3CH3COOK + H3AsO4 🔥→ K3AsO4 + 3CH3COOH
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The reaction of potassium acetate and arsenic acid yields potassium arsenate and acetic acid. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of potassium acetate and arsenic acid
General equation
- Salt of volatile acidBrønsted base + Nonvolatile acidBrønsted acid ⟶ Salt of non volatile acidConjugate base + Volatile acidConjugate acid
Oxidation state of each atom
- Reaction of potassium acetate and arsenic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CH3COOK | Potassium acetate | 3 | Brønsted base | Salt of volatile acid |
| H3AsO4 | Arsenic acid | 1 | Brønsted acid | Nonvolatile acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K3AsO4 | Potassium arsenate | 1 | Conjugate base | Salt of non volatile acid |
| CH3COOH | Acetic acid | 3 | Conjugate acid | Volatile acid |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium acetate and arsenic acid◆
ΔrG 36.1 kJ/mol K 0.47 × 10−6 pK 6.32
| 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 | 15.1 | 36.1 | −70 | – |
per 1 mol of | 5.03 | 12.0 | −23 | – |
per 1 mol of | 15.1 | 36.1 | −70 | – |
per 1 mol of | 15.1 | 36.1 | −70 | – |
per 1 mol of | 5.03 | 12.0 | −23 | – |
Changes in aqueous solution (2)
- Reaction of potassium acetate and arsenic acid
| 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 | 17.2 | – | – | – |
per 1 mol of | 5.73 | – | – | – |
per 1 mol of | 17.2 | – | – | – |
per 1 mol of | 17.2 | – | – | – |
per 1 mol of | 5.73 | – | – | – |
Changes in aqueous solution (3)
- Reaction of potassium acetate and arsenic acid◆
ΔrG 117.6 kJ/mol K 0.25 × 10−20 pK 20.60
| 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 | 14.4 | 117.6 | −347 | – |
per 1 mol of | 4.80 | 39.20 | −116 | – |
per 1 mol of | 14.4 | 117.6 | −347 | – |
per 1 mol of | 14.4 | 117.6 | −347 | – |
per 1 mol of | 4.80 | 39.20 | −116 | – |
Changes in aqueous solution (4)
- Reaction of potassium acetate and arsenic acid
| 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 | 16.5 | – | – | – |
per 1 mol of | 5.50 | – | – | – |
per 1 mol of | 16.5 | – | – | – |
per 1 mol of | 16.5 | – | – | – |
per 1 mol of | 5.50 | – | – | – |
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 |
|---|---|---|---|---|
| CH3COOK (cr) | -723.0[1] | – | – | – |
| CH3COOK (ai) | -738.39[1] | -652.58[1] | 189.1[1] | 15.5[1] |
| H3AsO4 (cr) | -906.3[1] | – | – | – |
| H3AsO4 (ao) | -902.5[1] | -766.0[1] | 184[1] | – |
| H3AsO4 (aq) | -904.6[1] | – | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (ao):Un-ionized aqueous solution, (aq):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 |
|---|---|---|---|---|
| K3AsO4 (ai) | -1645.27[1] | -1498.23[1] | 144.8[1] | – |
| CH3COOH (l) | -484.5[1] | -389.9[1] | 159.8[1] | 124.3[1] |
| CH3COOH (g) | -432.25[1] | -374.0[1] | 282.5[1] | 66.5[1] |
| CH3COOH (ai) | -486.01[1] | -369.31[1] | 86.6[1] | -6.3[1] |
| CH3COOH (ao) | -485.76[1] | -396.46[1] | 178.7[1] | – |
* (ai):Ionized aqueous solution, (l):Liquid, (g):Gas, (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°, -723.0 kJ · mol−1
- ^ ΔfH°, -738.39 kJ · mol−1
- ^ ΔfG°, -652.58 kJ · mol−1
- ^ S°, 189.1 J · K−1 · mol−1
- ^ Cp°, 15.5 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
- ^ ΔfH°, -1645.27 kJ · mol−1
- ^ ΔfG°, -1498.23 kJ · mol−1
- ^ S°, 144.8 J · K−1 · mol−1
- ^ ΔfH°, -484.5 kJ · mol−1
- ^ ΔfG°, -389.9 kJ · mol−1
- ^ S°, 159.8 J · K−1 · mol−1
- ^ Cp°, 124.3 J · K−1 · mol−1
- ^ ΔfH°, -432.25 kJ · mol−1
- ^ ΔfG°, -374.0 kJ · mol−1
- ^ S°, 282.5 J · K−1 · mol−1
- ^ Cp°, 66.5 J · K−1 · mol−1
- ^ ΔfH°, -486.01 kJ · mol−1
- ^ ΔfG°, -369.31 kJ · mol−1
- ^ S°, 86.6 J · K−1 · mol−1
- ^ Cp°, -6.3 J · K−1 · mol−1
- ^ ΔfH°, -485.76 kJ · mol−1
- ^ ΔfG°, -396.46 kJ · mol−1
- ^ S°, 178.7 J · K−1 · mol−1