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What is the pH of the solution when 0.2 ...

What is the pH of the solution when 0.2 mole of hydrochloric acid is added to one litre of a solution containing 1 M acetic acid and acetate ion ? Assume that the total volume is one litre .`K_(a)` for `CH_(3)COOH =1.8 xx 10^(-5)`.

Text Solution

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On adding HCI, the free hydrogen ions will combine with `CH_(3)COO^(-)` ions to form `CH_(3)COOH.` Thus the concentration of acetic acid increases while that of `CH_(3)COO^(-)` ions decreases.
`[CH_(3)COOH] =(0.2 +1) = 1.2 " mol litre"^(-1) = 1.2 M`
`["Salt"] = (1-0.2) -0.8" mol litre"^(-1) =.8 M`
Applying Henderson's equation `pH =pK_(a) + log. [["Salt"]]/[["Acid"]] =- log K_(a) + log. [["Salt"]]/[["Acid"]]`
`=- (log 1.8 xx 10^(-5)) + log. ((0.8))/((1.2))`
`= (5 - log 1.8) + log (0.67) = (5 -0.255) -0.174 = 4.571.`
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