(B) The Henderson-Hasselbalch equation for an acidic buffer is: $pH = pK_a + \log \frac{[salt]}{[acid]}$Given $K_a = 10^{-4}$,so $pK_a = - \log(10^{-4

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(B) The Henderson-Hasselbalch equation for an acidic buffer is: $pH = pK_a + \log \frac{[salt]}{[acid]}$Given $K_a = 10^{-4}$,so $pK_a = - \log(10^{-4}) = 4$.Substituting the values into the equation: $5 = 4 + \log \frac{[salt]}{[acid]}$$\log \frac{[salt]}{[acid]} = 5 - 4 = 1$Taking the antilog on both sides: $\frac{[salt]}{[acid]} = 10^1 = 10$Therefore,the ratio of $[salt]$ to $[acid]$ is $10:1$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Buffer solution

Medium

The ionization constant $(K_a)$ of a certain weak acid is $10^{-4}$. What should be the $[salt]$ to $[acid]$ ratio if we have to prepare a buffer with $pH = 5$ using this acid and one of its salts?

A
$1:10$
B
$10:1$
C
$5:4$
D
$4:5$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Buffer solution

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$A$ certain buffer solution contains equal concentrations of $X^-$ and $HX$. If the $K_a$ of $HX$ is $10^{-8}$,then the $pH$ of the buffer solution will be ...... .

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Find the $pH$ of a buffer solution prepared by mixing $300 \, mL$ of $0.3 \, M \, NH_3$ and $500 \, mL$ of $0.5 \, M \, NH_4Cl$. Given $K_b$ for $NH_3 = 1.8 \times 10^{-5}$.

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If $20 \ mL$ of $0.1 \ M \ NaOH$ is added to $30 \ mL$ of $0.2 \ M \ CH_3COOH$ $(pK_a = 4.74)$,find the $pH$ of the resulting solution.

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The ionization constant $(K_a)$ of a certain weak acid is $10^{-4}$. What should be the $[salt]$ to $[acid]$ ratio if we have to prepare a buffer with $pH = 5$ using this acid and one of its salts?

Similar Questions

The addition of small amounts of either acid or base to a buffer solution causes only small changes in $pH$ because the buffer solution

What is the concentration of $[H^+]$ in $mol/L$ in a mixed solution of $0.20 \ M \ CH_3COONa$ and $0.10 \ M \ CH_3COOH$? (Given: $K_a$ of $CH_3COOH = 1.8 \times 10^{-5}$)

$A$ certain buffer solution contains equal concentrations of $X^-$ and $HX$. If the $K_a$ of $HX$ is $10^{-8}$,then the $pH$ of the buffer solution will be ...... .

Find the $pH$ of a buffer solution prepared by mixing $300 \, mL$ of $0.3 \, M \, NH_3$ and $500 \, mL$ of $0.5 \, M \, NH_4Cl$. Given $K_b$ for $NH_3 = 1.8 \times 10^{-5}$.

If $20 \ mL$ of $0.1 \ M \ NaOH$ is added to $30 \ mL$ of $0.2 \ M \ CH_3COOH$ $(pK_a = 4.74)$,find the $pH$ of the resulting solution.

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