Ionization of Weak Acids and Weak Bases

A weak monoprotic acid is $0.04\%$ dissociated in $0.01\mathrm{M}$ solution. calculate dissociation constant of the acid?

Among the given pairs, which pair shows common ion effect?

${\mathrm{K}}_{\mathrm{a}}$ of ${\mathrm{H}}_2{\mathrm{O}}_2$ is in the order of 

A weak monobasic acid is $12\%$ ionized in $0.05 \mathrm{M}$ solution. The percentage of ionization in its $0.15 \mathrm{M}$ solution is

Suppose that pH of monobasic and dibasic acid is the same. Does this mean that the molar concentrations of both acids are identical ?

Which of the following is not an example of common ion effect?

A gas ${\mathrm{AB}}_3$ present in $10 \mathrm{lit}$ container at pressure $2.5 \mathrm{atm}$ and $273 \mathrm{K}$ temperature. On increasing the temperature to $546 \mathrm{K}$, ${\mathrm{AB}}_3$ dissociates into ${\mathrm{AB}}_2\left(\mathrm{g}\right)$ and ${\mathrm{B}}_2\left(\mathrm{g}\right)$. If the degree of dissociation of ${\mathrm{AB}}_3$ is $0.8$ then the final pressure at $546 \mathrm{K}$ is

If the concentration of ${\mathrm{OH}}^{-}$ ions is the reaction $\mathrm{Fe}{\left(\mathrm{OH}\right)}_3\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+3{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)$, is decreased by $\frac{1}{3}$ times, then equilibrium concentration of ${\mathrm{Fe}}^{3+}$ will increase by:

Write the relationship between ${\mathrm{K}}_{\mathrm{a}}$ and ${\mathrm{K}}_{\mathrm{b}}$ of conjugate acid-base pair at $298 \mathrm{K}$.

The concentration of ${\mathrm{S}}^{2-}$ in $0.1\mathrm{M}$ ${\mathrm{H}}_2 \mathrm{S}\left({\mathrm{Ka}}_1 {\mathrm{Ka}}_2=1.1\times {10}^{-21}{\mathrm{M}}^2\right)$ containing $0.1\mathrm{M} {\mathrm{H}}^{+}$ ion is $1.1\times {10}^{-\mathrm{y}}$. Calculate the value of $\mathrm{y}$.

Explain the reason for the smaller value of higher order ionization constants than the lower order ionization constant of polyacidic bases.

Define polyacidic bases and give some examples.

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?

Define the degree of dissociation of electrolytes.

What is common ion effect? Write an example.

${\mathrm{NH}}_3$ 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: