Calculate the dissociation constant of a $0.001 \ M$ weak monoacidic base undergoing $2 \%$ dissociation.
- A$4 \times 10^{-7}$
- B$2 \times 10^{-6}$
- C$2 \times 10^{-7}$
- D$1 \times 10^{-7}$
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The strongest Bronsted base among the following anions is:
MediumIIT 1981
View SolutionWhich of the following is the strongest conjugate base?
$H^{+}$ is a
Easy
View SolutionValues of dissociation constant,$K_a$ are given as follows:
Acid $K_a$ $HCN$ $6.2 \times 10^{-10}$ $HF$ $7.2 \times 10^{-4}$ $HNO_2$ $4.0 \times 10^{-4}$
Correct order of increasing base strength of the bases $CN^{-}$,$F^{-}$ and $NO_2^-$ will be:
| Acid | $K_a$ |
| $HCN$ | $6.2 \times 10^{-10}$ |
| $HF$ | $7.2 \times 10^{-4}$ |
| $HNO_2$ | $4.0 \times 10^{-4}$ |
Correct order of increasing base strength of the bases $CN^{-}$,$F^{-}$ and $NO_2^-$ will be:
DifficultJEE MAIN 2013
View SolutionConjugate acid of $NH_2^{-}$ and $NH_3$ are respectively
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