Ionic Equilibrium · Chemistry · MHT CET

Identify conjugate acid and conjugate base for $\mathrm{HCO}_3^{-}$ion respectively

Find the concentration of sodium acetate when added to 0.1 M solution of acetic acid to form a buffer solution of $\mathrm{pH}=5.5$ ?

( $\mathrm{pK}_{\mathrm{a}}$ of $\mathrm{CH}_3 \mathrm{COOH}=4.5$ )

Calculate the ionisation constant of $0.08 \mathrm{~mol} \mathrm{dm}{ }^{-3}$ of a monobasic acid having $\mathrm{pH}=2$.

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?

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

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

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

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

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

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

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

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

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?

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

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

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 $\mathrm{PbS}=8.0 \times 10^{-28}$ )

Which among the following salts forms basic solution in water?

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

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 $=112 \mathrm{~g} \mathrm{~mol}^{-1}$ )

Identify conjugate acid-base pair from following equilibrium reaction.

$$ \mathrm{HSO}_{3(\mathrm{aq})}^{-}+\mathrm{H}_3 \mathrm{O}_{(\mathrm{aq})}^{+} \rightleftharpoons \mathrm{H}_2 \mathrm{SO}_3+\mathrm{H}_2 \mathrm{O} $$

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

Identify the conjugate acid-base pair respectively from following equilibrium reaction.

$$ \mathrm{HPO}_{4(\mathrm{aq})}^{2-}+\mathrm{H}_2 \mathrm{O}_{(\ell)} \rightleftharpoons \mathrm{PO}_{4(\mathrm{aq})}^{3-}+\mathrm{H}_3 \mathrm{O}_{(\mathrm{eq})}^{+} $$

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?

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

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

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?

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

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

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

What is solubility product of the salt?

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? $\left(\mathrm{pK}_{\mathrm{a}}=4.7447\right)$

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

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? $\left(\mathrm{pK}_{\mathrm{a}}=4.680\right)$

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

Which from following substances acts as a base when reacted with water?

Calculate the pH of 0.02 M monobasic acid having $2 \%$ dissociation.

Calculate the solubility product of sparingly soluble salt BA at $27^{\circ} \mathrm{C}$ if its solubility is $1.8 \times 10^{-5} \mathrm{~mol} \mathrm{dm}^{-3}$ at same temperature.

Calculate the pH of 0.01 M sulphuric acid.

Which from following mixtures in water acts as a buffer?

Calculate the solubility in $\mathrm{mol} \mathrm{dm}^{-3}$ of sparingly soluble salt BA if its solubility product $4.9 \times 10^{-13}$ at same temperature.

An aqueous solution of strong monoacidic base is of $1 \times 10^{-4} \mathrm{M}$. What is the value of pH at $25^{\circ} \mathrm{C}$ ?

Acidic buffer solution is prepared by mixing proportionate quantity of

The degree of dissociation of 0.01 M solution of $\mathrm{NH}_4 \mathrm{OH}$ is $4.2 \times 10^{-2}$. What is the percent dissociation of $\mathrm{NH}_4 \mathrm{OH}$ ?

Conjugate acid of $\mathrm{NH}_2^{-}$and $\mathrm{NH}_3$ are respectively

A buffer solution is prepared by mixing $0.2 \mathrm{~M} \mathrm{~NH} \mathrm{O}_4 \mathrm{OH}$ and $1 \mathrm{~M} \mathrm{~NH}_4 \mathrm{Cl}$. What is the pH value of buffer solution? $\left(\right.$ Give $\left.\mathrm{pK}_{\mathrm{b}}=7.744\right)$

The dissociation constant of a weak monobasic acid is $3.2 \times 10^{-4}$. Calculate the degree of dissociation in its 0.04 M solution.

The solubility of $\mathrm{CaCO}_3$ is $7 \times 10^{-5} \mathrm{~mol} \mathrm{dm}^{-3}$ at $25^{\circ} \mathrm{C}$. What is its solubility product at same temperature?

Which among the following is the conjugate base of $\mathrm{HClO}_4$ ?

What is pH of a centimolar solution of $\mathrm{H}_2 \mathrm{SO}_4$ ?

A buffer solution is prepared by mixing 0.01 M HCN and 0.02 MNaCN . If $\mathrm{K}_{\mathrm{a}}$ for HCN is $6.6 \times 10^{-10}$, what is the concentration of $\mathrm{H}^{+}$ions in solution?

A monobasic acid is $5 \%$ dissociated in its 0.02 M solution. Calculate the dissociation constant of acid.

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

Calculate dissociation constant of a weak monobasic acid if it is $0.05 \%$ dissociated in 0.02 M solution.

A buffer solution contains equal concentrations of weak acid and its salt with strong base. Calculate pH of buffer solution if dissociation constant of weak acid is $1.8 \times 10^{-5}$.

Which from the following equations represents the relation between solubility ( $\mathrm{mol} \mathrm{~L}^{-1}$ ) and solubility product for a salt $\mathrm{B}_3 \mathrm{A}_2$ ?

Calculate solubility $\left(\mathrm{moldm}^{-3}\right)$ of a sparingly soluble electrolyte AB at 298 K if its solubility product is $1.6 \times 10^{-5}$ ?

What is the pH of $10^{-8} \mathrm{M~HCl}$ solution?

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

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

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

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 weak acid.

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?

Which from following salts is NOT derived from weak acid and weak base?

Calculate the solubility product of sparingly soluble salt BA at $25^{\circ} \mathrm{C}$ if its solubility is $7.2 \times 10^{-7} \mathrm{~mol} \mathrm{~dm}^{-3}$ at same temperature.

Calculate the $[\mathrm{OH}]$ if pOH of solution is 4.94

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

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 .

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 pH of 0.002 M KOH solution.

Calculate ' $\alpha$ ' for 0.1 M acetic acid $\left(\mathrm{K}_{\mathrm{a}}=1.0 \times 10^{-5}\right)$

Calculate $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$in 0.02 M solution of monobasic acid if dissociation constant is $1.8 \times 10^{-5}$.

Which of the following equations represents the relation between solubility and solubility product for salt BA$_3$?

Calculate the pH of buffer solution containing 0.027 M weak acid and 0.054 M of its salt with strong base if $\mathrm{pK}_{\mathrm{a}}$ is 4.2.

Calculate $\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$ of a monobasic acid if it is $0.04 \%$ dissociated in 0.05 M solution.

Calculate the solubility product of sparingly soluble salt BA at 300 K if its solubility is $9.1 \times 10^{-3} \mathrm{moldm}^{-3}$ at same temperature.

Which from following species acts as base ${ }^1$, according to Bronsted-Lowry theory?

$$\mathrm{HCl}+\mathrm{NH}_3 \text { 目的 } \mathrm{NH}_4^{+}+\mathrm{Cl}^{-} $$

What is the ratio of concentration of salt to concentration of weak acid in buffer solution to maintain its pH value $7.2\left(\mathrm{pK}_{\mathrm{a}}=6.2\right)$.

What is the value of pOH if a buffer solution is prepared by mixing equal volumes of $0.4 \mathrm{~M} \mathrm{~NH}_4 \mathrm{OH}$ and $0.5 \mathrm{~M} \mathrm{~NH}_4 \mathrm{Cl}$ solutions. $\left(\mathrm{pK}_{\mathrm{b}}=4.730\right)$

Which of the following salt solutions turns red litmus blue?

The solubility product of $$\mathrm{PbCl}_2$$ at $$298 \mathrm{~K}$$ is $$3.2 \times 10^{-5}$$. What is its solubility in $$\mathrm{mol} \mathrm{dm}{ }^{-3}$$ ?

Identify base$$_2$$ for following equation according to Bronsted-Lowry theory.

$$\mathrm{HCl}_{(\mathrm{aq})}+\mathrm{H}_2 \mathrm{O}_{(l)} \rightleftharpoons \mathrm{H}_3 \mathrm{O}_{(\mathrm{aq})}^{+}+\mathrm{Cl}_{(\mathrm{aq})}^{-}$$

An organic monobasic acid has dissociation constant $$2.25 \times 10^{-6}$$. What is percent dissociation in its $$0.01 \mathrm{~M}$$ solution?

Calculate the $$\mathrm{pH}$$ of $$0.01 \mathrm{~M}$$ strong dibasic acid.

Calculate dissociation constant of $$0.001 \mathrm{M}$$ weak monoacidic base undergoing $$2 \%$$ dissociation.

What is the $$\mathrm{pH}$$ of solution containing $$4.62 \times 10^{-4} \mathrm{M} \mathrm{H}^{+}$$ ions?

Which among the following salt solution in water is acidic in nature?

What is the molar concentration of acetic acid if value of it's, dissociation constant is $$1.8 \times 10^{-5}$$ and degree of dissociation is 0.02 ?

A buffer solution is prepared by mixing equimolar acetic acid and sodium acetate. If '$$\mathrm{K}_d$$' of acetic acid is $$1.78 \times 10^{-5}$$, find the $$\mathrm{pH}$$ of buffer solution.

The solubility product of $$\mathrm{Mg}(\mathrm{OH})_2$$ is $$1.8 \times 10^{-11}$$ at $$298 \mathrm{~K}$$. What is its solubility in $$\mathrm{mol} \mathrm{~dm}^{-3}$$ ?

If $$\mathrm{K}_{\mathrm{sp}}$$ is solubility product of $$\mathrm{Al}(\mathrm{OH})_3$$, its solubility is expressed by formula,

What is the solubility of $$\mathrm{AgCl}_{(\mathrm{s})}$$ if its solubility product is $$1.6 \times 10^{-10}$$ ?

A buffer solution is prepared by mixing $$0.01 \mathrm{~M}$$ weak acid and $$0.05 \mathrm{~M}$$ solution of a salt of weak acid and strong base. What is the $$\mathrm{pH}$$ of buffer solution? $$(\mathrm{pKa}=4.74)$$

Which among the following is NOT an example of salt of strong acid and weak base?

Find $$[\mathrm{OH}]$$ if a monoacidic base is $$3 \%$$ ionised in its $$0.04 \mathrm{~M}$$ solution.

What is the expression for solubility product of silver chromate if it's solubility is expressed as $$\mathrm{S} \mathrm{~mol} \mathrm{~L}^{-1}$$ ?

What is $$\mathrm{pH}$$ of solution containing $$50 \mathrm{~mL}$$ each of $$0.1 \mathrm{~M}$$ sodium acetate and $$0.01 \mathrm{~M}$$ acetic acid? $$\left(\mathrm{pK}_{\mathrm{a}} \mathrm{CH}_3 \mathrm{COOH}=4.50\right)$$

Identify the salt that undergoes hydrolysis and forms acidic solution from following.

A weak base is $$1.42 \%$$ dissociated in its $$0.05 \mathrm{~M}$$ solution. Calculate its dissociation constant.

Calculate the degree of dissociation of $$0.01 \mathrm{~M}$$ acetic acid at $$25^{\circ} \mathrm{C}\left[\Lambda_{\mathrm{c}}=15.0 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\right.$$ and $$\left.\Lambda_0=300 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}\right]$$

What is the pH of 0.005 M NaOH solution?

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

What is the concentration of $$\mathrm{OH}^{-}$$ ion in a solution containing $$0.05 \mathrm{~M} \mathrm{~H}^{+}$$ ions?

Calculate the $$\mathrm{pH}$$ of $$1.36 \times 10^{-2} \mathrm{M}$$ solution of perchloric acid.

Find solubility in terms of $$\mathrm{mol} \mathrm{~L}^{-1}$$ if solubility product of silver bromide is $$6.4 \times 10^{-13}$$.

Calculate the $$\mathrm{pH}$$ of a buffer solution containing $$0.01 ~\mathrm{M}$$ salt and $$0.004 \mathrm{~M}$$ weak acid.

$$\left(\mathrm{pK}_{\mathrm{a}}=4.762\right)$$

Calculate the concentration of $$\mathrm{H}^{+}$$ ions in a solution if pOH is 11.

Acetic acid dissociated to $$1.20 \%$$ in its $$0.01 \mathrm{~M}$$ solution. What is the value of its dissociation constant?

Find solubility of $$\mathrm{PbI}_2$$ if its solubility product is $$7.0 \times 10^{-9}$$.

What is the $$\mathrm{pH}$$ of a solution containing $$2.2 \times 10^{-6} \mathrm{M}$$ hydrogen ions?

What is the concentration of $$\left[\mathrm{H}_3 \mathrm{O}^{+}\right]$$ ion in $$\mathrm{mol} ~\mathrm{L}^{-1}$$ of $$0.001 ~\mathrm{M}$$ acetic acid $$(\alpha=0.134)$$ ?

A buffer solution is prepared by mixing 0.2 M sodium acetate and 0.1 M acetic acid. If pK$$_a$$ for acetic acid is 4.7, find the pH.

Which salt from following forms aqueous solution having $$\mathrm{pH}$$ less than 7 ?

Solubility of a salt $$\mathrm{A}_2 \mathrm{~B}_3$$ is $$1 \times 10^{-3} \mathrm{~mol} \mathrm{~dm}^{-3}$$. What is the value of its solubility product?

Which of the following aqueous solutions of salts will have highest $$\mathrm{pH}$$ value?

What is the $$\mathrm{pH}$$ of $$2 \times 10^{-3} \mathrm{M}$$ solution of monoacidic weak base if it ionises to the extent of $$5\%$$ ?

The solubility of sparingly soluble salt $$\mathrm{AB}_2$$ is $$1.0 \times 10^{-4} \mathrm{~mol} \mathrm{~dm}^{-3}$$. What is it's solubility product?

What is the $$\mathrm{pH}$$ of $$0.005 \mathrm{~M} \mathrm{~H}_2 \mathrm{SO}_4$$ solution?

The solubility product expression for $$\mathrm{Ca}_3\left(\mathrm{PO}_4\right)_2$$ is represented as

Identify conjugate acid-base pair in the following reaction.

$$ \mathrm{HCl}_{(\mathrm{aq})}+\mathrm{H}_2 \mathrm{O}_{(l)} \rightleftharpoons \mathrm{H}_3 \mathrm{O}_{(\mathrm{aq})}^{+}+\mathrm{Cl}_{(\mathrm{aq})}^{-}$$

Which among the following salts undergoes hydrolysis?

At $$298 \mathrm{~K}, 0.1 \mathrm{M}$$ solution of acetic acid is $1.34 \%$ ionized. What is the dissociation constant of acetic acid?

$$\mathrm{pH}$$ of soft drink is 3.6. Calculate the concentration of hydrogen ions in it.

Which among the following salt solution in water shows pH less than 7 ?

The solubility of $$\mathrm{Ag}_2 \mathrm{C}_2 \mathrm{O}_4$$ is $$2 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$$ at $$298 \mathrm{~K}$$. What is it's solubility product?

A weak monobasic acid is $$3.0 \%$$ dissociated in it's $$0.04 \mathrm{~M}$$ solution. What is the dissociation constant of acid?

Solubility product of $$\mathrm{AgBr}$$ is $$4.9 \times 10^{-13}$$. What is its solubility?

Which of the following is NOT a correct mathematical equation for Ostwald dilution law?

A weak monobasic acid is $$10 \%$$ dissociated in $$0.05 \mathrm{~M}$$ solution. What is its percentage dissociation in $$0.10 \mathrm{~M}$$ solution?

The dissociation constant of weak monobasic acid is 2.7 $$\times$$ 10$$^{-5}$$. If degree of dissociation of acid is 3 $$\times$$ 10$$^{-2}$$, what is the concentration of acid?

The solubility product of a sparingly soluble salt AX$$_2$$ is 3.2 $$\times$$ 10$$^{-8}$$. What is it's solubility in mol dm$$^{-3}$$ ?

Which of the following salt solutions is highly acidic?

The $$\left[\mathrm{OH}^{-}\right]$$ in a solution is $$1 \times 10^{-12} \mathrm{~mol} \mathrm{~dm}{ }^{-3}$$. What is the concentration of $$\mathrm{H}^{+}$$ ions?

Which among the following salt solution in water shows pH greater than 7?

The pH of 0.005 M KOH is 9.95. Calculate the [OH$$^-$$] ?

Which among the following salts turns blue litmus red in it's aqueous solution?

What is the pH of 0.02 M NaOH solution?

Dissociation constant of propionic acid is $$1.32 \times 10^{-5}$$. Calculate the degree of dissociation of acid in $$0.05 \mathrm{~M}$$ solution.

Solubility of $$\mathrm{AgCl}$$ is $$7.2 \times 10^{-7} \mathrm{~mol} ~\mathrm{dm}^{-3}$$. What is it's solubility product?

A substance containing hydrogen and releasing H$$^+$$ in aqueous medium is acid. Identify theory suggesting this concept, from following.

The solubility of AgCl in it's solution is 1.25 $$\times$$ 10$$^{-5}$$ mol dm$$^{-3}$$. What is solubility product of AgCl?

Which from following compounds accepts proton from water molecule according to Bronsted-Lowry theory?

The pH of 0.1 M solution of monobasic acid is 2.34. Calculate the degree of dissociation of the acid.

The precipitation power of an electrolyte increases with

If the van't Hoff-factor for $0.1 \mathrm{~M} \mathrm{~Ba}\left(\mathrm{NO}_3\right)_2$ solution is 2.74 , the degree of dissociation is