For each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base.
(a) \(\mathrm{HI}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q)+l^{-}(a q)\)
(b) \(\mathrm{CH}_{3} \mathrm{NH}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{CH}_{3} \mathrm{NH}_{3}^{+}(a q)+\mathrm{OH}^{-}(a q)\)
(c) \(\mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q)\)
.
(d) \(\mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{HCO}_{3}^{-}(a q)\)
Equation Transcription:
⇌
⇌
.
⇌
Text Transcription:
HI(aq)+H_2O(l) rightarrow H_3O^+(aq)+l^-(aq)
CH_3NH_2(aq)+H_2O(l) ⇌ CH_3NH_3+(aq)+OH^-(aq)
CO_3^2-(aq)+H_2O(l) ⇌ HCO_3^-(aq)+OH^-(aq)
.
H_2CO_3(aq)+H_2O(l) ⇌ H_3O^+(aq)+HCO_3^-(aq)
Problem 32P
For each reaction, identify the Bransted-Lowry add, the Bransted-Lowry base, the conjugate acid, and the conjugate base.
(a)
(b)
(c)
(d)
Step by Step Solution
Step 1 of 4
Bronsted-lowry definition of acid-base is as it applies to a wider range of acid-base phenomena. This definition focuses on the transfer of ions in an acid-base reaction. therefore , according to bronsted-lowry an acid is a proton donor (
) and a base is a proton acceptor(
). The substance that results after acid donates a proton is the conjugate base of that acid and the substance that results after the base accepts a proton is conjugate acid of that base.
(a).
The given reaction is as follows:
Now will identify the Bronsted-lowry acid, Bronsted-lowry base, conjugate acid and conjugate base in the given equation.
Bronsted-lowry acid =
Bronsted-lowry base =
Conjugate base =
Conjugate acid =