Identify the conjugate base in the following reaction: $H_2SO_4 + H_2O \rightleftharpoons H_3O^{+} + HSO_4^-$
- A$H_2O$
- B$HSO_4^-$
- C$H_3O^{+}$
- D$SO_2$
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Similar Questions
Considering the following reactions,which pair of reactions shows that water has basic properties?
$(i) \ CO_2 + H_2O \rightleftharpoons H_2CO_3$
$(ii) \ NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^-$
$(iii) \ HCl + H_2O \rightleftharpoons Cl^- + H_3O^+$
$(i) \ CO_2 + H_2O \rightleftharpoons H_2CO_3$
$(ii) \ NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^-$
$(iii) \ HCl + H_2O \rightleftharpoons Cl^- + H_3O^+$
Easy
View SolutionIn the following reaction $HCO_3^{-} + H_2O \rightleftharpoons CO_3^{2-} + H_3O^{+}$,which two substances are Bronsted bases?
Easy
View SolutionWhich of the following is not a Bronsted acid?
Easy
View SolutionWhich among the following is a correct conjugate acid-base pair for the equation stated below?
$HCl + NH_3 \rightleftharpoons NH_4^{+} + Cl^{-}$
$HCl + NH_3 \rightleftharpoons NH_4^{+} + Cl^{-}$
Consider the following data for a series of hydrogen halide Bronsted acids:-
Acid $HF$ $HCl$ $HBr$ $HI$ $K_a$ $7.2 \times 10^{-4}$ $1 \times 10^6$ $1 \times 10^9$ $3 \times 10^{11}$
Which of these Bronsted acids would have the weakest conjugate base?
| Acid | $HF$ | $HCl$ | $HBr$ | $HI$ |
| $K_a$ | $7.2 \times 10^{-4}$ | $1 \times 10^6$ | $1 \times 10^9$ | $3 \times 10^{11}$ |
Which of these Bronsted acids would have the weakest conjugate base?
Medium
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