(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 2 Equilibrium: 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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2 Equilibrium: Ionic Equilibrium

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Buffer solution

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$100 \ mL$ of a solution contains $0.1 \ M$ $NH_4OH$ and $0.1 \ M$ $NH_4Cl$. The $pH$ of the solution will not change on adding :-

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Calculate the $pH$ of the solution in which $0.2 \, M \, NH_{4}Cl$ and $0.1 \, M \, NH_{3}$ are present. The $pK_{b}$ of ammonia solution is $4.75$.

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$20 \ mL$ solution contains $0.1 \ M \ NH_4Cl$ and $0.01 \ M \ NH_4OH$. By adding which one will its $pH$ not change?

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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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$A$ solution contains $0.2 \ M \ NH_4OH$ and $0.2 \ M \ NH_4Cl$. If $1.0 \ mL$ of $0.001 \ M \ HCl$ is added,what will be the $[OH^-]$ of the resulting solution? [Given: $K_b = 2 \times 10^{-5}$]

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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:

Similar Questions

$100 \ mL$ of a solution contains $0.1 \ M$ $NH_4OH$ and $0.1 \ M$ $NH_4Cl$. The $pH$ of the solution will not change on adding :-

Calculate the $pH$ of the solution in which $0.2 \, M \, NH_{4}Cl$ and $0.1 \, M \, NH_{3}$ are present. The $pK_{b}$ of ammonia solution is $4.75$.

$20 \ mL$ solution contains $0.1 \ M \ NH_4Cl$ and $0.01 \ M \ NH_4OH$. By adding which one will its $pH$ not change?

$A$ 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?

$A$ solution contains $0.2 \ M \ NH_4OH$ and $0.2 \ M \ NH_4Cl$. If $1.0 \ mL$ of $0.001 \ M \ HCl$ is added,what will be the $[OH^-]$ of the resulting solution? [Given: $K_b = 2 \times 10^{-5}$]

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