Which of the following is the strongest conjugate base?
- A$Cl^{-}$
- B$F^{-}$
- C$Br^{-}$
- D$I^{-}$
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Similar Questions
Give the conjugate acid and conjugate base of the following:
$(i)$ $(CH_3)_2NH$
$(ii)$ $HPO_4^{2-}$
$(iii)$ $HS^{-}$
$(i)$ $(CH_3)_2NH$
$(ii)$ $HPO_4^{2-}$
$(iii)$ $HS^{-}$
Medium
View SolutionThe conjugate base of the bicarbonate ion $(HCO_3^-)$ is:
Easy
View Solution$A$ base is dissolved in water to yield a solution with a hydroxide ion concentration of $0.05 \ mol \ L^{-1}$. The solution is
Difficult
View SolutionAccording to the Bronsted-Lowry theory,the acids in the following reaction are:
$ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$
$ClO_4^{-} + HCO_3^{-} \rightarrow HClO_4 + CO_3^{2-}$
The conjugate bases for $HCO_3^-$ and $NH_3$,respectively,are
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