Ba(HCO3)2 + Zn(OH)2 → BaCO3 + ZnCO3 + 2H2O
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The reaction of barium hydrogencarbonate and zinc hydroxide yields barium carbonate, zinc carbonate, and water. This reaction is an acid-base reaction and is classified as follows:
Table of contents
Reaction data
Chemical equation
- Reaction of barium hydrogencarbonate and zinc 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 barium hydrogencarbonate and zinc hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ba(HCO3)2 | Barium hydrogencarbonate | 1 | Brønsted acid | Acid salt |
| Zn(OH)2 | Zinc hydroxide | 1 | Brønsted base | Base Hydroxide base |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| BaCO3 | Barium carbonate | 1 | Conjugate base | Salt |
| ZnCO3 | Zinc carbonate | 1 | Conjugate base | Salt |
| H2O | Water | 2 | – Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of barium hydrogencarbonate and zinc hydroxide◆
ΔrG −86.3 kJ/mol K 1.32 × 1015 pK −15.12
| 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 | – | −86.3 | – | – |
per 1 mol of | – | −86.3 | – | – |
per 1 mol of | – | −86.3 | – | – |
per 1 mol of | – | −86.3 | – | – |
per 1 mol of | – | −86.3 | – | – |
per 1 mol of | – | −43.1 | – | – |
Changes in standard condition (2)
- Reaction of barium hydrogencarbonate and zinc hydroxide◆
ΔrG −55.3 kJ/mol K 4.88 × 109 pK −9.69
| 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 | – | −55.3 | – | – |
per 1 mol of | – | −55.3 | – | – |
per 1 mol of | – | −55.3 | – | – |
per 1 mol of | – | −55.3 | – | – |
per 1 mol of | – | −55.3 | – | – |
per 1 mol of | – | −27.6 | – | – |
Changes in standard condition (3)
- Reaction of barium hydrogencarbonate and zinc hydroxide◆
ΔrG −55.6 kJ/mol K 5.50 × 109 pK −9.74
| 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 | −37.2 | −55.6 | 61.1 | – |
per 1 mol of | −37.2 | −55.6 | 61.1 | – |
per 1 mol of | −37.2 | −55.6 | 61.1 | – |
per 1 mol of | −37.2 | −55.6 | 61.1 | – |
per 1 mol of | −37.2 | −55.6 | 61.1 | – |
per 1 mol of | −18.6 | −27.8 | 30.6 | – |
Changes in standard condition (4)
- Reaction of barium hydrogencarbonate and zinc hydroxide◆
ΔrG −54.0 kJ/mol K 2.89 × 109 pK −9.46
| 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 | −35.9 | −54.0 | 60.7 | – |
per 1 mol of | −35.9 | −54.0 | 60.7 | – |
per 1 mol of | −35.9 | −54.0 | 60.7 | – |
per 1 mol of | −35.9 | −54.0 | 60.7 | – |
per 1 mol of | −35.9 | −54.0 | 60.7 | – |
per 1 mol of | −17.9 | −27.0 | 30.4 | – |
Changes in standard condition (5)
- Reaction of barium hydrogencarbonate and zinc hydroxide
| 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 | −36.9 | – | – | – |
per 1 mol of | −36.9 | – | – | – |
per 1 mol of | −36.9 | – | – | – |
per 1 mol of | −36.9 | – | – | – |
per 1 mol of | −36.9 | – | – | – |
per 1 mol of | −18.4 | – | – | – |
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 |
|---|---|---|---|---|
| Ba(HCO3)2 (ai) | -1921.63[1] | -1734.30[1] | 192.0[1] | – |
| Zn(OH)2 (cr) γ | – | -553.81[1] | – | – |
| Zn(OH)2 (cr) β | -641.91[1] | -553.52[1] | 81.2[1] | – |
| Zn(OH)2 (cr) ε | -643.25[1] | -555.07[1] | 81.6[1] | 72.4[1] |
| Zn(OH)2 (cr) precipitated | -642.2[1] | – | – | – |
| Zn(OH)2 (ai) | -613.88[1] | -461.56[1] | -133.5[1] | -251[1] |
| Zn(OH)2 (ao) | – | -522.73[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 |
|---|---|---|---|---|
| BaCO3 (cr) | -1216.3[1] | -1137.6[1] | 112.1[1] | 85.35[1] |
| BaCO3 (ai) | -1214.78[1] | -1088.59[1] | -47.3[1] | – |
| ZnCO3 (cr) | -812.78[1] | -731.52[1] | 82.4[1] | 79.71[1] |
| ZnCO3 (cr) 1 hydrate | – | -970.6[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)
- ^ ΔfH°, -1921.63 kJ · mol−1
- ^ ΔfG°, -1734.30 kJ · mol−1
- ^ S°, 192.0 J · K−1 · mol−1
- ^ ΔfG°, -553.81 kJ · mol−1
- ^ ΔfH°, -641.91 kJ · mol−1
- ^ ΔfG°, -553.52 kJ · mol−1
- ^ S°, 81.2 J · K−1 · mol−1
- ^ ΔfH°, -643.25 kJ · mol−1
- ^ ΔfG°, -555.07 kJ · mol−1
- ^ S°, 81.6 J · K−1 · mol−1
- ^ Cp°, 72.4 J · K−1 · mol−1
- ^ ΔfH°, -642.2 kJ · mol−1
- ^ ΔfH°, -613.88 kJ · mol−1
- ^ ΔfG°, -461.56 kJ · mol−1
- ^ S°, -133.5 J · K−1 · mol−1
- ^ Cp°, -251. J · K−1 · mol−1
- ^ ΔfG°, -522.73 kJ · mol−1
- ^ ΔfH°, -1216.3 kJ · mol−1
- ^ ΔfG°, -1137.6 kJ · mol−1
- ^ S°, 112.1 J · K−1 · mol−1
- ^ Cp°, 85.35 J · K−1 · mol−1
- ^ ΔfH°, -1214.78 kJ · mol−1
- ^ ΔfG°, -1088.59 kJ · mol−1
- ^ S°, -47.3 J · K−1 · mol−1
- ^ ΔfH°, -812.78 kJ · mol−1
- ^ ΔfG°, -731.52 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, 79.71 J · K−1 · mol−1
- ^ ΔfG°, -970.6 kJ · 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