Write the conjugate acids for the following Bronsted bases: $NH_{2}^{-}$,$NH_{3}$ and $HCOO^{-}$.
The conjugate acid of a Bronsted base is formed by adding a proton $(H^{+})$ to the base. The table below lists the conjugate acids for the given Bronsted bases:
| Bronsted base | Conjugate acid |
| $NH_{2}^{-}$ | $NH_{3}$ |
| $NH_{3}$ | $NH_{4}^{+}$ |
| $HCOO^{-}$ | $HCOOH$ |
Explore More
Similar Questions
For the species $HSO_4^{-}$ and $NH_3$,their conjugate acids respectively are
Non-metallic oxides dissolve in water to form
Medium
View SolutionWhich of the following is a Lewis acid?
Easy
View SolutionThe Bronsted acids in the reversible reaction are $HCO_3^- (aq) + OH^- (aq) \rightleftharpoons CO_3^{2-} (aq) + H_2O (l)$
Medium
View SolutionIdentify the acids in the following reaction: $HCl_{(aq)} + H_2O_{(aq)} \rightleftharpoons H_3O^{+}_{(aq)} + Cl^{-}_{(aq)}$. Which of these acids is stronger?
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo