2HNO3 + Zn(OH)2 → Zn(NO3)2 + 2H2O
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- Reaction of nitric acid and zinc hydroxide
The reaction of nitric acid and zinc hydroxide yields zinc nitrate and water. This reaction is an acid-base reaction and is classified as follows:
- Reaction of acid and base
- Reaction of acid and hydroxide base
- Reaction of strong acid and weak base
- Reaction of acid and amphoteric hydroxide
- Reaction of strong acid and amphoteric hydroxide
Table of contents
Reaction data
Chemical equation
- Reaction of nitric acid and zinc hydroxide
General equation
- Reaction of acid and base
- AcidBrønsted acid + BaseBrønsted base ⟶ SaltConjugate base + (H2O)(Conjugate acid)
- Reaction of acid and hydroxide base
- AcidBrønsted acid + Hydroxide baseBrønsted base ⟶ SaltConjugate base + H2OConjugate acid
- Reaction of strong acid and weak base
- Strong acidBrønsted acid + Weak baseBrønsted base ⟶ Salt of strong acid and weak baseConjugate base + (H2O)(Conjugate acid)
- Reaction of acid and amphoteric hydroxide
- AcidBrønsted acid + Amphoteric hydroxideBrønsted base ⟶ Salt of weak baseConjugate base + H2OConjugate acid
- Reaction of strong acid and amphoteric hydroxide
- Strong acidBrønsted acid + Amphoteric hydroxideBrønsted base ⟶ Salt of strong acid and weak baseConjugate base + H2OConjugate acid
Oxidation state of each atom
- Reaction of nitric acid and zinc hydroxide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| HNO3 | Nitric acid | 2 | Brønsted acid | Acid Strong acid |
| Zn(OH)2 | Zinc hydroxide | 1 | Brønsted base | Base Hydroxide base Weak base Amphoteric hydroxide |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Zn(NO3)2 | Zinc nitrate | 1 | Conjugate base | Salt Salt of strong acid and weak base Salt of weak base |
| H2O | Water | 2 | Conjugate acid | Water |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of nitric acid 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 | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
per 1 mol of | – | – | – | – |
Changes in standard condition (2)
- Reaction of nitric acid 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 | −65.3 | – | – | – |
per 1 mol of | −32.6 | – | – | – |
per 1 mol of | −65.3 | – | – | – |
per 1 mol of | −65.3 | – | – | – |
per 1 mol of | −32.6 | – | – | – |
Changes in standard condition (3)
- Reaction of nitric acid 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 | −63.9 | – | – | – |
per 1 mol of | −31.9 | – | – | – |
per 1 mol of | −63.9 | – | – | – |
per 1 mol of | −63.9 | – | – | – |
per 1 mol of | −31.9 | – | – | – |
Changes in standard condition (4)
- Reaction of nitric acid 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 | −65.0 | – | – | – |
per 1 mol of | −32.5 | – | – | – |
per 1 mol of | −65.0 | – | – | – |
per 1 mol of | −65.0 | – | – | – |
per 1 mol of | −32.5 | – | – | – |
Changes in aqueous solution (1)
- Reaction of nitric acid and zinc hydroxide◆
ΔrG −98.60 kJ/mol K 1.88 × 1017 pK −17.27
| 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 | – | −98.60 | – | – |
per 1 mol of | – | −49.30 | – | – |
per 1 mol of | – | −98.60 | – | – |
per 1 mol of | – | −98.60 | – | – |
per 1 mol of | – | −49.30 | – | – |
Changes in aqueous solution (2)
- Reaction of nitric acid and zinc hydroxide◆
ΔrG −67.52 kJ/mol K 6.75 × 1011 pK −11.83
| 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 | – | −67.52 | – | – |
per 1 mol of | – | −33.76 | – | – |
per 1 mol of | – | −67.52 | – | – |
per 1 mol of | – | −67.52 | – | – |
per 1 mol of | – | −33.76 | – | – |
Changes in aqueous solution (3)
- Reaction of nitric acid and zinc hydroxide◆
ΔrG −67.81 kJ/mol K 7.58 × 1011 pK −11.88
| 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 | −83.64 | −67.81 | −53.5 | – |
per 1 mol of | −41.82 | −33.91 | −26.8 | – |
per 1 mol of | −83.64 | −67.81 | −53.5 | – |
per 1 mol of | −83.64 | −67.81 | −53.5 | – |
per 1 mol of | −41.82 | −33.91 | −26.8 | – |
Changes in aqueous solution (4)
- Reaction of nitric acid and zinc hydroxide◆
ΔrG −66.26 kJ/mol K 4.06 × 1011 pK −11.61
| 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 | −82.30 | −66.26 | −53.9 | 125 |
per 1 mol of | −41.15 | −33.13 | −26.9 | 62.5 |
per 1 mol of | −82.30 | −66.26 | −53.9 | 125 |
per 1 mol of | −82.30 | −66.26 | −53.9 | 125 |
per 1 mol of | −41.15 | −33.13 | −26.9 | 62.5 |
Changes in aqueous solution (5)
- Reaction of nitric acid 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 | −83.3 | – | – | – |
per 1 mol of | −41.6 | – | – | – |
per 1 mol of | −83.3 | – | – | – |
per 1 mol of | −83.3 | – | – | – |
per 1 mol of | −41.6 | – | – | – |
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 |
|---|---|---|---|---|
| HNO3 (l) | -174.10[1] | -80.71[1] | 155.60[1] | 109.87[1] |
| HNO3 (g) | -135.06[1] | -74.72[1] | 266.38[1] | 53.35[1] |
| HNO3 (ai) | -207.36[1] | -111.25[1] | 146.4[1] | -86.6[1] |
| HNO3 (l) 1 hydrate | -473.46[1] | -328.77[1] | 216.90[1] | 182.46[1] |
| HNO3 (l) 3 hydrate | -1056.04[1] | -811.09[1] | 346.98[1] | 325.14[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] | – | – |
* (l):Liquid, (g):Gas, (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 |
|---|---|---|---|---|
| Zn(NO3)2 (cr) | -483.7[1] | – | – | – |
| Zn(NO3)2 (ai) | -568.61[1] | -369.57[1] | 180.7[1] | -126[1] |
| Zn(NO3)2 (cr) 1 hydrate | -805.0[1] | – | – | – |
| Zn(NO3)2 (cr) 2 hydrate | -1110.27[1] | – | – | – |
| Zn(NO3)2 (cr) 4 hydrate | -1699.12[1] | – | – | – |
| Zn(NO3)2 (cr) 6 hydrate | -2306.64[1] | -1772.71[1] | 456.9[1] | 323.0[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°, -174.10 kJ · mol−1
- ^ ΔfG°, -80.71 kJ · mol−1
- ^ S°, 155.60 J · K−1 · mol−1
- ^ Cp°, 109.87 J · K−1 · mol−1
- ^ ΔfH°, -135.06 kJ · mol−1
- ^ ΔfG°, -74.72 kJ · mol−1
- ^ S°, 266.38 J · K−1 · mol−1
- ^ Cp°, 53.35 J · K−1 · mol−1
- ^ ΔfH°, -207.36 kJ · mol−1
- ^ ΔfG°, -111.25 kJ · mol−1
- ^ S°, 146.4 J · K−1 · mol−1
- ^ Cp°, -86.6 J · K−1 · mol−1
- ^ ΔfH°, -473.46 kJ · mol−1
- ^ ΔfG°, -328.77 kJ · mol−1
- ^ S°, 216.90 J · K−1 · mol−1
- ^ Cp°, 182.46 J · K−1 · mol−1
- ^ ΔfH°, -1056.04 kJ · mol−1
- ^ ΔfG°, -811.09 kJ · mol−1
- ^ S°, 346.98 J · K−1 · mol−1
- ^ Cp°, 325.14 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°, -483.7 kJ · mol−1
- ^ ΔfH°, -568.61 kJ · mol−1
- ^ ΔfG°, -369.57 kJ · mol−1
- ^ S°, 180.7 J · K−1 · mol−1
- ^ Cp°, -126. J · K−1 · mol−1
- ^ ΔfH°, -805.0 kJ · mol−1
- ^ ΔfH°, -1110.27 kJ · mol−1
- ^ ΔfH°, -1699.12 kJ · mol−1
- ^ ΔfH°, -2306.64 kJ · mol−1
- ^ ΔfG°, -1772.71 kJ · mol−1
- ^ S°, 456.9 J · K−1 · mol−1
- ^ Cp°, 323.0 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