Which of the following will form a basic buff | vedclass

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Question

(D) basic buffer solution is formed by mixing a weak base with its salt of a strong acid,or by the partial neutralization of a weak base with a strong

Vedclass · Accepted Answer

$100 \ mL$ of $0.1 \ M$ $HCl + 200 \ mL$ of $0.1 \ M$ $NH_4OH$

Vedclass · Answer

(D) basic buffer solution is formed by mixing a weak base with its salt of a strong acid,or by the partial neutralization of a weak base with a strong acid.In option $D$,we have $100 \ mL$ of $0.1 \ M$ $HCl$ $(10 \ mmol)$ and $200 \ mL$ of $0.1 \ M$ $NH_4OH$ $(20 \ mmol)$.The reaction is: $NH_4OH + HCl \rightarrow NH_4Cl + H_2O$.After the reaction,$10 \ mmol$ of $NH_4OH$ (weak base) remains,and $10 \ mmol$ of $NH_4Cl$ (salt of weak base and strong acid) is formed.This mixture of a weak base and its salt acts as a basic buffer.

Which of the following will form a basic buffer solution?

Similar Questions

One litre of an aqueous solution contains $0.15 \ mol$ of $CH_3COOH$ $(pK_a = 4.8)$ and $0.15 \ mol$ of $CH_3COONa$. After the addition of $0.05 \ mol$ of solid $NaOH$ to this solution,the $pH$ will be:

In which of the following combinations is buffer action expected?
$1$. $NH_3 + NH_4Cl$
$2$. $HCl + NaCl$
$3$. $NH_3 + HCl$ in $2 : 1$ mole ratio
Select the correct answer using the code given below.

What is the total number of buffers formed during the titration of $H_3PO_4$ with $NaOH$?

Which of the following buffer solutions will have the highest acidic character?

The $pH$ of a buffer solution made by mixing $25 \ mL$ of $0.02 \ M$ $NH_4OH$ and $25 \ mL$ of $0.2 \ M$ $NH_4Cl$ at $25^{\circ}C$ is ($pK_b$ of $NH_4OH = 4.8$).

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