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2KHSO4 + 3(NH4)2CrO4 💧→ K2CrO4↓ + 2(NH4)2SO4 + (NH4)2Cr2O7 + H2O

2KHSO₄ + 3(NH₄)₂CrO₄ 💧→ K₂CrO₄↓ + 2(NH₄)₂SO₄ + (NH₄)₂Cr₂O₇ + H₂O

Last updated: August 11, 2023

Reaction of potassium hydrogensulfate and ammonium chromate: 2KHSO₄Potassium hydrogensulfate + 3(NH₄)₂CrO₄Ammonium chromate
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K₂CrO₄↓Potassium chromate + 2(NH₄)₂SO₄Ammonium sulfate + (NH₄)₂Cr₂O₇Ammonium dichromate + H₂OWater

The reaction of potassium hydrogensulfate and ammonium chromate yields potassium chromate, ammonium sulfate, ammonium dichromate, and water (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 potassium hydrogensulfate and ammonium chromate: 2KHSO₄Potassium hydrogensulfate + 3(NH₄)₂CrO₄Ammonium chromate
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K₂CrO₄↓Potassium chromate + 2(NH₄)₂SO₄Ammonium sulfate + (NH₄)₂Cr₂O₇Ammonium dichromate + H₂OWater

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 potassium hydrogensulfate and ammonium chromate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
KHSO₄	Potassium hydrogensulfate	2	Lewis acid	Very soluble in water
(NH₄)₂CrO₄	Ammonium chromate	3	Lewis base	Very soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
K₂CrO₄	Potassium chromate	1	Lewis conjugate	Insoluble in water
(NH₄)₂SO₄	Ammonium sulfate	2	Non-redox product	–
(NH₄)₂Cr₂O₇	Ammonium dichromate	1	Non-redox product	–
H₂O	Water	1	Non-redox product	–

Thermodynamic changes

Changes in standard condition

Reaction of potassium hydrogensulfate and ammonium chromate: 2KHSO₄Crystalline solid + 3(NH₄)₂CrO₄Crystalline solid
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K₂CrO₄↓Crystalline solid + 2(NH₄)₂SO₄Crystalline solid + (NH₄)₂Cr₂O₇Crystalline solid + H₂OLiquid

	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	−34.8	–	–	–
per 1 mol of Potassium hydrogensulfate	−17.4	–	–	–
per 1 mol of Ammonium chromate	−11.6	–	–	–
per 1 mol of Potassium chromate	−34.8	–	–	–
per 1 mol of Ammonium sulfate	−17.4	–	–	–
per 1 mol of Ammonium dichromate	−34.8	–	–	–
per 1 mol of Water	−34.8	–	–	–

Changes in aqueous solution

Reaction of potassium hydrogensulfate and ammonium chromate ◆ Δ_rG −59.8 kJ/mol K 3.00 × 10¹⁰ pK −10.48: 2KHSO₄Ionized aqueous solution + 3(NH₄)₂CrO₄Ionized aqueous solution
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K₂CrO₄↓Ionized aqueous solution + 2(NH₄)₂SO₄Ionized aqueous solution + (NH₄)₂Cr₂O₇Ionized aqueous solution + H₂OLiquid

	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	−57.6	−59.8	8.0	–
per 1 mol of Potassium hydrogensulfate	−28.8	−29.9	4.0	–
per 1 mol of Ammonium chromate	−19.2	−19.9	2.7	–
per 1 mol of Potassium chromate	−57.6	−59.8	8.0	–
per 1 mol of Ammonium sulfate	−28.8	−29.9	4.0	–
per 1 mol of Ammonium dichromate	−57.6	−59.8	8.0	–
per 1 mol of Water	−57.6	−59.8	8.0	–

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
KHSO₄ (cr)	-1160.6^[1]	-1031.3^[1]	138.1^[1]	–
KHSO₄ (ai)	-1139.72^[1]	-1039.18^[1]	234.3^[1]	-63^[1]
(NH₄)₂CrO₄ (cr)	-1167.3^[1]	–	–	–
(NH₄)₂CrO₄ (ai)	-1146.16^[1]	-886.36^[1]	277.0^[1]	–

* (cr):Crystalline solid, (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
K₂CrO₄ (cr)	-1403.7^[1]	-1295.7^[1]	200.12^[1]	145.98^[1]
K₂CrO₄ (ai)	-1385.91^[1]	-1294.30^[1]	255.2^[1]	–
(NH₄)₂SO₄ (cr)	-1180.85^[1]	-901.67^[1]	220.1^[1]	187.49^[1]
(NH₄)₂SO₄ (ai)	-1174.28^[1]	-903.14^[1]	246.9^[1]	-133.1^[1]
(NH₄)₂Cr₂O₇ (cr)	-1806.7^[1]	–	–	–
(NH₄)₂Cr₂O₇ (ai)	-1755.2^[1]	-1459.5^[1]	488.7^[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

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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