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Chemical reactions
Sr(CH3COO)2 + KHCO3 💧→ SrCO3↓ + CH3COOK + CH3COOH

Sr(CH₃COO)₂ + KHCO₃ 💧→ SrCO₃↓ + CH₃COOK + CH₃COOH

Last updated: June 13, 2022

Reaction of strontium acetate and potassium hydrogencarbonate: Sr(CH₃COO)₂Strontium acetate + KHCO₃Potassium hydrogencarbonate
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SrCO₃↓Strontium carbonate + CH₃COOKPotassium acetate + CH₃COOHAcetic acid

The reaction of strontium acetate and potassium hydrogencarbonate yields strontium carbonate, potassium acetate, and acetic 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 strontium acetate and potassium hydrogencarbonate: Sr(CH₃COO)₂Strontium acetate + KHCO₃Potassium hydrogencarbonate
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SrCO₃↓Strontium carbonate + CH₃COOKPotassium acetate + CH₃COOHAcetic 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 strontium acetate and potassium hydrogencarbonate

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
Sr(CH₃COO)₂	Strontium acetate	1	Lewis acid	Very soluble in water
KHCO₃	Potassium hydrogencarbonate	1	Lewis base	Very soluble in water

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
SrCO₃	Strontium carbonate	1	Lewis conjugate	Insoluble in water
CH₃COOK	Potassium acetate	1	Non-redox product	–
CH₃COOH	Acetic acid	1	Non-redox product	–

Thermodynamic changes

Changes in standard condition

Reaction of strontium acetate and potassium hydrogencarbonate: Sr(CH₃COO)₂Crystalline solid + KHCO₃Crystalline solid
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SrCO₃↓Crystalline solid + CH₃COOKCrystalline solid + CH₃COOHLiquid

	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	23.0	–	–	–
per 1 mol of Strontium acetate	23.0	–	–	–
per 1 mol of Potassium hydrogencarbonate	23.0	–	–	–
per 1 mol of Strontium carbonate	23.0	–	–	–
per 1 mol of Potassium acetate	23.0	–	–	–
per 1 mol of Acetic acid	23.0	–	–	–

Changes in aqueous solution (1)

Reaction of strontium acetate and potassium hydrogencarbonate: Sr(CH₃COO)₂Aqueous solution + KHCO₃Ionized aqueous solution
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SrCO₃↓Crystalline solid + CH₃COOKIonized aqueous solution + CH₃COOHUn-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	12.2	–	–	–
per 1 mol of Strontium acetate	12.2	–	–	–
per 1 mol of Potassium hydrogencarbonate	12.2	–	–	–
per 1 mol of Strontium carbonate	12.2	–	–	–
per 1 mol of Potassium acetate	12.2	–	–	–
per 1 mol of Acetic acid	12.2	–	–	–

Changes in aqueous solution (2)

Reaction of strontium acetate and potassium hydrogencarbonate: Sr(CH₃COO)₂Aqueous solution + KHCO₃Ionized aqueous solution
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SrCO₃↓Crystalline solid + CH₃COOKIonized aqueous solution + CH₃COOHIonized 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	12.0	–	–	–
per 1 mol of Strontium acetate	12.0	–	–	–
per 1 mol of Potassium hydrogencarbonate	12.0	–	–	–
per 1 mol of Strontium carbonate	12.0	–	–	–
per 1 mol of Potassium acetate	12.0	–	–	–
per 1 mol of Acetic acid	12.0	–	–	–

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
Sr(CH₃COO)₂ (cr)	-1487.4^[1]	–	–	–
Sr(CH₃COO)₂ (aq)	-1512.1^[1]	–	–	–
Sr(CH₃COO)₂ (cr) 0.5 hydrate	-1631.8^[1]	–	–	–
KHCO₃ (cr)	-963.2^[1]	-863.5^[1]	115.5^[1]	–
KHCO₃ (ai)	-944.37^[1]	-870.04^[1]	193.7^[1]	–

* (cr):Crystalline solid, (aq):Aqueous solution, (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
SrCO₃ (cr)	-1220.1^[1]	-1140.1^[1]	97.1^[1]	81.42^[1]
SrCO₃ (ai)	-1222.94^[1]	-1087.29^[1]	-89.5^[1]	–
CH₃COOK (cr)	-723.0^[1]	–	–	–
CH₃COOK (ai)	-738.39^[1]	-652.58^[1]	189.1^[1]	15.5^[1]
CH₃COOH (l)	-484.5^[1]	-389.9^[1]	159.8^[1]	124.3^[1]
CH₃COOH (g)	-432.25^[1]	-374.0^[1]	282.5^[1]	66.5^[1]
CH₃COOH (ai)	-486.01^[1]	-369.31^[1]	86.6^[1]	-6.3^[1]
CH₃COOH (ao)	-485.76^[1]	-396.46^[1]	178.7^[1]	–

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