If $1 \ mM$ solution of ethylamine produces $pH = 9$,then the ionization constant $(K_b)$ of ethylamine is $10^{-x}$. The value of $x$ is . . . . . . (nearest integer). [The degree of ionization of ethylamine can be neglected with respect to unity.]
- A$7$
- B$8$
- C$9$
- D$10$
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What is the $pH$ of $0.001 \,M$ aniline solution? The ionization constant of aniline can be taken from the 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,$(CH_{3})_{2}NH$ $5.4 \times 10^{-4}$ Triethylamine,$(C_{2}H_{5})_{3}N$ $6.45 \times 10^{-5}$ Ammonia,$NH_{3}$ $1.77 \times 10^{-5}$ Quinine $1.10 \times 10^{-6}$ Pyridine,$C_{5}H_{5}N$ $1.77 \times 10^{-9}$ Aniline,$C_{6}H_{5}NH_{2}$ $4.27 \times 10^{-10}$ Urea,$CO(NH_{2})_{2}$ $1.3 \times 10^{-14}$
| Base | $K_{b}$ |
| Dimethylamine,$(CH_{3})_{2}NH$ | $5.4 \times 10^{-4}$ |
| Triethylamine,$(C_{2}H_{5})_{3}N$ | $6.45 \times 10^{-5}$ |
| Ammonia,$NH_{3}$ | $1.77 \times 10^{-5}$ |
| Quinine | $1.10 \times 10^{-6}$ |
| Pyridine,$C_{5}H_{5}N$ | $1.77 \times 10^{-9}$ |
| Aniline,$C_{6}H_{5}NH_{2}$ | $4.27 \times 10^{-10}$ |
| Urea,$CO(NH_{2})_{2}$ | $1.3 \times 10^{-14}$ |
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View SolutionAt $25 \, ^\circ C$,the dissociation constant of a base $BOH$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in $0.01 \, M$ aqueous solution of the base would be:
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View SolutionThe hydrogen ion concentration of a $0.006 \ M$ benzoic acid solution is $(K_a = 6 \times 10^{-5})$
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