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1. The value of Kw at 25°C is

A. 10^7 B. 10^-7 C. 10^-14 D. 10^14

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2. If the pH of a solution is 4, its hydrogen ion concentration is

A. 10^-5 M B. 10^-4 M C. 10^-2 M D. 10^-3 M

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3. For a reaction at equilibrium, ΔG is

A. Zero B. Infinite C. Positive D. Negative

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4. For a reaction A + B ⇌ C + D, if Q > K, then

A. The reaction is at equilibrium B. The reaction proceeds in the forward direction C. No reaction occurs D. The reaction proceeds in the reverse direction

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5. The equilibrium constant Kc for a reaction is 10^4. This indicates that

A. Reaction does not proceed B. Neither reactants nor products are favored C. Products are favored D. Reactants are favored

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6. The equilibrium constant of a reaction depends on

A. Concentration B. Temperature C. Pressure D. Volume

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7. Which of the following expressions represents the equilibrium constant (Kc)?

A. Kc = [reactants]/[products] B. Kc = 1/[products] C. Kc = 1/[reactants] D. Kc = [products]/[reactants]

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8. The value of the equilibrium constant for an exothermic reaction

A. Decreases with increase in temperature B. Remains constant with increase in temperature C. Increases with increase in temperature D. Becomes zero with increase in temperature

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9. The pH of a 10^-3 M HCl solution is

A. 4 B. 2 C. 3 D. 1

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10. The solubility product (Ksp) is applicable for

A. Dilute solutions B. Unsaturated solutions C. Saturated solutions D. Supersaturated solutions

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11. Le Chatelier's principle predicts the effect of

A. Concentration changes B. All of these C. Pressure changes D. Temperature changes

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12. The equilibrium constant of a reaction increases with

A. Increase in temperature for an endothermic reaction B. Increase in temperature for an exothermic reaction C. Decrease in pressure D. Addition of a catalyst

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13. The Henderson-Hasselbalch equation is used to calculate

A. Solubility product B. Rate constant C. Equilibrium constant D. pH of a buffer solution

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14. The value of Kw at 25°C is

A. 10^-7 B. 10^-14 C. 10^7 D. 10^14

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15. The buffer capacity is maximum when

A. pH = 7 B. pH > pKa C. pH = pKa D. pH < pKa

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16. The solubility of BaSO4 in water is 1.05 × 10^-5 M. The Ksp of BaSO4 is approximately

A. 1.5 × 10^-10 B. 1.0 × 10^-10 C. 2.2 × 10^-10 D. 1.1 × 10^-10

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17. The buffer capacity is maximum when

A. pH = pKa B. pH < pKa C. pH = 7 D. pH > pKa

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18. The pH of a 0.01 M HCl solution is

A. 0 B. 2 C. 4 D. 1

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19. The common ion effect is observed in

A. Solutions of strong acids B. Solutions of strong bases C. Solutions of weak acids and their salts D. Solutions of neutral salts

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20. The equilibrium constant for a reaction is 1. What does this indicate?

A. Products are favored B. Reactants are favored C. Reactants and products are equally favored D. No reaction occurs