A weak acid is $ 0.1\% $ ionised in $0.1\, M $ solution. Its $pH$ is
$2$
$3$
$4$
$1$
The $pH$ of $0.004 \,M$ hydrazine solution is $9.7 .$ Calculate its ionization constant $K_{ b }$ and $pK _{ b }$
Find $pH$ of $5 \times 10^{-3}\, M$ $H_2CO_3$ solution having $10\%$ dissociation
Sulphurous acid $\left( H _{2} SO _{3}\right)$ has $Ka _{1}=1.7 \times 10^{-2}$ and $Ka _{2}=6.4 \times 10^{-8} .$ The $pH$ of $0.588 \,M\, H _{2} SO _{3}$ is ..... . (Round off to the Nearest Integer)
The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is
What is the $pH$ of $0.1\,M\,N{H_3}$