Single Choice

Which will make basic buffer?

A$$50mL$$ of $$0.1$$ M $$NaOH+25mL$$ of $$0.1M\,CH_3COOH$$
B$$100mL$$ of $$0.1$$ M$$CH_3COOH+100mL$$ of $$0.1M\,NaOH$$
C$$100mL$$ of $$0.1M\,HCl+200mL$$ of $$0.1M\,NH_4OH$$
Correct Answer
D$$100mL$$ of $$0.1M\,HCl+100mL$$ of $$0.1$$M\,NaOH$$

Solution

1) $$\begin{matrix} CH_ 3COOH+ & NaOH & \rightarrow & CH_ 3COONa+ & H\_ 2O \\ 25mL\times 0.1M=2.5mmol & \quad 50mL\times 0.1M=5mmol0 & & 0 & \\ 0 & 2.5mmol & & 2.5mmol & \end{matrix}$$
This is basic solution due to $$NaOH$$. This is not basic buffer.
2) $$\begin{matrix} CH_ 3COOH+ & NaOH & \rightarrow & CH_ 3COONa+ & H_ 2O \\ 100mL\times 0.1M=10mmol & \quad 100mL\times 0.1M=10mmol & & 0 & \\ 0 & 0 & & 10mmol & \end{matrix}$$
Hydrolysis of salt takes place. This is not buffer.
3) $$\begin{matrix} HCl & NH_{ 4 }OH & \rightarrow & NH_ 4Cl+ & H_ 2O \\ 100mL\times 0.1M=10mmol & \quad 200mL\times 0.1M=20mmol & & 0 & \\ 0 & 10 & & 10mmol & \end{matrix}$$
This is basic buffer.
4)$$\begin{matrix} HCl & NaOH & \rightarrow & NaCl+ & H_{ 2 }O \\ 100mL\times 0.1M=10mmol & \quad 100mL\times 0.1M=20mmol & & 0 & \\ 0 & 0 & & 10mmol & \end{matrix}$$
Neutral solution.

SIMILAR QUESTIONS

Ionic Equilibrium in Solutions

The mixed solution of pthallic acid and potassium hydrogen pthallate is _________.

Ionic Equilibrium in Solutions

If $$0.00050$$ mol $$NaH{CO}_{3}$$ is added to $$1$$ litre of a buffered solution of $$pH\ 8$$, then how much material will exist in each of the three forms $${H}_{2}{CO}_{3},H{CO}_{3}^{-}$$ and $${CO}_{3}^{2-}$$? For $${H}_{2}{CO}_{3}$$, $${K}_{1}=5\times {10}^{-7}$$; $${K}_{2}=5\times {10}^{-13}$$

Ionic Equilibrium in Solutions

Which one of the following mixture does not act as a buffer solution?

Ionic Equilibrium in Solutions

What is a buffer solution?

Ionic Equilibrium in Solutions

Which one of the following pairs of solution is not an acidic buffer?

Ionic Equilibrium in Solutions

The total number of different kind of buffers obtained during the titration of $$H_3PO_4$$ with $$NaOH$$ are:

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