – | – | – |
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 |
|---|---|---|---|---|
| Ca3(AsO4)2 (cr) | -3298.7[1] | -3063.0[1] | 226[1] | – |
| Ca3(AsO4)2 (cr) hydrated precipitate | -3343[1] | – | – | – |
| H2SeO4 (cr) | -530.1[1] | – | – | – |
| H2SeO4 (cr) 1 hydrate | -840.6[1] | – | – | – |
| H2SeO4 (l) 1 hydrate | -820.5[1] | – | – | – |
* (cr):Crystalline solid, (l):Liquid
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 |
|---|---|---|---|---|
| CaSeO4 (cr) | -1109.81[1] | – | – | – |
| CaSeO4 (cr) 2 hydrate | -1706.7[1] | -1486.8[1] | 222[1] | – |
| H3AsO4 (cr) | -906.3[1] | – | – | – |
| H3AsO4 (ao) | -902.5[1] | -766.0[1] | 184[1] | – |
| H3AsO4 (aq) | -904.6[1] | – | – | – |
* (cr):Crystalline solid, (ao):Un-ionized aqueous solution, (aq):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°, -3298.7 kJ · mol−1
- ^ ΔfG°, -3063.0 kJ · mol−1
- ^ S°, 226. J · K−1 · mol−1
- ^ ΔfH°, -3343. kJ · mol−1
- ^ ΔfH°, -530.1 kJ · mol−1
- ^ ΔfH°, -840.6 kJ · mol−1
- ^ ΔfH°, -820.5 kJ · mol−1
- ^ ΔfH°, -1109.81 kJ · mol−1
- ^ ΔfH°, -1706.7 kJ · mol−1
- ^ ΔfG°, -1486.8 kJ · mol−1
- ^ S°, 222. J · K−1 · mol−1
- ^ ΔfH°, -906.3 kJ · mol−1
- ^ ΔfH°, -902.5 kJ · mol−1
- ^ ΔfG°, -766.0 kJ · mol−1
- ^ S°, 184. J · K−1 · mol−1
- ^ ΔfH°, -904.6 kJ · mol−1