Write the conjugate acids for the following Bronsted bases: $NH_{2}^{-}$,$NH_{3}$ and $HCOO^{-}$
- A$NH_{3}$,$NH_{4}^{+}$,$HCOOH$
- B$NH_{3}$,$NH_{4}^{+}$,$HCOO^{-}$
- C$NH_{2}$,$NH_{4}^{+}$,$HCOOH$
- D$NH_{3}$,$NH_{4}^{+}$,$HCOO_{2}^{-}$
Explore More
Similar Questions
The ionization constants of $HF$,$HCOOH$,and $HCN$ at $298 \ K$ are $6.8 \times 10^{-4}$,$1.8 \times 10^{-4}$,and $4.8 \times 10^{-9}$ respectively. Calculate the ionization constants of their corresponding conjugate bases.
Medium
View SolutionWhich one of the following can be classified as a Bronsted base?
Easy
View SolutionWould gaseous $HCl$ be considered as an Arrhenius acid?
Easy
View SolutionMatch the given ionisation constant values with the corresponding acids.
$A$. $HI$ $(i)$ $3.2 \times 10^9$ $B$. $HF$ $(ii)$ $3.5 \times 10^{-4}$ $C$. $HCl$ $(iii)$ $1.3 \times 10^6$ $D$. $HBr$ $(iv)$ $1.0 \times 10^9$
The correct match is:
| $A$. $HI$ | $(i)$ $3.2 \times 10^9$ |
| $B$. $HF$ | $(ii)$ $3.5 \times 10^{-4}$ |
| $C$. $HCl$ | $(iii)$ $1.3 \times 10^6$ |
| $D$. $HBr$ | $(iv)$ $1.0 \times 10^9$ |
The correct match is:
The dissociation constant of a weak acid is $1.0 \times 10^{-5}$. The equilibrium constant for its reaction with a strong base is:
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