The ionization constant of $CH_3COOH$ is $1.7 \times 10^{-5}$. In a certain solution of acetic acid,the concentration of $H^+$ is $3.4 \times 10^{-4} \ M$. The concentration of the acetic acid solution is ............ .
- A$3.4 \times 10^{-4} \ M$
- B$3.4 \times 10^{-3} \ M$
- C$6.8 \times 10^{-4} \ M$
- D$6.8 \times 10^{-3} \ M$
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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,$CO(NH_{2})_{2}$ | $1.3 \times 10^{-14}$ |
Medium
View Solution$A$ weak monoacidic base is $1.2 \%$ dissociated in its $0.2 \ M$ solution. What is the value of dissociation constant?
Degree of dissociation is $10\%$ for $10^{-3} \ M$ solution of $H_2CO_3$. Then,the $pH$ of the solution is:
Medium
View SolutionWhat is the molar concentration of a weak monobasic acid if its dissociation constant is $5 \times 10^{-8}$ and it undergoes $0.5 \%$ dissociation (in $M$)?
Calculate the molar concentration of a weak monobasic acid if the acid dissociation constant $K_a = 1.8 \times 10^{-5}$ and the degree of dissociation $\alpha = 0.01$.
DifficultMHT CET 2026
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