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 $0.1 \ M$ $HCl$

Vedclass · Answer

(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

Calculate $pH$ of the solution obtained by mixing $50 \ mL$ of $0.2 \ M$ $NH_4Cl$ solution and $75 \ mL$ of $0.1 \ M$ $NaOH$ solution. Given $pK_b$ for aqueous $NH_3$ is $4.74$.

The $[HCO_{3}^{-}]/[H_{2}CO_{3}]$ ratio in the buffer present in blood $(pH = 7.4)$ is approximately $(pK_{a} = 6.1$ for $H_{2}CO_{3})$.

In which of the following does a buffer solution play an important role?

The addition of small amounts of either acid or base to a buffer solution causes only small changes in $pH$ because the buffer solution

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