Ionization of Weak Acids and Weak Bases

A weak mono acidic base is $5\%$ ionised in $0.1 \mathrm{M}$ solution. Find the concentration of hydroxide ions.

A monoprotic acid in a $0.1 \mathrm{M}$ solution ionises to $0.01\%$. Find its ionisation constant.

The acidic stregth of an acid does not depends on the polarity of the bond.

According to the polarity of the bond, the strongest acid will be

What is the role of solvent in acidic strength?

What is the role of polarity in acidic strength of an acid?

Arrange the following acids in the increasing order of their acidic strength.

$\mathrm{HF}, \mathrm{HCl}, \mathrm{HBr}, \mathrm{HI}$

Which of the following acid has the highest acidic strength.

The greater the strength of $\mathrm{H}-\mathrm{A}$ bond, the greater the acidic strength.

On increasing the bond strength of an acid, the acidic strength _____.

How does the bond strength affect the acidic strength.

The $\mathrm{pH}$ of $0.1 \mathrm{M}$ acetic acid solution is closest to [Dissociation constant of the acid, ${\mathrm{K}}_{\mathrm{a}}=1.8\times {10}^{-5}$]

Which of the following equation follows for base ionization constant is expressed in terms of concentration in molarity of various species in equilibrium.

Calculate the concentration of ${\mathrm{A}}^{-}$ ions in the solution of $0.01 \mathrm{M} \mathrm{HA}$.

$\left[{\mathrm{K}}_{\mathrm{a}}=4\times {10}^{-10}\right]$

Ionisation constant of  ${\mathrm{CH}}_3\mathrm{COOH}$ is $1.7\times {10}^{-5}$ and concentration of ${\mathrm{H}}^{+}$ ions is $3.4\times {10}^{-4}$. Then, the initial concentration of ${\mathrm{CH}}_3\mathrm{COOH}$ is 

Which of the following will occur if a $0.1 \mathrm{M}$ solution of a weak acid is diluted to $0.01 \mathrm{M}$ at constant temperature?

The ${\mathrm{K}}_{\mathrm{a}}$ values of formic acid and acetic acid are respectively $1.77\times {10}^{-4}$ and $1.75\times {10}^{-5}$. The ratio of acid strength of $0.1 \mathrm{N}$ acids is

Which of the following is a weak alkali?

The $\mathrm{pH}$ of an aqueous solution of ${10}^{-8}\mathrm{MHCl}$ is

${\mathrm{NH}}_3$ is dissolved in water.

${\mathrm{NH}}_3 + {\mathrm{H}}_2\mathrm{O} \leftrightharpoons {{\mathrm{NH}}_4}^{+}+{\mathrm{OH}}^{-}$

Its base dissociation constant is given by: