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Chemical reactions
2FeBr3 + 3Na2HPO4 💧→ 2FePO4↓ + 6NaBr + H3PO4

2FeBr₃ + 3Na₂HPO₄ 💧→ 2FePO₄↓ + 6NaBr + H₃PO₄

Last updated: June 13, 2022

Reaction of iron(III) bromide and sodium hydrogenphosphate: 2FeBr₃Iron(III) bromide + 3Na₂HPO₄Sodium hydrogenphosphate
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2FePO₄↓Iron(III) phosphate + 6NaBrSodium bromide + H₃PO₄Phosphoric acid

The reaction of iron(III) bromide and sodium hydrogenphosphate yields iron(III) phosphate, sodium bromide, and phosphoric acid (Other reactions are here). This reaction is an acid-base reaction and is classified as follows:

Precipitation reaction

Table of contents

Reaction data

Chemical equation

Reaction of iron(III) bromide and sodium hydrogenphosphate: 2FeBr₃Iron(III) bromide + 3Na₂HPO₄Sodium hydrogenphosphate
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2FePO₄↓Iron(III) phosphate + 6NaBrSodium bromide + H₃PO₄Phosphoric 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
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Insoluble in water/Very slightly soluble in water/Slightly soluble in waterLewis conjugate + Product(Non-redox product)

Oxidation state of each atom

Reaction of iron(III) bromide and sodium hydrogenphosphate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
FeBr₃	Iron(III) bromide	2	Lewis acid	Soluble in water
Na₂HPO₄	Sodium hydrogenphosphate	3	Lewis base	Soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
FePO₄	Iron(III) phosphate	2	Lewis conjugate	Insoluble in water
NaBr	Sodium bromide	6	Non-redox product	–
H₃PO₄	Phosphoric acid	1	Non-redox product	–

Thermodynamic changes

Changes in standard condition

Reaction of iron(III) bromide and sodium hydrogenphosphate: 2FeBr₃Crystalline solid + 3Na₂HPO₄Crystalline solid
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2FePO₄↓Crystalline solid + 6NaBrCrystalline solid + H₃PO₄Crystalline solid

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	−259.7	–	–	–
per 1 mol of Iron(III) bromide	−129.8	–	–	–
per 1 mol of Sodium hydrogenphosphate	−86.57	–	–	–
per 1 mol of Iron(III) phosphate	−129.8	–	–	–
per 1 mol of Sodium bromide	−43.28	–	–	–
per 1 mol of Phosphoric acid	−259.7	–	–	–

Changes in aqueous solution (1)

Reaction of iron(III) bromide and sodium hydrogenphosphate: 2FeBr₃Ionized aqueous solution + 3Na₂HPO₄Ionized aqueous solution
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2FePO₄↓Crystalline solid + 6NaBrIonized aqueous solution + H₃PO₄Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	90.6	–	–	–
per 1 mol of Iron(III) bromide	45.3	–	–	–
per 1 mol of Sodium hydrogenphosphate	30.2	–	–	–
per 1 mol of Iron(III) phosphate	45.3	–	–	–
per 1 mol of Sodium bromide	15.1	–	–	–
per 1 mol of Phosphoric acid	90.6	–	–	–

Changes in aqueous solution (2)

Reaction of iron(III) bromide and sodium hydrogenphosphate: 2FeBr₃Ionized aqueous solution + 3Na₂HPO₄Ionized aqueous solution
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2FePO₄↓Crystalline solid + 6NaBrIonized aqueous solution + H₃PO₄Un-ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	90.6	–	–	–
per 1 mol of Iron(III) bromide	45.3	–	–	–
per 1 mol of Sodium hydrogenphosphate	30.2	–	–	–
per 1 mol of Iron(III) phosphate	45.3	–	–	–
per 1 mol of Sodium bromide	15.1	–	–	–
per 1 mol of Phosphoric acid	90.6	–	–	–

Changes in aqueous solution (3)

Reaction of iron(III) bromide and sodium hydrogenphosphate: 2FeBr₃Ionized aqueous solution + 3Na₂HPO₄Ionized aqueous solution
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2FePO₄↓Crystalline solid + 6NaBrIonized aqueous solution + H₃PO₄Ionized aqueous solution

	Standard enthalpy of reaction Δ_rH° kJ · mol⁻¹	Standard Gibbs energy of reaction Δ_rG° kJ · mol⁻¹	Standard entropy of reaction Δ_rS° J · K⁻¹ · mol⁻¹	Standard heat capacity of reaction at constant pressure Δ_rC_p° J · K⁻¹ · mol⁻¹
per 1 mol of Equation	101.6	–	–	–
per 1 mol of Iron(III) bromide	50.80	–	–	–
per 1 mol of Sodium hydrogenphosphate	33.87	–	–	–
per 1 mol of Iron(III) phosphate	50.80	–	–	–
per 1 mol of Sodium bromide	16.93	–	–	–
per 1 mol of Phosphoric acid	101.6	–	–	–

Thermodynamic data of reactants

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
FeBr₃ (cr)	-268.2^[1]	–	–	–
FeBr₃ (g)	-123.8^[1]	–	–	–
FeBr₃ (ai)	-413.4^[1]	-316.7^[1]	-68.6^[1]	–
Na₂HPO₄ (cr)	-1748.1^[1]	-1608.2^[1]	150.50^[1]	135.31^[1]
Na₂HPO₄ (ai)	-1772.38^[1]	-1612.98^[1]	84.5^[1]	–
Na₂HPO₄ (cr) 2 hydrate	-2346.0^[1]	-2088.5^[1]	221.3^[1]	–
Na₂HPO₄ (cr) 7 hydrate	-3821.7^[1]	-3279.8^[1]	434.59^[1]	–
Na₂HPO₄ (cr) 12 hydrate	-5297.8^[1]	-4467.8^[1]	633.83^[1]	–

* (cr):Crystalline solid, (g):Gas, (ai):Ionized aqueous solution

Thermodynamic data of products

Chemical formula	Standard enthalpy of formation Δ_fH° kJ · mol⁻¹	Standard Gibbs energy of formation Δ_fG° kJ · mol⁻¹	Standard molar entropy S° J · K⁻¹ · mol⁻¹	Standard molar heat capacity at constant pressure C_p° J · K⁻¹ · mol⁻¹
FePO₄ (cr)	-1297.5^[1]	–	–	–
FePO₄ (cr) 2 hydrate strengite	-1888.2^[1]	-1657.5^[1]	171.25^[1]	180.54^[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
Janiel J. Reed (1989)
The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI Units
https://doi.org/10.18434/M32124
National Institute of Standards and Technology (NIST)
Citation list