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3MnSO4 + 4Na2HPO4 💧→ Mn3(PO4)2↓ + 3Na2SO4 + 2NaH2PO4

3MnSO₄ + 4Na₂HPO₄ 💧→ Mn₃(PO₄)₂↓ + 3Na₂SO₄ + 2NaH₂PO₄

Last updated: August 11, 2023

Reaction of manganese(II) sulfate and sodium hydrogenphosphate: 3MnSO₄Manganese(II) sulfate + 4Na₂HPO₄Sodium hydrogenphosphate
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Mn₃(PO₄)₂↓Manganese(II) phosphate + 3Na₂SO₄Sodium sulfate + 2NaH₂PO₄Sodium dihydrogenphosphate

The reaction of manganese(II) sulfate and sodium hydrogenphosphate yields manganese(II) phosphate, sodium sulfate, and sodium dihydrogenphosphate (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 manganese(II) sulfate and sodium hydrogenphosphate: 3MnSO₄Manganese(II) sulfate + 4Na₂HPO₄Sodium hydrogenphosphate
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Mn₃(PO₄)₂↓Manganese(II) phosphate + 3Na₂SO₄Sodium sulfate + 2NaH₂PO₄Sodium dihydrogenphosphate

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 manganese(II) sulfate and sodium hydrogenphosphate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
MnSO₄	Manganese(II) sulfate	3	Lewis acid	Very soluble in water
Na₂HPO₄	Sodium hydrogenphosphate	4	Lewis base	Soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Mn₃(PO₄)₂	Manganese(II) phosphate	1	Lewis conjugate	Insoluble in water
Na₂SO₄	Sodium sulfate	3	Non-redox product	–
NaH₂PO₄	Sodium dihydrogenphosphate	2	Non-redox product	–

Thermodynamic changes

Changes in standard condition (1)

Reaction of manganese(II) sulfate and sodium hydrogenphosphate: 3MnSO₄Crystalline solid + 4Na₂HPO₄Crystalline solid
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Mn₃(PO₄)₂↓Crystalline solid + 3Na₂SO₄Crystalline solidorthorhombic + 2NaH₂PO₄Crystalline 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	−163.4	–	–	–
per 1 mol of Manganese(II) sulfate	−54.47	–	–	–
per 1 mol of Sodium hydrogenphosphate	−40.85	–	–	–
per 1 mol of Manganese(II) phosphate	−163.4	–	–	–
per 1 mol of Sodium sulfate	−54.47	–	–	–
per 1 mol of Sodium dihydrogenphosphate	−81.70	–	–	–

Changes in standard condition (2)

Reaction of manganese(II) sulfate and sodium hydrogenphosphate: 3MnSO₄Crystalline solid + 4Na₂HPO₄Crystalline solid
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Mn₃(PO₄)₂↓Crystalline solid + 3Na₂SO₄Crystalline solidmetastable + 2NaH₂PO₄Crystalline 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	–	–	–	–
per 1 mol of Manganese(II) sulfate	–	–	–	–
per 1 mol of Sodium hydrogenphosphate	–	–	–	–
per 1 mol of Manganese(II) phosphate	–	–	–	–
per 1 mol of Sodium sulfate	–	–	–	–
per 1 mol of Sodium dihydrogenphosphate	–	–	–	–

Changes in aqueous solution (1)

Reaction of manganese(II) sulfate and sodium hydrogenphosphate: 3MnSO₄Un-ionized aqueous solution + 4Na₂HPO₄Ionized aqueous solution
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Mn₃(PO₄)₂↓Crystalline solid + 3Na₂SO₄Ionized aqueous solution + 2NaH₂PO₄Ionized 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	79.2	–	–	–
per 1 mol of Manganese(II) sulfate	26.4	–	–	–
per 1 mol of Sodium hydrogenphosphate	19.8	–	–	–
per 1 mol of Manganese(II) phosphate	79.2	–	–	–
per 1 mol of Sodium sulfate	26.4	–	–	–
per 1 mol of Sodium dihydrogenphosphate	39.6	–	–	–

Changes in aqueous solution (2)

Reaction of manganese(II) sulfate and sodium hydrogenphosphate: 3MnSO₄Ionized aqueous solution + 4Na₂HPO₄Ionized aqueous solution
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Mn₃(PO₄)₂↓Crystalline solid + 3Na₂SO₄Ionized aqueous solution + 2NaH₂PO₄Ionized 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	121.8	–	–	–
per 1 mol of Manganese(II) sulfate	40.60	–	–	–
per 1 mol of Sodium hydrogenphosphate	30.45	–	–	–
per 1 mol of Manganese(II) phosphate	121.8	–	–	–
per 1 mol of Sodium sulfate	40.60	–	–	–
per 1 mol of Sodium dihydrogenphosphate	60.90	–	–	–

Changes in aqueous solution (3)

Reaction of manganese(II) sulfate and sodium hydrogenphosphate: 3MnSO₄Un-ionized aqueous solution + 4Na₂HPO₄Ionized aqueous solution
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Mn₃(PO₄)₂↓Crystalline solid + 3Na₂SO₄Ionized aqueous solution + 2NaH₂PO₄Ionized 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	79.2	–	–	–
per 1 mol of Manganese(II) sulfate	26.4	–	–	–
per 1 mol of Sodium hydrogenphosphate	19.8	–	–	–
per 1 mol of Manganese(II) phosphate	79.2	–	–	–
per 1 mol of Sodium sulfate	26.4	–	–	–
per 1 mol of Sodium dihydrogenphosphate	39.6	–	–	–

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
MnSO₄ (cr)	-1065.25^[1]	-957.36^[1]	112.1^[1]	100.50^[1]
MnSO₄ (ai)	-1130.1^[1]	-972.7^[1]	-53.6^[1]	-243^[1]
MnSO₄ (ao)	-1115.9^[1]	-985.7^[1]	36.4^[1]	–
MnSO₄ (cr) 1 hydrate α	-1376.5^[1]	–	–	–
MnSO₄ (cr) 1 hydrate β	-1348.1^[1]	–	–	–
MnSO₄ (cr) 4 hydrate	-2258.1^[1]	–	–	–
MnSO₄ (cr) 5 hydrate	-2553.1^[1]	–	–	326^[1]
MnSO₄ (cr) 7 hydrate	-3139.3^[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, (ai):Ionized aqueous solution, (ao):Un-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
Mn₃(PO₄)₂ (cr)	-3116.7^[1]	–	–	–
Na₂SO₄ (cr) orthorhombic	-1387.08^[1]	-1270.16^[1]	149.58^[1]	128.20^[1]
Na₂SO₄ (cr) metastable	–	–	154.934^[1]	129.29^[1]
Na₂SO₄ (ai)	-1389.51^[1]	-1268.36^[1]	138.1^[1]	-201^[1]
Na₂SO₄ (cr) 10 hydrate	-4327.26^[1]	-3646.85^[1]	592.0^[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, (ai):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)
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