Ionic Equilibrium PYQs Set 1 (PDF)

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Mere Teacher · Previous Year Questions JEE Main Chemistry · Ionic Equilibrium · Set 1 (Q1-30)
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1. $For a reaction A (s) \sim B (s) + C (g) the set of all correct statements are(A) K is independent of [A] .(B) K is dependent on partial pressure of C at a given temperature.(C) ΔH will be independent of temperature.(D) ΔH is independent of the catalyst addition.$ (1) $A, B, C, D$ (2) $A, B only$ (3) $A, B, D only$ (4) $A, B, C only$ 2. $For a sparingly soluble salt AB_{2}, the equilibrium concentrations of A^{2 +} ions and B^{-} ions are 1.2 \times 10^{- 4} M and 0.24 \times 10^{- 3} M, respectively. The solubility product of AB_{2} is :$ (1) $6.91 \times 10^{- 12}$ (2) $0.276 \times 10^{- 12}$ (3) $27.65 \times 10^{- 12}$ (4) $0.069 \times 10^{- 12}$ 3. $For the following Assertion and Reason, the correct option is: Assertion: The pH of water increases with increases in temperature. Reason: The dissociation of water into H^{+} and O H^{-} is an exothermic reaction.$ (1) $Both Assertion and Reason are correct and reason is correct explanation of assertion.$ (2) $Both Assertion and Reason are correct and reason is not correct explanation of assertion.$ (3) $Assertion is true & reason is false.$ (4) $Both Assertion and Reason are incorrect.$ 4. $What is the pH of a solution containing 2.2 \times 10^{- 6} M hydrogen ions?$ (1) $6.34$ (2) $5.66$ (3) $4.34$ (4) $3.80$ 5. $The pH of 0.01 N lime water is$ (1) $13.09$ (2) $10$ (3) $12$ (4) $9.8$ 6. $The equilibrium constant (K_{p}) for the formation of ammonia from its constituent elements at 27^{\circ} C is 1.2 \times 10^{- 4} and at 127^{\circ} C is 0.60 \times 10^{- 4} . Calculate the mean heat of formation of ammonia per mole in this temperature range.$ (1) $- 82.64 cal$ (2) $- 826.4 cal$ (3) $- 1652.8 cal$ (4) $- 165.2 cal$ 7. $Which of the following statements is correct for a reversible process in a state of equilibrium?$ (1) $Δ G^{o} = - 2.30 RT log K$ (2) $Δ G^{o} = 2.30 RT log K$ (3) $Δ G = - 2.30 RT log K$ (4) $Δ G = 2.30 RT log K$ 8. $When one mole of A and one mole of B were heated in one litre flask at T (K), 0.5 mole of C was formed in the equilibrium, A + B ⇌ C + D the equilibrium constant, K_{C} is$ (1) $0.25$ (2) $0.5$ (3) $1$ (4) $2$ 9. $At T (K), K_{C} value for the reaction \frac{1}{3} N_{2} (g) H_{2} (g) ⇌ \frac{2}{3} NH_{3} (g) is 50 . The K_{C} value for the reaction 2 NH_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g) at the same temperature is$ (1) $4 \times 10^{- 6}$ (2) $8 \times 10^{- 6}$ (3) $6 \times 10^{- 6}$ (4) $8 \times 10^{- 3}$ 10. $What quantity (in mL) of a 45% acid solution of a mono-protic strong acid must be mixed with a 20% solution of the same acid to produce 800 mL of a 29.875% acid solution ?$ (1) $330$ (2) $316$ (3) $320$ (4) $325$ 11. $A weak acid HA has degree of dissociation x. Which option gives the correct expression of (pH pK_{a}) ?$ (1) $0$ (2) $log (1 + 2 x)$ (3) $log (\frac{1 - x}{x})$ (4) $log (\frac{x}{1 - x})$ 12. $Incorrect statement for the use of indicators in acid-base titration is :$ (1) $Methyl orange may be used for a weak acid vs weak base titration.$ (2) $Methyl orange is a suitable indicator for a strong acid vs weak base titration$ (3) $Phenolphthalein is a suitable indicator for a weak acid vs strong base titration$ (4) $Phenolphthalein may be used for a strong acid vs strong base titration.$ 13. $What is the pH of 10 L of a buffer solution containing 0.01 M NH_{4} Cl and 0.1 M NH_{4} OH having pK_{b} of 5 ?$ (1) $88$ (2) $7$ (3) $10$ (4) $5$ 14. $Solubility of a salt A_{2} B_{3} is 1 \times 10^{- 3} mol dm^{- 3} . What is the value of its solubility product?$ (1) $1.08 \times 10^{- 13}$ (2) $8.1 \times 10^{- 15}$ (3) $2.7 \times 10^{- 15}$ (4) $2.0 \times 10^{- 13}$ 15. $At T (K), the K_{p} for the reaction A_{2} B_{6} (g) \to A_{2} B_{4} (g) + B_{2} (g) is 0.04 atm . The equilibrium pressure (in atm) of (A_{2} B_{6}) g) when it is placed in a flask at 4 atm pressure and allowed to come to above equilibrium is$ (1) $0.362$ (2) $0.380$ (3) $3.62$ (4) $2.62$ 16. $An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would (Given log 2 = 0.30)$ (1) $increase to 1.3$ (2) $reduce to 0.5$ (3) $increase to 2$ (4) $remain same$ 17. $Hydrolysis of sucrose is given by the following reaction. Sucrose + H_{2} O ⇌ Glucose + Fructose If the equilibrium constant (K_{e}) is 2 \times 10^{13} at 300 K , the value of Δ_{r} G^{\circ} at the same temperature will be:$ (1) $8.314 J mol^{- 1} K-1\times300 K\timesln2\times1013$ (2) $8.314 J mol^{- 1} K-1\times300 K\timesln3\times1013$ (3) $-8.314 J mol^{- 1} K-1\times300 K\timesln4\times1013$ (4) $-8.314 J mol^{- 1} K-1\times300 K\timesln2\times1013$ 18. $100 mL of 0.1 MHCl is taken in a beaker and to it 100 mL of 0.1 MNaOH is added in steps of 2 mL and the pH is continuously measured. Which of the following graphs correctly depicts the change in pH?$ (1) (2) (3) (4) 19. $K_{P} / K_{C} for the reaction at T (K) is CO (g) + \frac{1}{2} O_{2} (g) ⇌ CO_{2} (g)$ (1) $RT$ (2) $2 RT$ (3) $RT$ (4) $1/ RT$ 20. $The pH of 0.01 MBOH solution is 10 . What is its degree of dissociation? (Given K_{b} of BOH is 1 \times 10^{- 6})$ (1) $10 %$ (2) $5 %$ (3) $2 %$ (4) $1 %$ 21. $The molar solubility(s) of zirconium phosphate with molecular formula (Zr^{4 +})_{3} (PO_{4}^{3 -})_{4} is given by relation:$ (1) $(\frac{K _{sp}}{9612})^{\frac{1}{3}}$ (2) $(\frac{K _{sp}}{6912})^{\frac{1}{7}}$ (3) $(\frac{K _{sp}}{8435})^{\frac{1}{7}}$ (4) $(\frac{K _{p}}{5348})^{\frac{1}{6}}$ 22. $HCl was passed through a solution of CaCl_{2}, MgCl_{2} and NaCl. Which of the following compound (s) crystallies (s)?$ (1) $Only NaCl$ (2) $Only MgCl_{2}$ (3) $NaCl, MgCl_{2} and CaCl_{2}$ (4) $Both MgCl_{2} and CaCl_{2}$ 23. $Which among the following salt solutions is basic in nature?$ (1) $Ammonium sulphate$ (2) $Ammonium nitrate$ (3) $Sodium acetate$ (4) $Ammonium chloride$ 24. $Assuming that the degree of hydrolysis is small, the pH of 0.1 M solution of sodium acetate (K_{a} = 1.0 \times 1 0^{-5}) will be:$ (1) $5.0$ (2) $6.0$ (3) $8.0$ (4) $9.0$ 25. $What is the molar solubility of Al (OH)_{3} in 0.2 MNaOH solution? Given that, solubility product of Al (OH)_{3} = 2.4 \times 10^{- 24} :$ (1) $3 \times 10^{- 19}$ (2) $12 \times 10^{- 21}$ (3) $3 \times 10^{- 22}$ (4) $12 \times 10^{- 23}$ 26. $The equilibrium constant (K_{C}) for the following equilibrium 2 SO_{2} (g) + O_{2} (g) ⇌ 2 SO_{3} (g) at 563 K is 100 . At equilibrium, the number of moles of SO_{3} in the 10 litre flask is twice the number of moles of SO_{2}, then the number of moles of oxygen is$ (1) $0.4$ (2) $0.3$ (3) $0.2$ (4) $0.1$ 27. $Le-Chateliers' principle is not applicable to$ (1) $H_{2} (g) I_{2} (g) ⇌ 2 HI (g)$ (2) $Fe (s) + S (s) ⇌ FeS (s)$ (3) $N_{2} (g) + 3 H_{2} (g) ⇌ 2 NH_{3} (g)$ (4) $N_{2} (g) + O_{2} (g) ⇌ 2 NO (g)$ 28. $The solubility of A g C 1 will be minimum in$ (1) $0.01 M C a C l_{2}$ (2) $pure water$ (3) $0.001 M A g N O_{3}$ (4) $0.01 M N a C l$ 29. $In HS, I, R - N H_{2}, N H_{3} order of proton accepting tendency will be$ (1) $I^{-} > N H_{3} > R - N H_{2} > H S^{-}$ (2) $N H_{3} > R - N H_{2} > H S^{-} > I^{-}$ (3) $R - N H_{2} > N H_{3} > H S^{-} > I^{-}$ (4) $H S^{-} > R - N H_{2} > N H_{3} > I^{-}$ 30. $K_{a} for CH_{3} COOH is 1.8 \times 10^{- 5} and K_{b} for NH_{4} OH is 1.8 \times 10^{- 5} . The pH of ammonium acetate solution will be$