A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
$1$
$2$
$3$
$11$
Degree of dissociation is $10\%$ for $10^{-3}\, M$ solution of $H_2CO_3$ then $pH$ of solution is
The $pH$ of the solution obtained on neutralisation of $40\, mL\, 0.1\, M\, NaOH$ with $40\, mL\, 0.1\, M\, CH_3COOH$ is
For a concentrated solution of a weak electrolyte ( $K _{ eq }=$ equilibrium constant) $A _2 B _3$ of concentration ' $c$ ', the degree of dissociation " $\alpha$ ' is
$p{K_a}$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1\,\,M$ sodium acetate solution will be
Write characteristics and uses of ${K_a}$ value.