What is the ratio of pH for a solution contai | vedclass

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(A) For the first solution: $CH_3COONa + HCl \rightarrow CH_3COOH + NaCl$. Initially,we have $1 \ mol$ of $CH_3COONa$ and $0.5 \ mol$ of $HCl$. After

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$1 : 1$

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(A) For the first solution: $CH_3COONa + HCl \rightarrow CH_3COOH + NaCl$. Initially,we have $1 \ mol$ of $CH_3COONa$ and $0.5 \ mol$ of $HCl$. After the reaction,$0.5 \ mol$ of $CH_3COONa$ remains and $0.5 \ mol$ of $CH_3COOH$ is formed. Using the Henderson-Hasselbalch equation: $pH_1 = pK_a + \log(\frac{[Salt]}{[Acid]}) = pK_a + \log(\frac{0.5}{0.5}) = pK_a$. For the second solution: $1 \ mol$ $CH_3COONa$ and $1 \ mol$ $CH_3COOH$ are present. $pH_2 = pK_a + \log(\frac{1}{1}) = pK_a$. Therefore,the ratio of $pH_1 : pH_2 = pK_a : pK_a = 1 : 1$.

What is the ratio of $pH$ for a solution containing $1 \ mol$ $CH_3COONa$ + $0.5 \ mol$ $HCl$ per liter and another solution containing $1 \ mol$ $CH_3COONa$ + $1 \ mol$ $CH_3COOH$ per liter?

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