Class 11 Chemistry — Chapter 7: Equilibrium Online Test

1. In qualitative inorganic analysis, group IV cations are precipitated in ammoniacal medium because

2. If the solubility of (AgCl) is , the value is

3. When in a basic buffer, the pH equals

4. The hydrolysis constant is defined as

5. The pH of a (0.1,M) solution of is

6. The (pH) of a (0.2,M) solution is

7. The pH of a solution is defined as

8. According to Ostwald’s law, the degree of ionization is related to

9. For a weak base solution where , the hydroxide ion concentration is

10. The ionization constant of an acid is a measure of its

11. In the reaction , the Brønsted–Lowry base is

12. When the concentration of a reactant is increased in a system at equilibrium, the equilibrium

13. The main difference between and is that

14. For a general reaction , the expression for is

15. For at fixed (T), raising the external pressure of an inert gas at constant volume changes the extent of decomposition

16. For at a temperature where , starting with stoichiometric at 1 atm, the equilibrium extent toward is

17. The reaction has at 500 K. If initially is high and are low, the reaction will

18. For the equilibrium , the equilibrium constant expression is

19. For a heterogeneous equilibrium such as , the equilibrium constant is expressed as:

20. For at , . If initially and , the reaction will:

1. Which condition is inherently included in the definition of equilibrium for a reaction mixture?

2. The strength of an acid is determined by the magnitude of its

3. The Haber process is exothermic. Which change increases the equilibrium yield of ?

4. Ostwald’s dilution law is not applicable to

5. For , the correct expression for is

6. For a general reaction , the expression for is

7. The (pH) of a salt solution formed by a weak acid and strong base can be expressed as

8. The degree of ionization of a weak acid is related to its concentration (( C )) as

9. The relationship between Gibbs free energy and reaction quotient is

10. Which statement best defines chemical equilibrium in a closed system?

11. For , with and initial , equilibrium is

12. The smaller the value of , the

13. Which condition is required for a reversible reaction to reach equilibrium?

14. For a salt of a weak base and strong acid, the expression for pH is

15. The ionization equation for acetic acid is

16. Which of the following is NOT implied by the definition of chemical equilibrium?

17. The pH of a (0.1,M) solution of is

18. The low ionizing power of solvents like benzene is due to

19. The importance of Henderson’s equation lies in the fact that it

20. For a weak electrolyte whose limiting molar conductivity at infinite dilution is and measured molar conductivity at concentration (C) is , the degree of ionization is

21. In at constant temperature, the equilibrium constant is numerically equal to

22. Why does a chemical system at equilibrium appear static to the observer?

23. In dissolution equilibrium of a solid in a liquid (at fixed (T)), which action increases the amount of undissolved solid without changing solubility?

24. The pH of a (0.05,M) (KOH) solution is

25. Which statement differentiates “dynamic” chemical equilibrium from “static” equilibrium?

26. A sealed flask contains at temperature (T). Doubling the mass of while keeping (T) fixed will

27. For with starting from , , the approximate equilibrium is

28. Which statement best describes a saturated solution in contact with undissolved solid at constant (T)?

29. In the esterification system , which experimental result evidences dynamic equilibrium at constant (T)?

30. The reaction quotient for is given by

1. The degree of ionization of a weak electrolyte generally

2. If for a base, the strength of the base is

3. Using the Henderson equation, the pH of a buffer containing (0.1,M) acetic acid and (0.1,M) sodium acetate is

4. Which of the following pairs contains both weak electrolytes?

5. When , the Gibbs free energy change for the reaction is

6. For a reaction at temperature (T), which equation connects the definition of equilibrium with thermodynamics?

7. According to Arrhenius, a base is a substance that

8. If , the hydroxide ion concentration is

9. The pH of a (0.1,M) solution of is

10. Which of the following best represents the neutralization of an acid and a base according to Arrhenius?

11. If the solubility of (AgCl) is , the value is

12. The pH of sodium acetate solution is

13. If the ionic product equals the solubility product , the system is

14. For , if and initial concentrations of all species are , then equilibrium concentrations will

15. When ( Q > K ), the direction of spontaneous change is

16. For a salt of a weak acid and a weak base , the hydrolysis constant is

17. When the concentration of a product is increased in a reversible reaction, the equilibrium

18. In the equilibrium , the equilibrium constant in pressure form is

19. For at 298 K, . The predicted extent toward (B) is

20. The pOH of a solution is defined as

21. Which of the following statements correctly describes a limitation of the Arrhenius concept?

22. In the Contact process, the catalyst used to oxidize is

23. For a weak base (B) of concentration (C), the degree of ionization satisfies

24. Ostwald’s dilution law can also be written in terms of

25. The expression for in the reaction is

26. Which kinetic observation most directly evidences dynamic equilibrium in a reversible reaction mixture?

27. In the equilibrium , increasing total pressure shifts equilibrium

28. In the Haber process , increasing the pressure will

29. The solubility of a salt in terms of is given by

30. For a weak monoprotic acid, the relation between , (C), and the degree of ionization is

31. For , the appropriate constant at (T) is

32. For an exothermic reaction, increasing temperature will shift equilibrium

33. A nonvolatile solute is dissolved in a solvent with at a given (T). If the solute mole fraction is , the solution’s vapour pressure is:

34. In the reaction , the conjugate base of is

35. In qualitative inorganic analysis, group IV cations are precipitated in ammoniacal medium because

36. In the presence of a common ion, the degree of ionization of a weak acid (HA)

37. In the Brønsted–Lowry theory, the strength of an acid is inversely related to

38. For the reaction , the equilibrium constant in terms of concentration is derived by equating:

39. Which condition is essential for establishing chemical equilibrium in the laboratory?

40. For a weak acid where is very small, Ostwald’s dilution law simplifies to

41. The relationship between and for a gas-phase equilibrium is:

42. The pH of a solution of sodium chloride ((NaCl)) is

43. For a weak base solution where , the hydroxide ion concentration is

44. For the reaction , the difference in gaseous moles is

45. According to Arrhenius, which of the following aqueous solutions has the highest concentration of ions?

46. The main function of a buffer in biological systems is to

47. For , with and initial , equilibrium is

48. The main difference between a weak acid and a weak electrolyte is that

49. The main difference between and is that

50. The Henderson–Hasselbalch equation for an acidic buffer is