JEE CHEMISTRY UNIT 06
QUIZ NO 1
TOTAL QUESTIONS = 20
1. Which of the following is a characteristic of chemical equilibrium?;Concentrations of reactants and products are equal;The rate of the forward reaction equals the rate of the backward reaction;The reaction stops completely;The reaction is irreversible;B
A.
B.
C.
D.
2. The pH of a 0.01 M HCl solution is
A. 2
B. 3
C. 1
D. 4
3. For a reversible reaction, the equilibrium constant is given as
A. K = [reactants]/[products]
B. K = 1/[reactants]
C. K = [products]/[reactants]
D. K = 1/[products]
4. The ionization constant of a weak acid is represented by
A. Kw
B. Ka
C. Kb
D. Ksp
5. Which of the following is a characteristic of a buffer solution?
A. It does not contain salts
B. It is only made of strong acids
C. It resists pH changes
D. It has a fixed pH
6. The pH of a buffer solution can be calculated using
A. Van der Waals equation
B. Henry's law
C. Henderson-Hasselbalch equation
D. Raoult's law
7. Which of the following represents the relationship between Kp and Kc?
A. Kp = Kc × RT
B. Kp = Kc / (RT)^Δn
C. Kp = Kc × (RT)^Δn
D. Kp = Kc / RT
8. For a buffer solution, the pH is maximum when
A. pH = pKa
B. pH > pKa
C. pH < pKa
D. pH = 7
9. Which of the following pairs represents a basic buffer?
A. NH3 and NH4Cl
B. H2SO4 and NaHSO4
C. CH3COOH and CH3COONa
D. HCl and NaCl
10. The equilibrium constant for a reaction is 1. What does this indicate?
A. Products are favored
B. Reactants and products are equally favored
C. Reactants are favored
D. No reaction occurs
11. Which of the following represents a basic buffer?
A. H2SO4 and NaHSO4
B. HCl and NaCl
C. CH3COOH and CH3COONa
D. NH3 and NH4Cl
12. Which of the following pairs acts as an acidic buffer?
A. NH3 and NH4Cl
B. NaOH and NaCl
C. HCl and NaCl
D. CH3COOH and CH3COONa
13. Le Chatelier's principle predicts the effect of
A. Only concentration changes
B. Only pressure changes
C. Only temperature changes
D. Temperature, pressure, and concentration changes
14. 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
15. The pKa value of a strong acid is
A. Low
B. High
C. Negative
D. Zero
16. For the reaction 2NO2 ⇌ N2O4, the equilibrium constant in terms of partial pressures is given by
A. Kp = (PNO2)/(PN2O4)
B. Kp = (PN2O4)/(P^2NO2)
C. Kp = 1/(PNO2)
D. Kp = (P^2NO2)/(PN2O4)
17. For a reaction at equilibrium, if Kc > 1, then
A. The system is at rest
B. Products are favored
C. Reactants are favored
D. Neither reactants nor products are favored
18. The Henderson-Hasselbalch equation is used to calculate
A. Molarity
B. Equilibrium constant
C. Rate constant
D. pH of a buffer solution
19. The solubility product (Ksp) of a salt increases with
A. Increase in temperature
B. Increase in pressure
C. Decrease in pressure
D. Decrease in temperature
20. Which of the following solutions has the highest pH?
A. 0.1 M CH3COOH
B. 0.1 M NaOH
C. 0.1 M NH4Cl
D. 0.1 M HCl
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