Which of the following does not form a buffer | vedclass

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(C) buffer solution is formed by a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid.In option $A$, $NH_3$ (weak ba

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$NaOH + CH_3COOH$ ($1 : 1$ mole ratio)

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(C) buffer solution is formed by a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid.In option $A$, $NH_3$ (weak base) and $HCl$ (strong acid) in a $2:1$ ratio result in $NH_4Cl$ and $NH_3$, forming a basic buffer.In option $B$, $CH_3COOH$ (weak acid) and $NaOH$ (strong base) in a $2:1$ ratio result in $CH_3COONa$ and $CH_3COOH$, forming an acidic buffer.In option $C$, $NaOH$ and $CH_3COOH$ in a $1:1$ ratio undergo complete neutralization to form $CH_3COONa$ (a salt of a weak acid and strong base), which does not act as a buffer.In option $D$, $NH_4Cl$ and $NH_3$ form a standard basic buffer.

Which of the following does not form a buffer solution?

Similar Questions

$40 \ mL$ of $0.1 \ M$ ammonia solution is mixed with $20 \ mL$ of $0.1 \ M \ HCl$. What is the $pH$ of the mixture? ($pK_b$ of ammonia solution is $4.74$).

$A$ buffer solution can be prepared by mixing which of the following?

The $K_a$ of $CH_3COOH$ is $1.8 \times 10^{-5}$. How many grams of $CH_3COONa$ are required in $0.1 \ M \ CH_3COOH$ to form a solution having $pH = 4.0$? (Molecular mass of $CH_3COONa = 82 \ g \ mol^{-1}$)

The ratio of volumes of $CH_3COOH$ $0.1 \ N$ to $CH_3COONa$ $0.1 \ N$ required to prepare a buffer solution of $pH$ $5.74$ is (Given, $pK_a$ of $CH_3COOH$ is $4.74$)

Which of the following is a buffer solution of strong acidic nature?

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