In a mixture of acetic acid and sodium acetat | vedclass

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(A) The $pH$ of an acidic buffer is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.Initially,let the ratio be $

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Increases by $1$

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(A) The $pH$ of an acidic buffer is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.Initially,let the ratio be $R = \frac{[Salt]}{[Acid]}$. So,$pH_1 = pK_a + \log(R)$.When the ratio is increased ten times,the new ratio becomes $10R$.The new $pH$ is $pH_2 = pK_a + \log(10R)$.$pH_2 = pK_a + \log(10) + \log(R) = pK_a + 1 + \log(R)$.Comparing the two,$pH_2 = pH_1 + 1$.Therefore,the $pH$ increases by $1$.

In a mixture of acetic acid and sodium acetate,the ratio of the concentration of the salt to the acid is increased ten times. Then the $pH$ of the solution:

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