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Calculate the pH at the equivalence poin...

Calculate the pH at the equivalence point when a solution of 0.1 M acetic acid is titrated with a solution of 0.1 M NaOH. `K_(a)` for acid `=1.9xx10^(-5)`.

Text Solution

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At equivalence point , the conc . Of acetate would be `0.05` M . Solution acetat is a of a strong base and weak acid , For such for such salts we have
`pH = 1/2 [pK_(w) + pK_(a) + log C] = 1/2 [ 14 - log (1.9 xx10^(-5)) + log (0.05)] `
` = 1/2 [ 14 + 4.72 - 1.3] = 8.71 ` .
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