Which of the following mixtures of solutions | vedclass

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(D) buffer solution is formed by a weak acid and its conjugate base,or a weak base and its conjugate acid. In option $A$,$CH_3COOH$ (weak acid) and $N

Vedclass · Accepted Answer

$50 \ mL$ of $0.2 \ M$ $NH_3 + 50 \ mL$ of $0.1 \ M$ $HCl$

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(D) buffer solution is formed by a weak acid and its conjugate base,or a weak base and its conjugate acid. In option $A$,$CH_3COOH$ (weak acid) and $NaOH$ (strong base) react in a $1:1$ molar ratio ($5 \ mmol$ each) to form $CH_3COONa$ (salt),leaving no weak acid behind. In option $B$,$HCl$ (strong acid) and $NaOH$ (strong base) neutralize completely to form $NaCl$ and water. In option $C$,$NH_3$ (weak base) and $HCl$ (strong acid) react in a $1:1$ molar ratio ($10 \ mmol$ each) to form $NH_4Cl$ (salt),leaving no weak base behind. In option $D$,$NH_3$ $(10 \ mmol)$ reacts with $HCl$ $(5 \ mmol)$ to form $5 \ mmol$ of $NH_4Cl$ and leaves $5 \ mmol$ of unreacted $NH_3$. This mixture of a weak base $(NH_3)$ and its conjugate acid $(NH_4^+)$ acts as a basic buffer.

Which of the following mixtures of solutions can function as a buffer solution?

Similar Questions

The $pH$ of a buffer solution containing $0.2 \ mol/L$ $CH_3COONa$ and $1.5 \ mol/L$ $CH_3COOH$ is ($K_a$ for acetic acid is $1.8 \times 10^{-5}$).

$pH$ of $0.1 \ M$ solution of a weak acid $(HA)$ is $4.50$. It is neutralized with $NaOH$ solution to decrease the acid content to half. The $pH$ of the resulting solution is:

An aqueous buffer is prepared by adding $100 \, mL$ of $0.1 \, mol \, L^{-1}$ acetic acid to $50 \, mL$ of $0.2 \, mol \, L^{-1}$ of sodium acetate. If $pK_a$ of acetic acid is $4.76$,the $pH$ of the buffer is

Find the $pH$ when $0.2 \, mol$ of $HCl$ is added to $1 \, L$ of a solution containing $1 \, M$ $CH_3COOH$ and $1 \, M$ $CH_3COO^-$. Assume the total volume remains $1 \, L$. Given $K_a$ for $CH_3COOH = 1.8 \times 10^{-5}$.

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