Which of the following would produce a buffer | vedclass

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(A) buffer solution is formed by mixing a weak acid and its salt with a strong base, or a weak base and its salt with a strong acid. When $1 \ M \ CH_

Vedclass · Accepted Answer

$1 \ M \ CH_3COOH$ and $0.5 \ M \ NaOH$

Vedclass · Answer

(A) buffer solution is formed by mixing a weak acid and its salt with a strong base, or a weak base and its salt with a strong acid. When $1 \ M \ CH_3COOH$ and $0.5 \ M \ NaOH$ are mixed in equal volumes, the reaction is: $CH_3COOH + NaOH \longrightarrow CH_3COONa + H_2O$. Since the concentration of $CH_3COOH$ $(1 \ M)$ is double that of $NaOH$ $(0.5 \ M)$, after the reaction, $0.5 \ M$ of $CH_3COOH$ remains unreacted, and $0.5 \ M$ of $CH_3COONa$ is formed. This mixture of a weak acid $(CH_3COOH)$ and its salt $(CH_3COONa)$ acts as an acidic buffer.

Which of the following would produce a buffer solution when mixed in equal volumes?

Similar Questions

Buffer solutions have constant acidity and alkalinity because

If $12.5 \ mL$ of $0.1 \ M$ $KOH$ is added into $50 \ mL$ of $0.1 \ M$ $CH_3COOH$ solution,then what would be the final $pH$? $(K_a(CH_3COOH) = 2 \times 10^{-5})$

Assertion : In a titration of weak acid and $NaOH$,the $pH$ at half equivalence point is $pK_a$.
Reason : At half equivalence point,it forms an acidic buffer and the buffer capacity is maximum where $[acid] = [salt]$.

Give the importance of buffer solution.

$A$ buffer solution is prepared by mixing $0.2 \ M$ sodium acetate and $0.1 \ M$ acetic acid. If $pK_{a}$ for acetic acid is $4.7$,find the $pH$.

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