NaIO3 → Na+ + IO3−
Last updated:
- Electrolytic dissociation of sodium iodate
Electrolytic dissociation of sodium iodate yields sodium ion and iodate ion. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Electrolytic dissociation of sodium iodate
General equation
- Electrolytic dissociation of salt
- SaltLewis conjugate ⟶ CationLewis acid + AnionLewis base
Oxidation state of each atom
- Electrolytic dissociation of sodium iodate
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
NaIO3 | Sodium iodate | 1 | Lewis conjugate | Salt |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Na+ | Sodium ion | 1 | Lewis acid | Cation |
IO3− | Iodate ion | 1 | Lewis base | Anion |
Thermodynamic changes
Changes in standard condition
- Electrolytic dissociation of sodium iodate
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 | 20.4 | – | – | – |
per 1 mol of | 20.4 | – | – | – |
per 1 mol of Sodium ion | 20.4 | – | – | – |
per 1 mol of Iodate ion | 20.4 | – | – | – |
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 |
---|---|---|---|---|
NaIO3 (cr) | -481.788[1] | – | – | 92.0[1] |
NaIO3 (ai) | -461.5[1] | -389.9[1] | 177.4[1] | – |
NaIO3 (cr) 1 hydrate | -779.48[1] | -634.03[1] | 162.3[1] | – |
NaIO3 (cr) 5 hydrate | -1952.25[1] | – | – | – |
* (cr):Crystalline solid, (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 |
---|---|---|---|---|
Na+ (g) | 609.358[1] | – | – | – |
Na+ (ao) | -240.12[1] | -261.905[1] | 59.0[1] | 46.4[1] |
IO3− (ao) | -221.3[1] | -128.0[1] | 118.4[1] | – |
* (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°, -481.788 kJ · mol−1
- ^ Cp°, 92.0 J · K−1 · mol−1
- ^ ΔfH°, -461.5 kJ · mol−1
- ^ ΔfG°, -389.9 kJ · mol−1
- ^ S°, 177.4 J · K−1 · mol−1
- ^ ΔfH°, -779.48 kJ · mol−1
- ^ ΔfG°, -634.03 kJ · mol−1
- ^ S°, 162.3 J · K−1 · mol−1
- ^ ΔfH°, -1952.25 kJ · mol−1
- ^ ΔfH°, 609.358 kJ · mol−1
- ^ ΔfH°, -240.12 kJ · mol−1
- ^ ΔfG°, -261.905 kJ · mol−1
- ^ S°, 59.0 J · K−1 · mol−1
- ^ Cp°, 46.4 J · K−1 · mol−1
- ^ ΔfH°, -221.3 kJ · mol−1
- ^ ΔfG°, -128.0 kJ · mol−1
- ^ S°, 118.4 J · K−1 · mol−1