2nd Year Chemistry Chapter 3 Test03. Chemical Equilibria

Q1. Multiple choice questions (Attempt all · 10 × 1 = 10)

1. If Kpc > 1, it means the solute is more soluble in:
   1. Organic solvent
   2. Water
   3. Both equally
   4. None of these
2. The bicarbonate buffer system in blood involves:
   1. NH₄OH and NH₄Cl
   2. NaOH and Na₂CO₃
   3. HCl and NaCl
   4. H₂CO₃ and HCO₃⁻
3. The common ion effect occurs when:
   1. A strong base is added to a strong acid
   2. Two salts are mixed in water
   3. A salt containing a common ion is added to a weak electrolyte
   4. Neutralization occurs
4. The dissociation of AgBr in water gives:
   1. Ag + Br₂
   2. AgBr + H₂O
   3. Ag⁺ + Br⁻
   4. Ag + Br⁻
5. Large molecules usually have a:
   1. Higher partition coefficient in polar phase
   2. Lower partition coefficient in non-polar phase
   3. Higher partition coefficient in non-polar phase
   4. No effect on partition coefficient
6. Which of the following salts is slightly soluble?
   1. KNO₃
   2. NaCl
   3. AgBr
   4. HCl
7. When a strong base like NaOH is added to the buffer solution, OH⁻ is neutralized by:
   1. CH₃COOH
   2. CH₃COONa
   3. H₂O
   4. Na⁺
8. A higher value of Ksp means:
   1. Salt is less soluble
   2. Salt is more soluble
   3. Salt is insoluble
   4. Salt has no solubility
9. The principle that explains common ion effect is:
   1. Henry’s law
   2. Le Chatelier’s principle
   3. Boyle’s law
   4. Graham’s law
10. Polar solutes prefer:
    1. Non-polar solvents
    2. Polar solvents
    3. Gaseous phase
    4. None of these