A $0.1\, M$ solution of $HF$ is $1\%$ ionized. What is the $K_a$
${10^{ - 5}}$
${10^{ - 4}}$
$3 \times {10^{ - 5}}$
$3 \times {10^{ - 4}}$
What is the $ pH$ of $0.01\, M$ glycine solution? For glycine, $K{a_1} = 4.5 \times {10^{ - 3}}$ and $K{a_2} = 1.7 \times {10^{ - 10}}$ at $298 \,K$
$2\, gm$ 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 $1.8 \times 10^{-5}$
${K_{C{H_3}COOH}} = 1.9 \times {10^{ - 5}}$. Calculate $pH$ at end point in titration of $0.1$ $M$ $C{H_3}COOH$ and $0.1$ $M$ $NaOH$.
What is the $pH$ of $0.001 \,M$ aniline solution? The ionization constant of aniline can be taken from Table . Calculate the degree of ionization of aniline in the solution. Also calculate the ionization constant of the conjugate acid of aniline.
Base | $K _{ b }$ |
Dimethylamine, $\left( CH _{3}\right)_{2} NH$ | $5.4 \times 10^{-4}$ |
Triethylamine, $\left( C _{2} H _{5}\right)_{3} N$ | $6.45 \times 10^{-5}$ |
Ammonia, $NH _{3}$ or $NH _{4} OH$ | $1.77 \times 10^{-5}$ |
Quinine, ( $A$ plant product) | $1.10 \times 10^{-6}$ |
Pyridine, $C _{5} H _{5} N$ | $1.77 \times 10^{-9}$ |
Aniline, $C _{6} H _{5} NH _{2}$ | $4.27 \times 10^{-10}$ |
Urea, $CO \left( NH _{2}\right)_{2}$ | $1.3 \times 10^{-14}$ |
Derive ${K_w} = {K_a} \times {K_b}$ and ${K_w} = p{K_a} \times p{K_b}$ for weak base $B$ and its conjugate acid ${B{H^ + }}$.