(A) For a basic buffer solution, the $pOH$ is given by the Henderson-Hasselbalch equation: $pOH = pK_{b} + \log \frac{[Salt]}{[Base]}$ Given that the

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(A) For a basic buffer solution, the $pOH$ is given by the Henderson-Hasselbalch equation: $pOH = pK_{b} + \log \frac{[Salt]}{[Base]}$ Given that the molar concentrations of the base and its conjugate acid (salt) are the same, we have $[Salt] = [Base]$. Substituting this into the equation: $pOH = pK_{b} + \log(1)$ Since $\log(1) = 0$, we get: $pOH = pK_{b}$ Therefore, the $pOH$ of the buffer solution is the same as the $pK_{b}$ of the base.

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

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If the molar concentrations of a base and its conjugate acid are the same, then the $pOH$ of the buffer solution is:

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A
same as $pK_{b}$ of the base
B
same as $pK_{a}$ of the base
C
same as $pK_{a}$ of the acid
D
same as $pK_{b}$ of the acid

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6-2.Equilibrium-II (Ionic Equilibrium)

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$A$ certain buffer solution contains equal concentrations of $X^{-}$ and $HX$. The $K_a$ for $HX$ is $10^{-8}$. The $pH$ of the buffer is

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The $pK_b$ of $CN^{\Theta}$ is $4.7$. The $pH$ of a solution prepared by mixing $2.5 \ mol$ of $KCN$ and $2.5 \ mol$ of $HCN$ in water and making the total volume up to $500 \ mL$ is:

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$A$ buffer solution of $100 \ mL$ has a $pH$ value of $4$. When $1 \ mL$ of dilute $HCl$ is added to it,what happens to the $pH$ of the buffer solution?

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When an acid or alkali is mixed with a buffer solution,the $pH$ of the buffer solution:

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How many $mL$ of $0.2 \, M \, KCN$ should be mixed with $200 \, mL$ of $0.1 \, M \, HCN$ so as to make a mixture of $pH = 3$ ($pK_a$ for $HCN = 6$)?

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If the molar concentrations of a base and its conjugate acid are the same, then the $pOH$ of the buffer solution is:

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$A$ certain buffer solution contains equal concentrations of $X^{-}$ and $HX$. The $K_a$ for $HX$ is $10^{-8}$. The $pH$ of the buffer is

The $pK_b$ of $CN^{\Theta}$ is $4.7$. The $pH$ of a solution prepared by mixing $2.5 \ mol$ of $KCN$ and $2.5 \ mol$ of $HCN$ in water and making the total volume up to $500 \ mL$ is:

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When an acid or alkali is mixed with a buffer solution,the $pH$ of the buffer solution:

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