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[Chemistry] Equilibrium Question


CH3OH + CH3COOH CH3COOCH3 + H2O (ΔH = -8.5 kJ/mol)

Could anyone help me to understand why adding sodium hydroxide to the mixture shift the equilibrium to the left?
Reply 1
The reaction you've provided is an example of an esterification reaction, where methanol (CH3OH) and acetic acid (CH3COOH) react to form methyl acetate (CH3COOCH3) and water (H2O), with a negative change in enthalpy (ΔH = -8.5 kJ/mol). Which is same same , CH3OH + CH3COOH CH3COOCH3 + H2O.
I think by adding sodium hydroxide (NaOH) to the mixture can indeed shift the equilibrium of this reaction to the left. This is because sodium hydroxide is a strong base that can react with acetic acid (CH3COOH) to form the acetate ion (CH3COO-) and water. This reaction is a neutralization reaction,
By removing some of the acetic acid from the reaction mixture through this neutralization. Try to apply Le Chatelier's principle

Hope you have understood.
Reply 2
Thank you!

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