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6-2.Equilibrium-II (Ionic Equilibrium)
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A weak base $MOH$ of $0.1\, N$ concentration shows a $pH$ value of $9$. What is the percentage degree of ionisation of the base ? ......$\%$
A
$0.01$
B
$0.001$
C
$0.1$
D
$0.02$
Solution
$\mathrm{pOH}=5$
$\mathrm{OH}^{-}=10^{-5}$
$\mathrm{OH}=\mathrm{C} \alpha$
$\alpha=\frac{10^{-5}}{10^{-1}}=10^{-4} ; \alpha(\text { in } \%)=10^{-2}$
Standard 11
Chemistry
Similar Questions
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, $CO \left( NH _{2}\right)_{2}$ | $1.3 \times 10^{-14}$ |
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