Equilibrium: NEET questions with solutions

NEET tests this chapter through Kc/Kp calculations, Le Chatelier predictions, and ionic equilibrium numericals: pH of weak acids and strong bases, buffers, and Ksp–solubility. Marks are lost by forgetting stoichiometric powers in K, mixing ln with log in ΔG° = −RT ln K, and not accounting for neutralisation before applying the buffer equation.

1. 1.For the gas-phase equilibrium 2SO₃(g) ⇌ 2SO₂(g) + O₂(g), which relation between Kp and Kc is correct?Relationship between Kp and KcEasySingle correct
2. 2.For the equilibrium N₂O₄(g) ⇌ 2NO₂(g), ΔH > 0, which change increases the amount of NO₂ present at the new equilibrium?Factors affecting equilibria: Le Chatelier's principleEasySingle correct
3. 3.2.0 mol of A(g) and 2.0 mol of B(g) are placed in a sealed 2.0 L flask at a fixed temperature. The reaction A(g) + B(g) ⇌ 2C(g) reaches…Calculating equilibrium constantsMediumSingle correct
4. 4.What is the pH of a 0.020 M aqueous solution of a weak monobasic acid HA whose Ka = 2.0 × 10⁻⁵ at 298 K? (log 2 = 0.301, log 6.32 = 0.80)Ionization constants of weak acidsMediumSingle correct
5. 5.Read the Assertion (A) and Reason (R) and choose the correct option.Common ion effect in ionization of acidsMediumAssertion–Reason
6. 6.A sparingly soluble salt M₂X dissociates as M₂X(s) ⇌ 2M⁺(aq) + X²⁻(aq). Its solubility product at 298 K is 3.2 × 10⁻¹¹. What is its molar…Solubility product constantMediumSingle correct
7. 7.What is the pH of a 0.005 M aqueous solution of Ba(OH)₂ at 298 K? Assume complete dissociation. (Kw = 1.0 × 10⁻¹⁴, log 2 = 0.301)The pH scale: strong basesEasySingle correct
8. 8.60 mL of 0.10 M aqueous NH₃ is mixed with 20 mL of 0.10 M HCl at 298 K. What is the pH of the resulting solution?Buffer solutionsHardSingle correct
9. 9.For a reaction at 300 K, ΔG° = +5.74 kJ mol⁻¹. What is the value of the equilibrium constant K at this temperature?Relationship between equilibrium constant K and ΔG°HardSingle correct