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Question

Calculate the ratio of pH of a solution containing 1 mol. of CH3COONa+1mol of HCl per litre and of other solution containing 1 mol of CH3COONa+1mol of CH3COOH per litre.

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Solution

Case I: pH when 1 mol CH and 1 mol HCI are present
CH3COONa+HClCH3COOH+NaCl
Before reaction 1 1 0 0
After reaction 0 0 1 1
[CH3COOH]=1 M
[H]=Cα=C(KaC)=KaC=(Ka)(C=1)
pH1=12logKa
Case II: pH when 1 mol CH3COONa and 1 mole of CH3COOH; a buffer solution
pH2=logKa+log[Salt][Acid]
[[Salt]=1M[Acid]=1M]
pH2=logKa
pH1pH2=12=0.5

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