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  3. 3BaBr2 + 6NaH2PO4 💧→ Ba3(PO4)2↓ + 6NaBr + 4H3PO4

3BaBr2 + 6NaH2PO4 💧→ Ba3(PO4)2↓ + 6NaBr + 4H3PO4

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Reaction of barium bromide and sodium dihydrogenphosphate
3BaBr2Barium bromide + 6NaH2PO4Sodium dihydrogenphosphate
💧
⟶
Ba3(PO4)2↓Barium phosphate + 6NaBrSodium bromide + 4H3PO4Phosphoric acid

The reaction of barium bromide and sodium dihydrogenphosphate yields barium phosphate, sodium bromide, and phosphoric acid. This reaction is an acid-base reaction and is classified as follows:

Table of contents
  1. 1Reaction data
  2. 2Thermodynamic changes
  3. 3References
  4. 4Related categories

Reaction data

Chemical equation

Reaction of barium bromide and sodium dihydrogenphosphate
3BaBr2Barium bromide + 6NaH2PO4Sodium dihydrogenphosphate
💧
⟶
Ba3(PO4)2↓Barium phosphate + 6NaBrSodium bromide + 4H3PO4Phosphoric acid

General equation

Precipitation reaction
Miscible with water/Very soluble in water/Soluble in waterLewis acid + Miscible with water/Very soluble in water/Soluble in waterLewis base
💧
⟶
Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of barium bromide and sodium dihydrogenphosphate

Reactants

Chemical formulaNameCoefficientTypeType in general
equation
BaBr2Barium bromide3
Lewis acid
Very soluble in water
NaH2PO4Sodium dihydrogenphosphate6
Lewis base
Very soluble in water

Products

Chemical formulaNameCoefficientTypeType in general
equation
Ba3(PO4)2Barium phosphate1
Lewis conjugate
Insoluble in water
NaBrSodium bromide6
Non-redox product
–
H3PO4Phosphoric acid4
Non-redox product
–

Thermodynamic changes

Changes in standard condition

Reaction of barium bromide and sodium dihydrogenphosphate
3BaBr2Crystalline solid + 6NaH2PO4Crystalline solid
💧
⟶
Ba3(PO4)2↓Crystalline solid + 6NaBrCrystalline solid + 4H3PO4Crystalline solid
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
118–––
per 1 mol of
39.3–––
19.7–––
per 1 mol of
118–––
per 1 mol of
19.7–––
per 1 mol of
29.5–––

Changes in aqueous solution (1)

Reaction of barium bromide and sodium dihydrogenphosphate
3BaBr2Ionized aqueous solution + 6NaH2PO4Ionized aqueous solution
💧
⟶
Ba3(PO4)2↓Crystalline solid + 6NaBrIonized aqueous solution + 4H3PO4Un-ionized aqueous solution
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
145–––
per 1 mol of
48.3–––
24.2–––
per 1 mol of
145–––
per 1 mol of
24.2–––
per 1 mol of
36.3–––

Changes in aqueous solution (2)

Reaction of barium bromide and sodium dihydrogenphosphate
3BaBr2Ionized aqueous solution + 6NaH2PO4Ionized aqueous solution
💧
⟶
Ba3(PO4)2↓Crystalline solid + 6NaBrIonized aqueous solution + 4H3PO4Un-ionized aqueous solution
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
145–––
per 1 mol of
48.3–––
24.2–––
per 1 mol of
145–––
per 1 mol of
24.2–––
per 1 mol of
36.3–––

Changes in aqueous solution (3)

Reaction of barium bromide and sodium dihydrogenphosphate
3BaBr2Ionized aqueous solution + 6NaH2PO4Ionized aqueous solution
💧
⟶
Ba3(PO4)2↓Crystalline solid + 6NaBrIonized aqueous solution + 4H3PO4Ionized aqueous solution
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
189–––
per 1 mol of
63.0–––
31.5–––
per 1 mol of
189–––
per 1 mol of
31.5–––
per 1 mol of
47.3–––

Thermodynamic data of reactants

Chemical formulaStandard 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
BaBr2 (cr)-757.3[1]-736.8[1]146[1]–
BaBr2 (g)-439[1]-473[1]331[1]61.5[1]
BaBr2 (ai)-780.73[1]-768.68[1]174.5[1]–
BaBr2 (cr)
1 hydrate
-1068.2[1]–––
BaBr2 (cr)
2 hydrate
-1366.1[1]-1230.4[1]226[1]–
NaH2PO4 (cr)-1536.8[1]-1386.1[1]127.49[1]116.86[1]
NaH2PO4 (ai)-1536.41[1]-1392.17[1]149.4[1]–
NaH2PO4 (cr)
1 hydrate
-1833.0[1]–––
NaH2PO4 (cr)
2 hydrate
-2128.4[1]–––
* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formulaStandard 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
Ba3(PO4)2 (cr)-4092[1]–––
NaBr (cr)-361.062[1]-348.983[1]86.82[1]51.38[1]
NaBr (g)-143.1[1]-177.06[1]241.19[1]36.32[1]
NaBr (ai)-361.665[1]-365.849[1]141.4[1]-95.4[1]
NaBr (cr)
2 hydrate
-951.94[1]-828.29[1]179.1[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

  1. 1
    Janiel J. Reed (1989)
    The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
    National Institute of Standards and Technology (NIST)