Ionic Equilibrium Book Back Practice Test

12th Standard Chemistry — Ionic Equilibrium: Book Back 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.\(1.80 \times 10^{-5}\)

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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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