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Question

# The pH of the solution when 0.2 mol HCl is added to 1 L of solution containing 0.1 M of of CH3COO− (acetate ion) is : Ka=1.8×10−5 and Volume= 1 L

A
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Solution

## The correct option is A 1Given, nHCl=0.2 mol [CH3COO−]=0.1 M Ka=1.8×10−5 and Volume= 1 L [HCl]=0.21=0.2 M CH3COO−+HCl⇌CH3COOH+HClInitial: 0.1 0.2 0 0Equilibrium: 0 0.1 0.1 0.1 Moles of CH3COOH=0.1 Since CH3COOH is a weak acid and HCl is a strong acid. In solution, both strong acid HCl and weak acid CH3COOH are present ∴ the dissociation of weak acid (CH3COOH) is suppressed by strong acid (HCl), due to common ion effect. Hence, we can neglect the [H+]ion from CH3COOH and consider [H+]ion only from HCl, that is a strong acid. [H+]=0.1pH=−log[H+]pH=−log(0.1)pH=1

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