Ionic Equilibrium: JEE Main Chemistry Previous Year Questions

274 previous year questions from Ionic Equilibrium. Here are the 25 most important ones; open any question for the correct answer and a full step-by-step solution.

1. $For a reaction A (s) \sim B (s) + C (g) the set of all correct statements are(A) K is independent of [A] .(B) K\dots$
2. $For a sparingly soluble salt AB_{2}, the equilibrium concentrations of A^{2 +} ions and B^{-} ions are 1.2 \times 10^{- 4} M and\dots$
3. $For the following Assertion and Reason, the correct option is: Assertion: The pH of water increases with increases in temperature. Reason: The dissociation of water into\dots$
4. $What is the pH of a solution containing 2.2 \times 10^{- 6} M hydrogen ions?$
5. $The pH of 0.01 N lime water is$
6. $The equilibrium constant (K_{p}) for the formation of ammonia from its constituent elements at 27^{\circ} C is 1.2 \times 10^{- 4} and at\dots$
7. $Which of the following statements is correct for a reversible process in a state of equilibrium?$
8. $When one mole of A and one mole of B were heated in one litre flask at T (K), 0.5 mole of C was formed in the equilibrium,\dots$
9. $At T (K), K_{C} value for the reaction\dots$
10. $What quantity (in mL) of a 45% acid solution of a mono-protic strong acid must be mixed with a 20% solution of the same acid to produce 800 mL of a 29.875% acid solution\dots$
11. $A weak acid HA has degree of dissociation x. Which option gives the correct expression of (pH pK_{a}) ?$
12. $K_{a} for CH_{3} COOH is 1.8 \times 10^{- 5} and K_{b} for NH_{4} OH is 1.8 \times 10^{- 5} . The pH of ammon\dots$
13. $Incorrect statement for the use of indicators in acid-base titration is :$
14. $What is the pH of 10 L of a buffer solution containing 0.01 M NH_{4} Cl and 0.1 M NH_{4} OH having pK_{b} of 5 ?$
15. $Solubility of a salt A_{2} B_{3} is 1 \times 10^{- 3} mol dm^{- 3} . What is the value of its solubility product?$
16. $At T (K), the K_{p} for the reaction A_{2} B_{6} (g) \to A_{2} B_{4} (g) + B_{2} (g) is\dots$
17. $An aqueous solution of HCl with pH 1.0 is diluted by adding equal volume of water (ignoring dissociation of water). The pH of HCl solution would (Given\dots$
18. $Hydrolysis of sucrose is given by the following reaction. Sucrose + H_{2} O ⇌ Glucose + Fructose If the equilibrium constant (K_{e}) is\dots$
19. $100 mL of 0.1 MHCl is taken in a beaker and to it 100 mL of 0.1 MNaOH is added in steps of 2 mL and the pH is continuously measured. Which of the following graphs correct\dots$
20. $K_{P} / K_{C} for the reaction at T (K) is CO (g) + \frac{1}{2} O_{2} (g) ⇌ CO_{2} (g)$
21. $The pH of 0.01 MBOH solution is 10 . What is its degree of dissociation? (Given K_{b} of BOH is 1 \times 10^{- 6})$
22. $The molar solubility(s) of zirconium phosphate with molecular formula (Zr^{4 +})_{3} (PO_{4}^{3 -})_{4} is given by relation:$
23. $HCl was passed through a solution of CaCl_{2}, MgCl_{2} and NaCl. Which of the following compound (s) crystallies (s)?$
24. $Which among the following salt solutions is basic in nature?$
25. $Assuming that the degree of hydrolysis is small, the pH of 0.1 M solution of sodium acetate (K_{a} = 1.0 \times 1 0^{-5}) will be:$

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Ionic Equilibrium: JEE Main Chemistry Previous Year Questions

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