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

2. If for a reaction and , the reaction will

3. The solubility product differs from the ionic product in that

4. According to Arrhenius theory, neutralization occurs when

5. A weak acid is characterized by

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

7. The degree of ionization of a weak acid in the presence of its strong electrolyte salt is

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

9. In the Haber process , increasing the pressure will

10. For gases behaving ideally, the mass-action expression in terms of partial pressures for is:

11. For the decomposition reaction , the unit of is

12. The product of and ( C ) for a weak acid at a given temperature is

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

14. Temperature generally affects degree of ionization of weak acids/bases by

15. The relation between force of attraction ( F ) and dielectric constant ( D ) is

16. Identify the Lewis acid in the reaction .

17. The reaction conditions in the Haber process are typically

18. A closed flask containing water at shows constant vapour pressure. Which measurement provides direct evidence that liquid–vapour equilibrium is dynamic?

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

20. The pH of a basic buffer is given by

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

22. For a weak base ( BOH ), Ostwald’s dilution law is expressed as

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

24. Which of the following is a weak base?

25. In a closed container at fixed (T), liquid–vapour equilibrium is reached when:

26. 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

27. The conjugate acid of a strong base is

28. The Contact process involves the oxidation of to : . Increasing pressure will

29. For a system with , , the sign of is

30. Which of the following statements about and is true?

1. The molar solubility (S) of a salt in terms of is

2. Decreasing pressure on a gaseous equilibrium mixture causes the equilibrium to shift

3. The pair is an example of

4. When a solution is just saturated with a salt, the ionic product is

5. For a weak base ( BOH ), Ostwald’s dilution law is expressed as

6. Which of the following statements is true regarding the common ion effect?

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

8. Which of the following statements is true for homogeneous equilibrium systems?

9. When temperature increases, the numerical value of relative to :

10. A salt derived from a weak acid and a weak base gives a solution that is

11. For a system at constant (T) and (P), a spontaneous process always has

12. A solution with has hydrogen ion concentration

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

14. The smaller the value of , the

15. The reaction quotient for is given by

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

17. In a mixture of acetic acid and sodium acetate, the concentration of ions is governed mainly by

18. According to Arrhenius theory, neutralization occurs when

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

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

21. Which interaction most clearly illustrates Lewis acidity of a metal cation in solution?

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

23. The ionization of acetic acid decreases on addition of sodium acetate because

24. For a system with , , the sign of is

25. For a weak acid solution, if concentration decreases 100 times, the degree of ionization increases approximately by a factor of

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

27. Consider with at 298 K. Starting from , the expected equilibrium is

28. The common ion effect refers to

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

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

31. Which of the following statements is true about ?

32. Which of the following is the best Lewis base toward ?

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

34. In a homogeneous equilibrium, changing the total pressure affects the equilibrium position if

35. In the reaction , if and , the reaction will

36. According to Le Chatelier’s principle, if the concentration of a reactant is increased, the system will

37. Strong bases are those that

38. For the reaction , the unit of is

39. Temperature affects the mass-action constant because:

40. The solubility product differs from the ionic product in that

41. A closed flask containing water at shows constant vapour pressure. Which measurement provides direct evidence that liquid–vapour equilibrium is dynamic?

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

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

44. The pH of a solution of potassium nitrate is

45. When , the reaction

46. Which of the following salts gives an acidic solution in water?

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

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

49. The relationship between pH and pOH at 25°C is

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