The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is
$3:5$
$5:3$
$100:1$
$1:100$
The dissociation constant of a substituted benzoic acid at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-4}$. The $\mathrm{pH}$ of a $0.01 \ \mathrm{M}$ solution of its sodium salt is
Accumulation of lactic acid $(HC_3H_5O_3),$ a monobasic acid in tissues leads to pain and a feeling of fatigue. In a $0.10\, M$ aqueous solution, lactic acid is $3.7\%$ dissociates. The value of dissociation constant, $K_a,$ for this acid will be
The $pH$ of a $0.1\ M$ aqueous solution of a very weak acid $(HA)$ is $3$. What is its degree of dissociation ?......$\%$
The $pH$ of $0.004 \,M$ hydrazine solution is $9.7 .$ Calculate its ionization constant $K_{ b }$ and $pK _{ b }$
Which of the following will occur if a $0.1 \,M$ solution of a weak acid is diluted to $0.01\,M$ at constant temperature