Ionic Equilibrium

Dissociation constant of 0.01 M weak acid is $10^{-4}$. What is percent dissociation of acid?

The solubility product of AgBr is $4.9 \times 10^{-13}$ at a certain temperature. Calculate the solubility.

Which among the following salts turns red litmus blue in its aqueous solution?

The solubility product of salt $\mathrm{B}_2 \mathrm{~A}$ is $3.2 \times 10^{-11}$ at 298 K . What is solubility of the salt at same temperature?

What is pH of weak dibasic acid, that is $2 \%$ dissociated in its M/100 solution at 298 K ?

The solubility product of the sparingly soluble salt $\mathrm{AB}_2$ is $2.56 \times 10^{-10}$ at 298 K . Calculate its solubility in $\mathrm{mol} \mathrm{dm}^{-3}$ at the same temperature?

Which among the following salts turns blue litmus red in its aqueous solution?

Calculate the value of dissociation constant of weak acid, which dissociates to $0.01 \%$ in its 0.1 M solution?

Which among the following salts forms basic solution when dissolved in water?

A monobasic weak acid dissociates $2 \%$ in its 0.002 M solution. Calculate the dissociation constant of weak acid.

Calculate the pH of centimolar solution of monoacidic weak base. Which is $10 \%$ dissociated in its aqueous solution?

A weak base is $5 \%$ dissociated in its 0.01 M solution. Calculate the dissociation constant.

Which among the following salts forms basic solution in water?

Solubility of binary sparingly soluble salt is $1.12 \times 10^{-4} \mathrm{~g} / \mathrm{dm}^3$. Calculate its solubility product (molar mass of salt $=112 \mathrm{~g} \mathrm{~mol}^{-1}$ )

Which amlong the following salts forms basic solution when dissolved in water?

Calculate the equilibrium concentration of $\mathrm{Pb}^{++}$ions in a solution of PbS containing $1 \times 10^{-11} \mathrm{~mol} \mathrm{dm}^{-3}$ of sulphide ions.
(Given $\mathrm{K}_{\mathrm{sp}}$ for $\mathrm{PbS}=8.0 \times 10^{-28}$ ...

The pH of monoacidic base is 10 . Calculate its percentage dissociation in 0.01 M solution at 298 K ?

Identify the conjugate acid-base pair respectively from following equilibrium reaction.
$$ \mathrm{HPO}_{4(\mathrm{aq})}^{2-}+\mathrm{H}_2 \mathrm{O}_{(\ell)} \rightleftharpoons \mathrm{PO}_{4(\mathrm{aq})}^{3-}+\mathrm{H}_3 \mathrm{O}_{(\m...

The solubility of sparingly soluble salt $\mathrm{AX}_2$ is $1 \times 10^{-4} \mathrm{~mol} \mathrm{dm}^{-3}$ at 298 K . Calculate its solubility product.

Calculate the value of dissociation constant of weak monoacidic base if it dissociates to $2 \%$ in 0.1 M solution?

Identify conjugate acid-base pair from following equilibrium reaction.
\(\mathrm{HSO}_{3(\mathrm{aq})}^{-}+\mathrm{H}_3 \mathrm{O}_{(\mathrm{aq})}^{+} \rightleftharpoons \mathrm{H}_2 \mathrm{SO}_3+\mathrm{H}_2 \mathrm{O}\)

The solubility product of NiS is $4.9 \times 10^{-5}$ at 298 K . Calculate its solubility in $\mathrm{mol} \mathrm{dm}^{-3}$ at the same temperature?

A weak monoacidic base dissociates to $1.5 \%$ in 0.001 M solution at 298 K . Calculate the dissociation constant of weak base.

The solubility product of $\mathrm{PbI}_2$ is $1.08 \times 10^{-7}$.
Calculate its solubility in $\mathrm{mol} \mathrm{dm}^{-3}$ at 298 K .

What is the value of pH of a NaOH solution that dissociates $2 \%$ in its 0.01 M solution?

Which from following formulae is used to find the $\left[\mathrm{OH}^{-}\right]$ion concentration of a weak monoacidic base?

The solubility of calcium carbonate at 298 K is $6.4 \times 10^{-5} \mathrm{~mol} \mathrm{dm}^{-3}$. Calculate the value of solubility product at the same temperature?

A monobasic weak acid dissociates to $1.2 \%$ in its 0.01 M solution at 298 K . Calculate dissociation constant of it.

Solubility of $\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$ is ' S ' $\mathrm{mol} \mathrm{dm}{ }^{-3}$. Find solubility product.

The solubility of AgBr is $7.1 \times 10^{-7} \mathrm{~mol} \mathrm{dm}^{-3}$. Calculate its solubility product at the same temperature.

What is the pH of buffer solution formed by mixing 0.01 M acetic acid and 0.05 M sodium acetate? $\left(\mathrm{pK}_{\mathrm{a}}=4.7447\right)$

The solubility of salt $\mathrm{BA}_2$ is $4 \times 10^{-4} \mathrm{~mol} \mathrm{dm}^{-3}$.
What is solubility product of the salt?

4 gram of NaOH is added in water to form 500 mL solution at 298 K . What is pH of solution? (Molar mass of $\mathrm{NaOH}=40 \mathrm{~g} \mathrm{~mol}^{-1}$ )

Which among the following salts turns red litmus blue in its aqueous solution?

The solubility product of a sparingly soluble salt AX is $4.9 \times 10^{-13}$. What is its solubility in $\mathrm{mol} \mathrm{dm}^{-3}$ ?

Which among the following salts is NOT hydrolysed in water?

The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it in $\mathrm{mol} \mathrm{dm}^{-3}$ ?

What is the value of $K_{s p}$ for saturated solution of $\mathrm{Ba}(\mathrm{OH})_2$ having pH 12 ?

If pH of solution changes from 4 to 5 , then the $\mathrm{H}_3 \mathrm{O}^{+}$ion concentration of solution

What is the pH of buffer solution prepared by mixing 0.01 M weak acid and 0.02 M salt of weak acid with strong base? $\left(\mathrm{pK}_{\mathrm{a}}=4.680\right)$

Which among the following is correct conjugate acid base pair for the equation stated below?
\(\mathrm{HCl}+\mathrm{NH}_3 \rightleftharpoons \mathrm{NH}_4^{+}+\mathrm{Cl}^{-}\)

Dissociation constant and degree of dissociation of weak acid are $1.8 \times 10^{-5}$ and 0.03 respectively. What will be the concentration of solution of weak acid?

Molar conductivity of 0.02 M weak acid is $7.92 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and its molar conductivity at infinite dilution is $232.7 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$.
Calculate degree of dissociation of wea...

What is the pOH of millimolar solution of $\mathrm{Ca}(\mathrm{OH})_2$ ?

Which from following buffers is used to maintain the pH of human blood naturally?

Calculate the pH of buffer solution containing 0.04 M NaF and $0.02 \mathrm{~M~HF}\left[\mathrm{pK}_a=3 \cdot 142\right]$.

Calculate the solubility of sparingly soluble salt BA in $\mathrm{mol} \mathrm{dm}^{-3}$ at 300 K if its solubility product is $4.9 \times 10^{-9}$ at same temperature.

Calculate the concentration of weak monobasic acid if its degree of dissociation and dissociation constant are $5.0 \times 10^{-4}$ and $5.0 \times 10^{-9}$ respectively.

Calculate the pH of a buffer solution containing 0.35 M weak acid and 0.70 M of its salt with strong base if $\mathrm{pK}_{\mathrm{a}}$ is 4.56 .

Which from following mixtures in water acts as a basic buffer?