Which of the following cannot act both as Bronsted acid and as Bronsted base?
- A$HCO_3^-$
- B$NH_3$
- C$HCl$
- D$HSO_4^-$
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Which statement about the following equilibrium is true?
$(CH_3)_3CO^-K^+ + H_2O \rightleftharpoons (CH_3)_3COH + K^+OH^-$
Given: $pK_a(H_2O) = 15.7$,$pK_a((CH_3)_3COH) = 18$
$(CH_3)_3CO^-K^+ + H_2O \rightleftharpoons (CH_3)_3COH + K^+OH^-$
Given: $pK_a(H_2O) = 15.7$,$pK_a((CH_3)_3COH) = 18$
Medium
View SolutionWhat is a Lewis acid?
Easy
View SolutionThe conjugate bases for $HCO_3^-$ and $NH_3$,respectively,are
Identify the conjugate acid-base pair in the following reaction.
$H_2O + HCl \rightarrow H_3O^{+} + Cl^{-}$
$H_2O + HCl \rightarrow H_3O^{+} + Cl^{-}$
The number of species among the following that can act both as Bronsted acids and bases is $HCl, ClO_4^{-}, OH^{-}, H^{+}, H_2O, HSO_4^{-}, SO_4^{2-}, H_2SO_4, Cl^{-}$.
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