Concentration $C{N^ - }$ in $0.1\,M\,HCN$ is $[{K_a} = 4 \times {10^{ - 10}}]$
$2.5 \times {10^{ - 6}}M$
$4.5 \times {10^{ - 6}}M$
$6.3 \times {10^{ - 6}}M$
$9.2 \times {10^{ - 6}}M$
Which of the following base is weakest
Explain a general step-wise approach to evaluate the $pH$ of the weak electrolyte.
Derive the equation of ionization constant $({K_b})$ of weak base.
The degree of ionization of a $0.1 \,M$ bromoacetic acid solution is $0.132$ Calculate the $pH$ of the solution and the $p K_{ a }$ of bromoacetic acid.
Determine the degree of ionization and $pH$ of a $0.05 \,M$ of ammonia solution. The ionization constant of ammonia can be taken from Table $7.7 .$ Also, calculate the ionization constant of the conjugate acid of ammonia.