K3AsO4 + 3HIO3 → 3KIO3 + H3AsO4
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- Reaction of potassium arsenate and iodic acid
The reaction of potassium arsenate and iodic acid yields potassium iodate 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 potassium arsenate and iodic 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 potassium arsenate and iodic acid
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| K3AsO4 | Potassium arsenate | 1 | Brønsted base | Salt of weak acid |
| HIO3 | Iodic acid | 3 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| KIO3 | Potassium iodate | 3 | Conjugate base | Salt of strong acid |
| H3AsO4 | Arsenic acid | 1 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in aqueous solution (1)
- Reaction of potassium arsenate and iodic acid◆
ΔrG −103.6 kJ/mol K 1.41 × 1018 pK −18.15
| 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 | −44.1 | −103.6 | 201 | – |
per 1 mol of | −44.1 | −103.6 | 201 | – |
per 1 mol of | −14.7 | −34.53 | 67.0 | – |
per 1 mol of | −14.7 | −34.53 | 67.0 | – |
per 1 mol of | −44.1 | −103.6 | 201 | – |
Changes in aqueous solution (2)
- Reaction of potassium arsenate and iodic 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 | −46.2 | – | – | – |
per 1 mol of | −46.2 | – | – | – |
per 1 mol of | −15.4 | – | – | – |
per 1 mol of | −15.4 | – | – | – |
per 1 mol of | −46.2 | – | – | – |
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 |
|---|---|---|---|---|
| K3AsO4 (ai) | -1645.27[1] | -1498.23[1] | 144.8[1] | – |
| HIO3 (cr) | -230.1[1] | – | – | – |
| HIO3 (ao) | -211.3[1] | -132.6[1] | 166.9[1] | – |
* (ai):Ionized aqueous solution, (cr):Crystalline solid, (ao):Un-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 |
|---|---|---|---|---|
| KIO3 (cr) | -501.37[1] | -418.35[1] | 151.46[1] | 106.48[1] |
| KIO3 (ai) | -473.6[1] | -411.2[1] | 220.9[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
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°, -1645.27 kJ · mol−1
- ^ ΔfG°, -1498.23 kJ · mol−1
- ^ S°, 144.8 J · K−1 · mol−1
- ^ ΔfH°, -230.1 kJ · mol−1
- ^ ΔfH°, -211.3 kJ · mol−1
- ^ ΔfG°, -132.6 kJ · mol−1
- ^ S°, 166.9 J · K−1 · mol−1
- ^ ΔfH°, -501.37 kJ · mol−1
- ^ ΔfG°, -418.35 kJ · mol−1
- ^ S°, 151.46 J · K−1 · mol−1
- ^ Cp°, 106.48 J · K−1 · mol−1
- ^ ΔfH°, -473.6 kJ · mol−1
- ^ ΔfG°, -411.2 kJ · mol−1
- ^ S°, 220.9 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