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 of the following has the smallest degree of ionization in water?

2. What does “macroscopic constancy” mean in a system at equilibrium?

3. The pH of a solution of sodium acetate is

4. For the reaction with and initial , the equilibrium concentration of (HI) is

5. Which of the following is an example of an Arrhenius base?

6. Which statement is true about the relation between and ( C )?

7. The unit of for the reaction is

8. If the ionic product (Q) is less than , the solution is

9. Ostwald’s dilution law fails for strong electrolytes because

10. For at 298 K with and initial , the direction to reach equilibrium is

11. Which of the following is a weak electrolyte?

12. A catalyst affects equilibrium by

13. Which of the following statements is true about ?

14. The smaller the value of , the

15. A saturated solution of (AgCl) at 25°C has . What is ?

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

17. For a general reaction , the expression for is

18. For gaseous reactions, the equilibrium constant is related to partial pressures by:

19. The expression for the hydrolysis constant of a salt of a weak acid and a strong base is

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

21. The Henderson–Hasselbalch equation is most useful for

22. For the decomposition reaction , the equilibrium constant is derived as:

23. The Arrhenius concept is limited to

24. The of (AgCl) is expressed as

25. The pH of a solution of potassium nitrate is

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

27. Which of the following acts as a Lewis base in the reaction ?

28. If for a gaseous reaction, the relation between and is:

29. A salt formed by a strong acid and a strong base (e.g., ( NaCl )) gives a solution that is

30. Which example illustrates macroscopic constancy but microscopic activity?

1. For a weak acid with small , the degree of ionization is approximately proportional to

2. In the reaction , the conjugate base of is

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

4. Which of the following is not a weak electrolyte?

5. The unit of for the reaction is

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

7. The pH of a (0.001,M) (NaOH) solution is

8. For a gaseous system, the reaction quotient in terms of partial pressure is represented as

9. The conjugate base of is

10. The reaction conditions in the Haber process are typically

11. The pH of a weak acid solution increases upon addition of its salt because

12. For a weak monoprotic acid of initial concentration (C) with , Ostwald’s dilution law gives

13. Which of the following pairs will show a common ion effect?

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

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

16. Which of the following solvents would favor maximum ionization of NaCl?

17. The equilibrium constant for a reaction is expressed as:

18. The optimum temperature for the Contact process is around

19. The unit of for the reaction is

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

21. For a weak acid solution of concentration (C), the hydrogen ion concentration is approximately

22. 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:

23. A salt formed by a strong acid and a strong base (e.g., ( NaCl )) gives a solution that is

24. The pH of a solution of ammonium chloride is

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

26. For , the equilibrium constant in concentration terms is

27. The salt of a weak base and a strong acid shows acidic reaction because

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

29. For , the mass-action expressions are and . At equilibrium, the condition implied is:

30. A catalyst affects equilibrium by

31. When ( Q < K ) for a reaction, the system will

32. The unit of for the reaction is

33. Which statement is true about the relation between and ( C )?

34. For , if initial concentrations of all species are and , the equilibrium will be

35. The common ion effect refers to

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

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

38. The larger the value of , the

39. The degree of hydrolysis ((h)) of a salt of a weak acid and strong base is given by

40. Temperature affects the mass-action constant because:

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

42. Which is a correct necessary condition embedded in the definition of chemical equilibrium for a gas-phase reaction?

43. Removing a product from a reversible reaction mixture will

44. In the same equilibrium, decreasing pressure shifts the reaction

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

46. If for the reaction at 300 K, the value of is

47. If the dielectric constant of a medium increases, the force of attraction between ions

48. If the ionic product (Q) is less than , the solution is

49. For a salt , the relationship between and molar solubility (S) is

50. Among the following, which has the highest (pH) value for 0.1 M solution?