Which of the following base is weakest
$N{H_4}OH:{K_b} = 1.6 \times {10^{ - 6}}$
${C_6}{H_5}N{H_2}:{K_b} = 3.8 \times {10^{ - 10}}$
${C_2}{H_5}N{H_2}:{K_b} = 5.6 \times {10^{ - 4}}$
${C_6}{H_7}N:{K_b} = 6.3 \times {10^{ - 10}}$
A certain amount of $H_2CO_3$ & $HCl$ are dissolved to form $1$ litre solution. At equilibrium it is found that concentration of $H_2CO_3$ & $CO_3^{-\,-}$ are $0.1\,M$ & $0.01\,M$ respectively. Calculate the $pH$ of solution. Given that for $H_2CO_3$ $K_{a_1} =10^{-5}$ & $K_{a_2} =10^{-8}$
The $pH$ of the solution obtained on neutralisation of $40\, mL\, 0.1\, M\, NaOH$ with $40\, mL\, 0.1\, M\, CH_3COOH$ is
What is the percent ionization $(\alpha)$ of a $0.01\, M\, HA$ solution ? .......$\%$ $(K_a = 10^{-6})$
$HClO$ is a weak acid. The concentration of ${H^ + }$ ions in $0.1\,M$ solution of $HClO\,({K_a} = 5 \times {10^{ - 8}})$ will be equal to
$2\, gm$ 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 $1.8 \times 10^{-5}$