(A) For an acidic buffer,the Henderson-Hasselbalch equation is given by: $pH = pK_{a} + \log \frac{[\text{Salt}]}{[\text{Acid}]}$ Given that the conce

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(A) For an acidic buffer,the Henderson-Hasselbalch equation is given by: $pH = pK_{a} + \log \frac{[\text{Salt}]}{[\text{Acid}]}$ Given that the concentrations of the weak acid and its salt are equal,i.e.,$[\text{Salt}] = [\text{Acid}]$. Therefore,the equation simplifies to: $pH = pK_{a} = -\log K_{a}$ Given $K_{a} = 1.8 \times 10^{-5}$. $pH = -\log (1.8 \times 10^{-5}) = -(\log 1.8 + \log 10^{-5})$ $pH = -(\log 1.8 - 5) = 5 - \log 1.8$ Using $\log 1.8 \approx 0.2553$: $pH = 5 - 0.2553 = 4.7447$

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

Medium

$A$ buffer solution contains equal concentrations of weak acid and its salt with a strong base. Calculate the $pH$ of the buffer solution if the dissociation constant of the weak acid is $1.8 \times 10^{-5}$.

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A
$4.7447$
B
$5.142$
C
$5.8496$
D
$4.0128$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Buffer solution

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Which of the following acts as a buffer solution?

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The $pOH$ of a basic buffer (e.g.,$NH_4OH/NH_4Cl$) is $5$. If the concentration of the salt is tripled while the concentration of the base remains constant,find the new $pOH$ value. (Given: $\log 3 = 0.48$)

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$A$ buffer that is a mixture of acetic acid $(K_a = 2 \times 10^{-5})$ and potassium acetate has $pH = 5.18$. The $\frac{[CH_3COO^{-}]}{[CH_3COOH]}$ ratio in this buffer is approximately:

Medium

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When $30 \ mL$ of $0.2 \ M \ NH_4OH$ is added to $30 \ mL$ of $2 \ M \ NH_4Cl$ solution. If the $pH$ of the buffer formed is $8.2$,what is the $pK_b$ of $NH_4OH$?

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What would be the $pH$ of a solution obtained by mixing $5 \ g$ of acetic acid and $7.5 \ g$ of sodium acetate and making the volume equal to $500 \ mL$? $(K_a = 1.75 \times 10^{-5}, pK_a = 4.76)$

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$A$ buffer solution contains equal concentrations of weak acid and its salt with a strong base. Calculate the $pH$ of the buffer solution if the dissociation constant of the weak acid is $1.8 \times 10^{-5}$.

Similar Questions

Which of the following acts as a buffer solution?

The $pOH$ of a basic buffer (e.g.,$NH_4OH/NH_4Cl$) is $5$. If the concentration of the salt is tripled while the concentration of the base remains constant,find the new $pOH$ value. (Given: $\log 3 = 0.48$)

$A$ buffer that is a mixture of acetic acid $(K_a = 2 \times 10^{-5})$ and potassium acetate has $pH = 5.18$. The $\frac{[CH_3COO^{-}]}{[CH_3COOH]}$ ratio in this buffer is approximately:

When $30 \ mL$ of $0.2 \ M \ NH_4OH$ is added to $30 \ mL$ of $2 \ M \ NH_4Cl$ solution. If the $pH$ of the buffer formed is $8.2$,what is the $pK_b$ of $NH_4OH$?

What would be the $pH$ of a solution obtained by mixing $5 \ g$ of acetic acid and $7.5 \ g$ of sodium acetate and making the volume equal to $500 \ mL$? $(K_a = 1.75 \times 10^{-5}, pK_a = 4.76)$

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