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6-2.Equilibrium-II (Ionic Equilibrium)
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Calculate the ${H^ + }$ ion concentration in a $1.00\,(M)$ $\,HCN\,$ litre solution $({K_a} = 4 \times {10^{ - 10}})$
A
$4 \times {10^{ - 14}}\,mole/litre$
B
$2 \times {10^{ - 5}}\,mole/litre$
C
$2.5 \times {10^{ - 5}}\,mole/litre$
D
None of these
Solution
(b) $[{H^ + }] = \sqrt {K \times C} $
$[{H^ + }] = \sqrt {4 \times {{10}^{ – 10}} \times 1} $ ; $[{H^ + }] = 2 \times {10^{ – 5}}$ $mole/litre$
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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