The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by
$
\left[ H ^{+}\right]= K _{ a } \frac{[ acid ]}{[\text { salt }]}
$
$
\left.\left[ H ^{+}\right]= K _{ a } \text { [salt }\right]
$
$
\left[ H ^{+}\right]= K _{ a } \text { [acid] }
$
$
\left[ H ^{+}\right]= K _{ a } \frac{[\text { salt }]}{[\text { acid }]}
$
The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by $\left[ H ^{+}\right]= K _{ a } \frac{[\text { acid }]}{[\text { salt }]}$.
Explanation:
According to Henderson equation
$
\begin{aligned}
& pH = pK _{ a }+\log \frac{[\text { salt }]}{[\text { acid }]} \\
& \text { i.e., }-\log \left[ H ^{+}\right]=-\log K _{ a }+\log \frac{[\text { salt }]}{[\text { acid }]} \\
& -\log \left[ H ^{+}\right]=\log \frac{[\text { salt }]}{[\text { acid }]} \times \frac{1}{ K _{ a }} \\
& \log \frac{1}{\left[ H ^{+}\right]}=\log \frac{[\text { salt }]}{[\text { acid }]} \times \frac{1}{ K _{ a }} \\
& \therefore\left[ H ^{+}\right]= K _{ a } \frac{[\text { acid }]}{[\text { salt }]}
\end{aligned}
$
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.