Ca3(PO4)2 + 6HBr → 3CaBr2 + 2H3PO4
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The reaction of calcium phosphate and hydrogen bromide yields calcium bromide and phosphoric 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 calcium phosphate and hydrogen bromide
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 calcium phosphate and hydrogen bromide
Reactants
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| Ca3(PO4)2 | Calcium phosphate | 1 | Brønsted base | Salt of weak acid |
| HBr | Hydrogen bromide | 6 | Brønsted acid | Strong acid |
Products
| Chemical formula | Name | Coefficient | Type | Type in general equation |
|---|---|---|---|---|
| CaBr2 | Calcium bromide | 3 | Conjugate base | Salt of strong acid |
| H3PO4 | Phosphoric acid | 2 | Conjugate acid | Weak acid |
Thermodynamic changes
Changes in standard condition (1)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG −23.6 kJ/mol K 1.36 × 104 pK −4.13
| 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 | −267.2 | −23.6 | −817 | – |
per 1 mol of | −267.2 | −23.6 | −817 | – |
per 1 mol of | −44.53 | −3.93 | −136 | – |
per 1 mol of | −89.07 | −7.87 | −272 | – |
per 1 mol of | −133.6 | −11.8 | −409 | – |
Changes in standard condition (2)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG −32.8 kJ/mol K 5.58 × 105 pK −5.75
| 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 | −278.1 | −32.8 | −822 | – |
per 1 mol of | −278.1 | −32.8 | −822 | – |
per 1 mol of | −46.35 | −5.47 | −137 | – |
per 1 mol of | −92.70 | −10.9 | −274 | – |
per 1 mol of | −139.1 | −16.4 | −411 | – |
Changes in aqueous solution (1)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG −61.1 kJ/mol K 5.06 × 1010 pK −10.70
| 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 | −84.3 | −61.1 | −78.9 | – |
per 1 mol of | −84.3 | −61.1 | −78.9 | – |
per 1 mol of | −14.0 | −10.2 | −13.2 | – |
per 1 mol of | −28.1 | −20.4 | −26.3 | – |
per 1 mol of | −42.1 | −30.6 | −39.5 | – |
Changes in aqueous solution (2)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG −61.1 kJ/mol K 5.06 × 1010 pK −10.70
| 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 | −84.3 | −61.1 | −78.9 | – |
per 1 mol of | −84.3 | −61.1 | −78.9 | – |
per 1 mol of | −14.0 | −10.2 | −13.2 | – |
per 1 mol of | −28.1 | −20.4 | −26.3 | – |
per 1 mol of | −42.1 | −30.6 | −39.5 | – |
Changes in aqueous solution (3)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG −70.3 kJ/mol K 2.07 × 1012 pK −12.32
| 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 | −95.2 | −70.3 | −83.8 | – |
per 1 mol of | −95.2 | −70.3 | −83.8 | – |
per 1 mol of | −15.9 | −11.7 | −14.0 | – |
per 1 mol of | −31.7 | −23.4 | −27.9 | – |
per 1 mol of | −47.6 | −35.1 | −41.9 | – |
Changes in aqueous solution (4)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG −70.3 kJ/mol K 2.07 × 1012 pK −12.32
| 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 | −95.2 | −70.3 | −83.8 | – |
per 1 mol of | −95.2 | −70.3 | −83.8 | – |
per 1 mol of | −15.9 | −11.7 | −14.0 | – |
per 1 mol of | −31.7 | −23.4 | −27.9 | – |
per 1 mol of | −47.6 | −35.1 | −41.9 | – |
Changes in aqueous solution (5)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG 186.6 kJ/mol K 0.20 × 10−32 pK 32.69
| 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 | −62.5 | 186.6 | −835.9 | – |
per 1 mol of | −62.5 | 186.6 | −835.9 | – |
per 1 mol of | −10.4 | 31.10 | −139.3 | – |
per 1 mol of | −20.8 | 62.20 | −278.6 | – |
per 1 mol of | −31.3 | 93.30 | −417.9 | – |
Changes in aqueous solution (6)
- Reaction of calcium phosphate and hydrogen bromide◆
ΔrG 177.4 kJ/mol K 0.83 × 10−31 pK 31.08
| 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 | −73.4 | 177.4 | −840.8 | – |
per 1 mol of | −73.4 | 177.4 | −840.8 | – |
per 1 mol of | −12.2 | 29.57 | −140.1 | – |
per 1 mol of | −24.5 | 59.13 | −280.3 | – |
per 1 mol of | −36.7 | 88.70 | −420.4 | – |
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 |
|---|---|---|---|---|
| Ca3(PO4)2 (cr) β, low temp. form | -4120.8[1] | -3884.7[1] | 236.0[1] | 227.82[1] |
| Ca3(PO4)2 (cr) α, high temp. form | -4109.9[1] | -3875.5[1] | 240.91[1] | 231.58[1] |
| Ca3(PO4)2 (ai) | -4183.2[1] | -3698.1[1] | -599.9[1] | – |
| HBr (g) | -36.40[1] | -53.45[1] | 198.695[1] | 29.142[1] |
| HBr (ai) | -121.55[1] | -103.96[1] | 82.4[1] | -141.8[1] |
* (cr):Crystalline solid, (ai):Ionized aqueous solution, (g):Gas
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 |
|---|---|---|---|---|
| CaBr2 (cr) | -682.8[1] | -663.6[1] | 130[1] | – |
| CaBr2 (g) | -398.3[1] | – | – | – |
| CaBr2 (ai) | -785.92[1] | -761.49[1] | 111.7[1] | – |
| CaBr2 (cr) 6 hydrate | -2506.2[1] | -2152.8[1] | 410[1] | – |
| H3PO4 (cr) | -1279.0[1] | -1119.1[1] | 110.50[1] | 106.06[1] |
| H3PO4 (l) | -1266.9[1] | – | – | – |
| H3PO4 (ai) | -1277.4[1] | -1018.7[1] | -220.3[1] | – |
| H3PO4 (ao) | -1288.34[1] | -1142.54[1] | 158.2[1] | – |
| H3PO4 (cr) 0.5 hydrate | -1431.3[1] | -1242.1[1] | 129.16[1] | 126.02[1] |
| H3PO4 (cr) 1 hydrate | -1568.83[1] | – | – | – |
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution, (l):Liquid, (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°, -4120.8 kJ · mol−1
- ^ ΔfG°, -3884.7 kJ · mol−1
- ^ S°, 236.0 J · K−1 · mol−1
- ^ Cp°, 227.82 J · K−1 · mol−1
- ^ ΔfH°, -4109.9 kJ · mol−1
- ^ ΔfG°, -3875.5 kJ · mol−1
- ^ S°, 240.91 J · K−1 · mol−1
- ^ Cp°, 231.58 J · K−1 · mol−1
- ^ ΔfH°, -4183.2 kJ · mol−1
- ^ ΔfG°, -3698.1 kJ · mol−1
- ^ S°, -599.9 J · K−1 · mol−1
- ^ ΔfH°, -36.40 kJ · mol−1
- ^ ΔfG°, -53.45 kJ · mol−1
- ^ S°, 198.695 J · K−1 · mol−1
- ^ Cp°, 29.142 J · K−1 · mol−1
- ^ ΔfH°, -121.55 kJ · mol−1
- ^ ΔfG°, -103.96 kJ · mol−1
- ^ S°, 82.4 J · K−1 · mol−1
- ^ Cp°, -141.8 J · K−1 · mol−1
- ^ ΔfH°, -682.8 kJ · mol−1
- ^ ΔfG°, -663.6 kJ · mol−1
- ^ S°, 130. J · K−1 · mol−1
- ^ ΔfH°, -398.3 kJ · mol−1
- ^ ΔfH°, -785.92 kJ · mol−1
- ^ ΔfG°, -761.49 kJ · mol−1
- ^ S°, 111.7 J · K−1 · mol−1
- ^ ΔfH°, -2506.2 kJ · mol−1
- ^ ΔfG°, -2152.8 kJ · mol−1
- ^ S°, 410. J · K−1 · mol−1
- ^ ΔfH°, -1279.0 kJ · mol−1
- ^ ΔfG°, -1119.1 kJ · mol−1
- ^ S°, 110.50 J · K−1 · mol−1
- ^ Cp°, 106.06 J · K−1 · mol−1
- ^ ΔfH°, -1266.9 kJ · mol−1
- ^ ΔfH°, -1277.4 kJ · mol−1
- ^ ΔfG°, -1018.7 kJ · mol−1
- ^ S°, -220.3 J · K−1 · mol−1
- ^ ΔfH°, -1288.34 kJ · mol−1
- ^ ΔfG°, -1142.54 kJ · mol−1
- ^ S°, 158.2 J · K−1 · mol−1
- ^ ΔfH°, -1431.3 kJ · mol−1
- ^ ΔfG°, -1242.1 kJ · mol−1
- ^ S°, 129.16 J · K−1 · mol−1
- ^ Cp°, 126.02 J · K−1 · mol−1
- ^ ΔfH°, -1568.83 kJ · mol−1