A solution of weak acid $HA$ containing $0.01$ moles of acid per litre of solutions has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.
$1\% ,\,{10^{ - 6}}$
$0.01\% ,\,{10^{ - 4}}$
$1\% ,\,{10^{ - 4}}$
$0.01\% ,\,{10^{ - 6}}$
$2\, gm$ acetic acid and $3\, gm$ sodium acetate are present in $100\, ml$. aqueous solution then what will be the $pH$ of solution if ionisation constant of acetic acid is $1.8 \times 10^{-5}$
The ionization constant of acetic acid is $1.74 \times 10^{-5}$. Calculate the degree of dissociation of acetic acid in its $0.05\, M$ solution. Calculate the concentration of acetate ion in the solution and its $pH$.
$5\%$ ionization is occur in $0.01$ $M$ $C{H_3}COOH$ solution. Calculate its dissociation constant.
The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is
Explain a general step-wise approach to evaluate the $pH$ of the weak electrolyte.