MCQ
A buffer solution contains $6.4 \times {10^{ - 5}}$ of acetic acid and $0.1\,\,M$ of sodium acetate. What will be its $pH$, if $p{K_a}$ of acetic acid is $4.75$
- A$4$
- ✓$4.75$
- C$5$
- D$5.25$
✓
Answer
Correct option: B.
$4.75$
(b) $pH = p{K_a} + {\rm{log}}\frac{{{\rm{[Salt]}}}}{{{\rm{[Acid]}}}}$; $pH = 4.75 + {\rm{log}}\frac{{0.1}}{{0.1}}$
$pH = 4.75 + {\rm{log}}\,\,1$; $pH = 4.75$
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
Internal energy does not include
Which of the following is not affected by change in pressure?
Electronic configuration of $S{c^{21}}$ is
→Product $(B)$ is
→The oxidation state of iodine in $\mathrm{H}_4 \mathrm{IO}_6{ }^{\ominus}$ is :
→One mole of Argon is heated using $PV^{5/2} =$ constant. By what amount heat is absorbed during the process, when temperature changes by $\Delta T = 26\ K$ ......$J$
→The electronegativity of the following elements increases in the order
$CH \equiv CH\mathop {\xrightarrow{{HgS{O_4}}}}\limits_{{H_2}S{O_4}} \mathop {\xrightarrow{{C{H_3}MgBr}}}\limits_{{H_2}O} \xrightarrow{{P/B{r_2}}}$
→The following equilibrium exists in an aqueous solution of hydrogen sulphide : ${H_2}S $ $\rightleftharpoons$ $ {H^ + } + H{S^ - }$
→If dilute $HCl$ is added to an aqueous solution of ${H_2}S$ without any change in temperature
Arrange the following radical order of decreasing stability
