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Chemical reactions
ZnCO3 + 2NaOH → Na2CO3 + Zn(OH)2

ZnCO₃ + 2NaOH → Na₂CO₃ + Zn(OH)₂

Last updated: June 13, 2022

Reaction of zinc carbonate and sodium hydroxide: ZnCO₃Zinc carbonate + 2NaOHSodium hydroxide
⟶
Na₂CO₃Sodium carbonate + Zn(OH)₂Zinc hydroxide

The reaction of zinc carbonate and sodium hydroxide yields sodium carbonate and zinc hydroxide. This reaction is an acid-base reaction and is classified as follows:

Reaction of salt of weak base and strong base

Table of contents

Reaction data

Reactants

Chemical formula	Name	Coefficient	Type	Type in general equation
ZnCO₃	Zinc carbonate	1	Brønsted acid	Salt of weak base
NaOH	Sodium hydroxide	2	Brønsted base	Strong base

Products

Chemical formula	Name	Coefficient	Type	Type in general equation
Na₂CO₃	Sodium carbonate	1	Conjugate acid	Salt of strong base
Zn(OH)₂	Zinc hydroxide	1	Conjugate base	Weak base

Thermodynamic changes

Changes in standard condition (1)

Reaction of zinc carbonate and sodium hydroxide ◆ Δ_rG −107.74 kJ/mol K 7.50 × 10¹⁸ pK −18.88: ZnCO₃Crystalline solid + 2NaOHCrystalline solid
⟶
Na₂CO₃Crystalline solid + Zn(OH)₂Crystalline solidγ

	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	–	−107.74	–	–
per 1 mol of Zinc carbonate	–	−107.74	–	–
per 1 mol of Sodium hydroxide	–	−53.870	–	–
per 1 mol of Sodium carbonate	–	−107.74	–	–
per 1 mol of Zinc hydroxide	–	−107.74	–	–

Changes in standard condition (2)

Reaction of zinc carbonate and sodium hydroxide ◆ Δ_rG −107.45 kJ/mol K 6.67 × 10¹⁸ pK −18.82: ZnCO₃Crystalline solid + 2NaOHCrystalline solid
⟶
Na₂CO₃Crystalline solid + Zn(OH)₂Crystalline solidβ

	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	−108.59	−107.45	4.9	–
per 1 mol of Zinc carbonate	−108.59	−107.45	4.9	–
per 1 mol of Sodium hydroxide	−54.295	−53.725	2.5	–
per 1 mol of Sodium carbonate	−108.59	−107.45	4.9	–
per 1 mol of Zinc hydroxide	−108.59	−107.45	4.9	–

Changes in standard condition (3)

Reaction of zinc carbonate and sodium hydroxide ◆ Δ_rG −109.00 kJ/mol K 1.25 × 10¹⁹ pK −19.10: ZnCO₃Crystalline solid + 2NaOHCrystalline solid
⟶
Na₂CO₃Crystalline solid + Zn(OH)₂Crystalline solidε

	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	−109.93	−109.00	5.3	−14.1
per 1 mol of Zinc carbonate	−109.93	−109.00	5.3	−14.1
per 1 mol of Sodium hydroxide	−54.965	−54.500	2.6	−7.05
per 1 mol of Sodium carbonate	−109.93	−109.00	5.3	−14.1
per 1 mol of Zinc hydroxide	−109.93	−109.00	5.3	−14.1

Changes in standard condition (4)

Reaction of zinc carbonate and sodium hydroxide: ZnCO₃Crystalline solid + 2NaOHCrystalline solid
⟶
Na₂CO₃Crystalline solid + Zn(OH)₂Crystalline solidprecipitated

	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	−108.9	–	–	–
per 1 mol of Zinc carbonate	−108.9	–	–	–
per 1 mol of Sodium hydroxide	−54.45	–	–	–
per 1 mol of Sodium carbonate	−108.9	–	–	–
per 1 mol of Zinc hydroxide	−108.9	–	–	–

Changes in aqueous solution (1)

Reaction of zinc carbonate and sodium hydroxide ◆ Δ_rG −4.55 kJ/mol K 6.27 × 10⁰ pK −0.80: ZnCO₃Crystalline solid + 2NaOHIonized aqueous solution
⟶
Na₂CO₃Ionized aqueous solution + Zn(OH)₂Un-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	–	−4.55	–	–
per 1 mol of Zinc carbonate	–	−4.55	–	–
per 1 mol of Sodium hydroxide	–	−2.27	–	–
per 1 mol of Sodium carbonate	–	−4.55	–	–
per 1 mol of Zinc hydroxide	–	−4.55	–	–

Changes in aqueous solution (2)

Reaction of zinc carbonate and sodium hydroxide ◆ Δ_rG −35.63 kJ/mol K 1.75 × 10⁶ pK −6.24: ZnCO₃Crystalline solid + 2NaOHIonized aqueous solution
⟶
Na₂CO₃Ionized aqueous solution + Zn(OH)₂Crystalline solidγ

	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	–	−35.63	–	–
per 1 mol of Zinc carbonate	–	−35.63	–	–
per 1 mol of Sodium hydroxide	–	−17.82	–	–
per 1 mol of Sodium carbonate	–	−35.63	–	–
per 1 mol of Zinc hydroxide	–	−35.63	–	–

Changes in aqueous solution (3)

Reaction of zinc carbonate and sodium hydroxide ◆ Δ_rG −35.34 kJ/mol K 1.55 × 10⁶ pK −6.19: ZnCO₃Crystalline solid + 2NaOHIonized aqueous solution
⟶
Na₂CO₃Ionized aqueous solution + Zn(OH)₂Crystalline solidβ

	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	−46.28	−35.34	−36.3	–
per 1 mol of Zinc carbonate	−46.28	−35.34	−36.3	–
per 1 mol of Sodium hydroxide	−23.14	−17.67	−18.1	–
per 1 mol of Sodium carbonate	−46.28	−35.34	−36.3	–
per 1 mol of Zinc hydroxide	−46.28	−35.34	−36.3	–

Changes in aqueous solution (4)

Reaction of zinc carbonate and sodium hydroxide ◆ Δ_rG −36.89 kJ/mol K 2.90 × 10⁶ pK −6.46: ZnCO₃Crystalline solid + 2NaOHIonized aqueous solution
⟶
Na₂CO₃Ionized aqueous solution + Zn(OH)₂Crystalline solidε

	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	−47.62	−36.89	−35.9	–
per 1 mol of Zinc carbonate	−47.62	−36.89	−35.9	–
per 1 mol of Sodium hydroxide	−23.81	−18.45	−17.9	–
per 1 mol of Sodium carbonate	−47.62	−36.89	−35.9	–
per 1 mol of Zinc hydroxide	−47.62	−36.89	−35.9	–

Changes in aqueous solution (5)

Reaction of zinc carbonate and sodium hydroxide: ZnCO₃Crystalline solid + 2NaOHIonized aqueous solution
⟶
Na₂CO₃Ionized aqueous solution + Zn(OH)₂Crystalline solidprecipitated

	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	−46.6	–	–	–
per 1 mol of Zinc carbonate	−46.6	–	–	–
per 1 mol of Sodium hydroxide	−23.3	–	–	–
per 1 mol of Sodium carbonate	−46.6	–	–	–
per 1 mol of Zinc hydroxide	−46.6	–	–	–

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
ZnCO₃ (cr)	-812.78^[1]	-731.52^[1]	82.4^[1]	79.71^[1]
ZnCO₃ (cr) 1 hydrate	–	-970.6^[1]	–	–
NaOH (cr)	-425.609^[1]	-379.494^[1]	64.455^[1]	59.54^[1]
NaOH (g)	-207.1^[1]	-210.0^[1]	228.43^[1]	48.37^[1]
NaOH (ai)	-470.114^[1]	-419.150^[1]	48.1^[1]	-102.1^[1]
NaOH (cr) 1 hydrate	-734.543^[1]	-629.338^[1]	99.50^[1]	90.17^[1]
NaOH (l) 2 hydrate	-1019.076^[1]	-873.091^[1]	195.979^[1]	239.41^[1]
NaOH (l) 3.5 hydrate	-1459.798^[1]	-1236.356^[1]	286.089^[1]	354.43^[1]
NaOH (l) 4 hydrate	-1605.15^[1]	-1356.64^[1]	318.70^[1]	–
NaOH (l) 5 hydrate	-1894.31^[1]	-1596.34^[1]	386.06^[1]	–
NaOH (l) 7 hydrate	-2469.02^[1]	-2073.80^[1]	526.31^[1]	–

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

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
Na₂CO₃ (cr)	-1130.68^[1]	-1044.44^[1]	134.98^[1]	112.30^[1]
Na₂CO₃ (ai)	-1157.38^[1]	-1051.64^[1]	61.1^[1]	–
Na₂CO₃ (cr) 1 hydrate	-1431.26^[1]	-1285.31^[1]	168.11^[1]	145.60^[1]
Na₂CO₃ (cr) 7 hydrate	-3199.96^[1]	-2714.2^[1]	422.2^[1]	–
Na₂CO₃ (cr) 10 hydrate	-4081.32^[1]	-3427.66^[1]	562.7^[1]	550.32^[1]
Zn(OH)₂ (cr) γ	–	-553.81^[1]	–	–
Zn(OH)₂ (cr) β	-641.91^[1]	-553.52^[1]	81.2^[1]	–
Zn(OH)₂ (cr) ε	-643.25^[1]	-555.07^[1]	81.6^[1]	72.4^[1]
Zn(OH)₂ (cr) precipitated	-642.2^[1]	–	–	–
Zn(OH)₂ (ai)	-613.88^[1]	-461.56^[1]	-133.5^[1]	-251^[1]
Zn(OH)₂ (ao)	–	-522.73^[1]	–	–

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

Δ_rG	−107.74 kJ/mol
K	7.50 × 10¹⁸
pK	−18.88

Δ_rG	−107.45 kJ/mol
K	6.67 × 10¹⁸
pK	−18.82

Δ_rG	−109.00 kJ/mol
K	1.25 × 10¹⁹
pK	−19.10

Δ_rG	−4.55 kJ/mol
K	6.27 × 10⁰
pK	−0.80

ZnCO3 + 2NaOH → Na2CO3 + Zn(OH)2