A solution is prepared by dissolving $0.01$ moles of $NH_4Cl$ and $0.1$ moles of $NH_3$ in $1$ L of water. If the $K_b$ for $NH_3$ is $1.8 imes 10^{-5}$, what is the approximate pH of the solution?

Which species are formed when $H_2O$ and $HF$ act as Bronsted acids?

In ${\rm{H}}{{\rm{S}}^ - },{{\rm{I}}^ - },{\rm{R}} - {\rm{N}}{{\rm{H}}_2},{\rm{N}}{{\rm{H}}_3}$ order of proton accepting tendency will be:

Which of the following species can act as both a Brønsted-Lowry acid and a Lewis base?

If water ($H_2O$) acts as a Bronsted acid, what is its conjugate base? If hydrogen fluoride ($HF$) acts as a Bronsted acid, what is its conjugate base?

Which among the following is the strongest acid?

Which theory defines a base as a proton acceptor?

Conjugate acid-base pair differs by a/an:

Which of these is a Lewis acid?

In water, the acid ${\rm{HCl}}{{\rm{O}}_4},{\rm{HCl}},{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}\;and\;{\rm{HN}}{{\rm{O}}_3}$ exhibit the same strength as they are completely ionised in water (a base). This is called … of the solvent water.

Which of the following is not a Lewis acid?