Pb(HSO4)2 + Co(OH)2 → PbSO4 + CoSO4 + 2H2O
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The reaction of lead(II) hydrogensulfate and cobalt(II) hydroxide yields lead(II) sulfate, cobalt(II) sulfate, and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of lead(II) hydrogensulfate and cobalt(II) hydroxide
General equation
- Reaction of acid salt and base
- Acid saltBrønsted acid + BaseBrønsted base ⟶ SaltConjugate base + (H2O)
- Reaction of acid salt and hydroxide base
- Acid saltBrønsted acid + Hydroxide baseBrønsted base ⟶ SaltConjugate base + H2OConjugate acid
Oxidation state of each atom
- Reaction of lead(II) hydrogensulfate and cobalt(II) hydroxide
Reactants
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
Pb(HSO4)2 | Lead(II) hydrogensulfate | 1 | Brønsted acid | Acid salt |
Co(OH)2 | Cobalt(II) hydroxide | 1 | Brønsted base | Base Hydroxide base |
Products
Chemical formula | Name | Coefficient | Type | Type in general equation |
---|---|---|---|---|
PbSO4 | Lead(II) sulfate | 1 | Conjugate base | Salt |
CoSO4 | Cobalt(II) sulfate | 1 | Conjugate base | Salt |
H2O | Water | 2 | – Conjugate acid | Water |
Thermodynamic changes
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 |
---|---|---|---|---|
Pb(HSO4)2 | – | – | – | – |
Co(OH)2 (cr) blue, precipitated | – | -450.1[1] | – | – |
Co(OH)2 (cr) pink, precipitated | -539.7[1] | -454.3[1] | 79[1] | – |
Co(OH)2 (cr) pink, precipitated, aged | – | -458.1[1] | – | – |
Co(OH)2 (ai) | -518.0[1] | -369.0[1] | -134[1] | – |
Co(OH)2 (ao) | – | -421.7[1] | – | – |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (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 |
---|---|---|---|---|
PbSO4 (cr) | -919.94[1] | -813.14[1] | 148.57[1] | 103.207[1] |
CoSO4 (cr) | -888.3[1] | -782.3[1] | 118.0[1] | – |
CoSO4 (ai) | -967.3[1] | -799.1[1] | -92[1] | – |
CoSO4 (cr) 6 hydrate | -2683.6[1] | -2235.36[1] | 367.61[1] | 353.38[1] |
CoSO4 (cr) 7 hydrate | -2979.93[1] | -2473.42[1] | 406.06[1] | 390.49[1] |
H2O (cr) | – | – | – | – |
H2O (l) | -285.830[1] | -237.129[1] | 69.91[1] | 75.291[1] |
H2O (g) | -241.818[1] | -228.572[1] | 188.825[1] | 33.577[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (l):Liquid, (g):Gas
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)
- ^ ΔfG°, -450.1 kJ · mol−1
- ^ ΔfH°, -539.7 kJ · mol−1
- ^ ΔfG°, -454.3 kJ · mol−1
- ^ S°, 79. J · K−1 · mol−1
- ^ ΔfG°, -458.1 kJ · mol−1
- ^ ΔfH°, -518.0 kJ · mol−1
- ^ ΔfG°, -369.0 kJ · mol−1
- ^ S°, -134. J · K−1 · mol−1
- ^ ΔfG°, -421.7 kJ · mol−1
- ^ ΔfH°, -919.94 kJ · mol−1
- ^ ΔfG°, -813.14 kJ · mol−1
- ^ S°, 148.57 J · K−1 · mol−1
- ^ Cp°, 103.207 J · K−1 · mol−1
- ^ ΔfH°, -888.3 kJ · mol−1
- ^ ΔfG°, -782.3 kJ · mol−1
- ^ S°, 118.0 J · K−1 · mol−1
- ^ ΔfH°, -967.3 kJ · mol−1
- ^ ΔfG°, -799.1 kJ · mol−1
- ^ S°, -92. J · K−1 · mol−1
- ^ ΔfH°, -2683.6 kJ · mol−1
- ^ ΔfG°, -2235.36 kJ · mol−1
- ^ S°, 367.61 J · K−1 · mol−1
- ^ Cp°, 353.38 J · K−1 · mol−1
- ^ ΔfH°, -2979.93 kJ · mol−1
- ^ ΔfG°, -2473.42 kJ · mol−1
- ^ S°, 406.06 J · K−1 · mol−1
- ^ Cp°, 390.49 J · K−1 · mol−1
- ^ ΔfH°, -285.830 kJ · mol−1
- ^ ΔfG°, -237.129 kJ · mol−1
- ^ S°, 69.91 J · K−1 · mol−1
- ^ Cp°, 75.291 J · K−1 · mol−1
- ^ ΔfH°, -241.818 kJ · mol−1
- ^ ΔfG°, -228.572 kJ · mol−1
- ^ S°, 188.825 J · K−1 · mol−1
- ^ Cp°, 33.577 J · K−1 · mol−1