Ionic Equilibrium PYQs - Last 10 Years

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Practice 202 MHT CET Chemistry questions from Ionic Equilibrium. Use the year-wise and type-wise breakdown to prioritize recent PYQs, then continue into the question list below.

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Last 10 Years Ionic Equilibrium Questions

Showing 50 of 202 filtered questions.

1Ionic Equilibrum

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.

2Ionic Equilibrum

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

3Ionic Equilibrum

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

4Ionic Equilibrum

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.

5Ionic Equilibrum

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

6Ionic Equilibrum

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

7Ionic Equilibrum

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

8Ionic Equilibrum

Calculate pH of 0.002 M KOH solution.

9Ionic Equilibrum

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. $\left(\mathrm{pK}_{\mathrm{b}}=4.730\right)$

10Ionic Equilibrum

Which of the following salt solutions turns red litmus blue?

11Ionic Equilibrum

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

12Ionic Equilibrum

Which from following species acts as base ${ }^1$, according to Bronsted-Lowry theory?
\(\mathrm{HCl}+\mathrm{NH}_3 \text { 目的 } \mathrm{NH}_4^{+}+\mathrm{Cl}^{-}\)

13Ionic Equilibrum

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.

14Ionic Equilibrum

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

15Ionic Equilibrum

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.

16Ionic Equilibrum

Calculate the pH of 0.01 M sulphuric acid.

17Ionic Equilibrum

Which from following mixtures in water acts as a buffer?

18Ionic Equilibrum

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

19Ionic Equilibrum

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.

20Ionic Equilibrum

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

21Ionic Equilibrum

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.

22Ionic Equilibrum

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....

23Ionic Equilibrum

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

24Ionic Equilibrum

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 $\mathrm{NH}_4 \mathrm{OH}$ ?

25Ionic Equilibrum

Acidic buffer solution is prepared by mixing proportionate quantity of

26Ionic Equilibrum

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

27Ionic Equilibrum

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

28Ionic Equilibrum

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?

29Ionic Equilibrum

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

30Ionic Equilibrum

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

31Ionic Equilibrum

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

32Ionic Equilibrum

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?

33Ionic Equilibrum

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

34Ionic Equilibrum

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

35Ionic Equilibrum

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

36Ionic Equilibrum

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 $1.8 \times 10^{-5}$.

37Ionic Equilibrum

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

38Ionic Equilibrum

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?

39Ionic Equilibrum

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

40Ionic Equilibrum

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.

41Ionic Equilibrum

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 \((\alpha=0.134)\) ?

42Ionic Equilibrum

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

43Ionic Equilibrum

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

44Ionic Equilibrum

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

45Ionic Equilibrum

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

46Ionic Equilibrum

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

47Ionic Equilibrum

Identify base\(_2\) for following equation according to Bronsted-Lowry theory.
\(\mathrm{HCl}_{(\mathrm{aq})}+\mathrm{H}_2 \mathrm{O}_{(l)} \rightleftharpoons \mathrm{H}_3 \mathrm{O}_{(\mathrm{aq})}^{+}+\mathrm{Cl}_{(\mathrm{aq})}^{-}\)

48Ionic Equilibrum

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

49Ionic Equilibrum

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

50Ionic Equilibrum

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