Calculate the value of the equilibrium constant (Kc) for the reaction of acetic

Question

Calculate the value of the equilibrium constant (Kc) for the reaction of acetic acid with sodium hydroxide.

What is the significance of the value of Kc in this case?

Explanation / Answer

The reaction can be written as, CH3COOH + NaOH ---> CH3COONa + H2O Equilibrium constant Kc can be determined by a simple method i.e. IN THE NUMERATOR the multiplication of the concentration of the products raise the power of its coefficient individually IN THE DENOMINATOR the multiplication of the concentration of the reactants raise the power of its coefficient respectively If there is H2O in the reaction then we do not put it in the equilibrium constant equation because its concentration is assumed to be unity. Therefore the equation for Kc is, Kc = [CH3COONa] / ([CH3COOH][NaOH]) where the coefficient of all the reactants and products is unity.

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