Ionic Equilibrium Practice Test — Class 12 Chemistry

12th Standard Chemistry — Ionic Equilibrium: Online Practice Test

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Concentration of the \(Ag^+\) ions in a saturated solution of \(Ag_2C_2O_4\) is \(2.24 \times 10^{-4}\text{ mol L}^{-1}\) solubility product of \(Ag_2C_2O_4\) is (NEET – 2017)

A.\(2.42 \times 10^{-8}\text{ mol}^3\text{L}^{-3}\) B.\(2.66 \times 10^{-12}\text{ mol}^3\text{L}^{-3}\) C.\(4.5 \times 10^{-11}\text{ mol}^3\text{L}^{-3}\) D.\(5.619 \times 10^{-12}\text{ mol}^3\text{L}^{-3}\)

Following solutions were prepared by mixing different volumes of NaOH of HCl different concentrations. (NEET – 2018) i. 60 mL \(\frac{M}{10}\) HCl + 40mL \(\frac{M}{10}\) NaOH ii. 55 mL \(\frac{M}{10}\) HCl + 45 mL \(\frac{M}{10}\) NaOH iii. 75 mL \(\frac{M}{5}\) HCl + 25mL \(\frac{M}{5}\) NaOH iv. 100 mL \(\frac{M}{10}\) HCl + 100 mL \(\frac{M}{10}\) NaOH pH of which one of them will be equal to 1?

A.iv B.i C.ii D.iii

The solubility of \(BaSO_4\) in water is \(2.42 \times 10^{-3}\text{ gL}^{-1}\) at 298K. The value of its solubility product \(K_{sp}\) will be (NEET -2018). (Given molar mass of \(BaSO_4 = 233\text{g mol}^{-1}\))

A.\(1.08 \times 10^{-14}\text{ mol}^2\text{ L}^{-2}\) B.\(1.08 \times 10^{-12}\text{ mol}^2\text{ L}^{-2}\) C.\(1.08 \times 10^{-10}\text{ mol}^2\text{ L}^{-2}\) D.\(1.08 \times 10^{-8}\text{ mol}^2\text{ L}^{-2}\)

pH of a saturated solution of \(Ca(OH)_2\) is 9. The Solubility product (\(K_{sp}\)) of \(Ca(OH)_2\) is

A.\(0.5 \times 10^{-15}\) B.\(0.25 \times 10^{-10}\) C.\(0.125 \times 10^{-15}\) D.\(0.5 \times 10^{-10}\)

Conjugate base for Bronsted acids \(H_2O\) and HF are

A.\(OH^-\) and \(H_2F^+\), respectively B.\(H_3O^+\) and \(F^-\), respectively C.\(OH^-\) and \(F^-\), respectively D.\(H_3O^+\) and \(H_2F^+\), respectively

Which will make basic buffer?

A.50 mL of 0.1M NaOH + 25mL of 0.1M \(CH_3COOH\) B.100 mL of 0.1M \(CH_3COOH\) + 100 mL of 0.1M \(NH_4OH\) C.100 mL of 0.1M HCl + 200 mL of 0.1M \(NH_4OH\) D.100 mL of 0.1M HCl + 100 mL of 0.1M NaOH

Which of the following fluro compounds is most likely to behave as a Lewis base? (NEET – 2016)

A.\(BF_3\) B.\(PF_3\) C.\(CF_4\) D.\(SiF_4\)

Which of these is not likely to act as Lewis base?

A.\(BF_3\) B.\(PF_3\) C.CO D.\(F^-\)

The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively

A.acidic, acidic, basic B.basic, acidic, basic C.basic, neutral, basic D.none of these

Q10

The percentage of pyridine (\(C_5H_5N\)) that forms pyridinium ion (\(C_5H_5NH^+\)) in a 0.10M aqueous pyridine solution (\(K_b\) for \(C_5H_5N = 1.7 \times 10^{-9}\)) is

A.0.006% B.0.013% C.0.77% D.1.6%

Q11

Equal volumes of three acid solutions of pH 1, 2 and 3 are mixed in a vessel. What will be the \(H^+\) ion concentration in the mixture?

A.\(3.7 \times 10^{-2}\) B.\(10^{-6}\) C.0.111 D.none of these

Q12

The solubility of AgCl (s) with solubility product \(1.6 \times 10^{-10}\) in 0.1M NaCl solution would be

A.\(1.26 \times 10^{-5} M\) B.\(1.6 \times 10^{-9} M\) C.\(1.6 \times 10^{-11} M\) D.Zero

Q13

If the solubility product of lead iodide is \(3.2 \times 10^{-8}\), its solubility will be

A.\(2 \times 10^{-3} M\) B.\(4 \times 10^{-4} M\) C.\(1.6 \times 10^{-5} M\) D.\(1.8 \times 10^{-5} M\)

Q14

MY and \(NY_3\), are insoluble salts and have the same \(K_{sp}\) values of \(6.2 \times 10^{-13}\) at room temperature. Which statement would be true with regard to MY and \(NY_3\)?

A.The salts MY and \(NY_3\) are more soluble in 0.5M KY than in pure water B.The addition of the salt of KY to the suspension of MY and \(NY_3\) will have no effect on their solubilities C.The molar solubilities of MY and \(NY_3\) in water are identical D.The molar solubility of MY in water is less than that of \(NY_3\)

Q15

What is the pH of the resulting solution when equal volumes of 0.1M NaOH and 0.01M HCl are mixed?

A.2.0 B.3 C.7.0 D.12.65

Q16

The dissociation constant of a weak acid is \(1 \times 10^{-3}\). In order to prepare a buffer solution with a pH = 4, the \([Acid]/[Salt]\) ratio should be

A.4:3 B.3:4 C.10:1 D.1:10

Q17

The pH of \(10^{-5}\) M KOH solution will be

A.9 B.5 C.19 D.none of these

Q18

\(H_2PO_4^-\) is the conjugate base of

A.\(PO_4^{3-}\) B.\(P_2O_5\) C.\(H_3PO_4\) D.\(HPO_4^{2-}\)

Q19

Which of the following can act as Lowry – Bronsted acid as well as base?

A.HCl B.\(SO_4^{2-}\) C.\(HPO_4^{2-}\) D.\(Br^-\)

Q20

The pH of an aqueous solution is Zero. The solution is

A.slightly acidic B.strongly acidic C.neutral D.basic

Q21

The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by

A.\([H^+] = K_a \frac{[acid]}{[salt]}\) B.\([H^+] = K_a [salt]\) C.\([H^+] = K_a [acid]\) D.\([H^+] = K_a \frac{[salt]}{[acid]}\)

Q22

Which of the following relation is correct for degree of hydrolysis of ammonium acetate?

A.\(h = \sqrt{\frac{K_h}{C}}\) B.\(h = \sqrt{\frac{K_a}{K_b}}\) C.\(h = \sqrt{\frac{K_w}{K_a \cdot K_b}}\) D.\(h = \sqrt{\frac{K_a \cdot K_b}{K_w}}\)

Q23

Dissociation constant of \(NH_4OH\) is \(1.8 \times 10^{-5}\) the hydrolysis constant of \(NH_4Cl\) would be

A.\(1.8 \times 10^{-19}\) B.\(5.55 \times 10^{-10}\) C.\(5.55 \times 10^{-5}\) D.\(1.80 \times 10^{-5}\)

Q24

According to the Arrhenius theory, which of the following best describes a base?

A.A substance that donates a proton to another substance B.A species that accepts an electron pair C.A substance that dissociates to give hydroxyl ions in water D.A species that donates a proton to water

Q25

In the Lowry-Bronsted concept, what is the conjugate acid formed when \(H_2O\) acts as a base and accepts a proton?

A.\(OH^-\) B.\(H_3O^+\) C.\(H_2O_2\) D.\(H_2\)

Q26

Which of the following is classified as a Lewis acid due to being an electron-deficient molecule?

A.\(NH_3\) B.\(H_2O\) C.\(BF_3\) D.\(F^-\)

Q27

If an aqueous solution has a hydronium ion concentration \([H_3O^+]\) of \(1 \times 10^{-4}\) M, what is its pH?

A.4 B.10 C.7 D.14

Q28

The ionic product of water (\(K_w\)) is known to increase when which of the following occurs?

A.Pressure is decreased B.Temperature is increased C.A strong acid is added D.A strong base is added

Q29

According to Ostwald's dilution law, the degree of dissociation (\(\alpha\)) of a weak electrolyte is:

A.Directly proportional to the molar concentration B.Inversely proportional to the square root of concentration C.Independent of the volume of the solution D.Equal to the square of the dissociation constant

Q30

What is the term for the suppression of a weak acid's dissociation by adding a salt that contains a shared ion?

A.Buffer action B.Salt hydrolysis C.Common ion effect D.Electrolysis

Q31

Which of the following combinations would produce an acidic buffer solution?

A.\(NH_4OH\) and \(NH_4Cl\) B.\(CH_3COOH\) and \(CH_3COONa\) C.\(HCl\) and \(NaCl\) D.\(NaOH\) and \(NaCl\)

Q32

Identify the Henderson-Hasselbalch equation used specifically to calculate the pOH of a basic buffer.

A.\(pH = pK_a + \log \frac{[salt]}{[acid]}\) B.\(pOH = pK_b + \log \frac{[salt]}{[base]}\) C.\(pH = pK_w - pOH\) D.\(K_h = \frac{K_w}{K_a}\)

Q33

An aqueous solution of ammonium chloride (\(NH_4Cl\)) is acidic because of the hydrolysis of which species?

A.The \(Cl^-\) ion B.The \(NH_4^+\) ion C.The entire \(NH_4Cl\) molecule D.Water molecules only

Q34

Which of the following salts will form a neutral aqueous solution with a pH of 7 at 298K?

A.\(CH_3COONa\) B.\(NH_4Cl\) C.\(NaCl\) D.\(Na_2CO_3\)

Q35

For the sparingly soluble salt silver chromate (\(Ag_2CrO_4\)), the solubility product (\(K_{sp}\)) expression is:

A.\([Ag^+][CrO_4^{2-}]\) B.\([Ag^+][CrO_4^{2-}]^2\) C.\([Ag^+]^2[CrO_4^{2-}]\) D.\([Ag^+] + [CrO_4^{2-}]\)

Q36

If 's' represents the molar solubility of \(Ag_2CrO_4\) in water, how is \(K_{sp}\) related to 's'?

A.\(K_{sp} = s^2\) B.\(K_{sp} = 4s^2\) C.\(K_{sp} = 4s^3\) D.\(K_{sp} = 27s^4\)

Q37

In which condition will a precipitate definitely form when two solutions are mixed?

A.Ionic Product is equal to \(K_{sp}\) B.Ionic Product is less than \(K_{sp}\) C.Ionic Product is greater than \(K_{sp}\) D.Ionic Product is zero

Q38

Which of the following species acts as a Lewis base by donating an electron pair to form a coordinate bond?

A.\(Fe^{3+}\) B.\(BF_3\) C.\(NH_3\) D.\(AlCl_3\)

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About this Ionic Equilibrium test

This free online practice test covers Ionic Equilibrium from the 12th Standard Chemistry (Samacheer Kalvi) syllabus. Choose the number of questions and an optional time limit, then answer and submit — everything is checked in your browser, with the correct answers and a worked explanation shown at the end. For the full solutions to every question in this set, see the solved MCQs page.

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