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

2. Ostwald’s dilution law applies to

3. Which statement best captures the scope advantage of the Lewis concept?

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

5. If , the reaction will

6. A solution has . The pOH and pH values are

7. If the hydrogen ion concentration of a solution is , its pH is

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

9. For the reaction , what type of equilibrium is established?

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

11. A strong acid is one that

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

13. The smaller the value of , the

14. The importance of the solubility product lies in its use for

15. When , the reaction

16. In the equilibrium , increasing total pressure shifts equilibrium

17. For the decomposition at equilibrium, which is true?

18. Which of the following reactions illustrates amphoteric behavior of water?

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

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

21. For with and initial , the equilibrium fraction of (A) converted is

22. The molar solubility (S) of a salt (AB) in terms of its solubility product is

23. The equilibrium constant for a gaseous reaction increases with temperature if the reaction is:

24. According to Arrhenius theory, neutralization occurs when

25. A reaction is spontaneous in the forward direction when

26. Which of the following pairs correctly shows the order of increasing ionization?

27. For at equilibrium, the concentration form predicted by the mass-action law is:

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

29. If for a certain gaseous system and the calculated , the direction of reaction is

30. The pH of ammonium acetate depends on

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

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

3. The common ion effect is an application of

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

5. For the decomposition reaction , the unit of is

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

7. Buffers are important in analytical chemistry because they

8. The hydrolysis constant of at 25°C is . If , then the base dissociation constant of is approximately

9. The pH of a solution of potassium nitrate is

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

11. The salt formed from (NaOH) and (HCl) will have a pH value of

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

13. In the equilibrium (water–gas reaction), the pressure-form expression is

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

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

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

17. At chemical equilibrium for a reversible reaction in a closed system, which statement is correct?

18. The ability of a solvent to dissolve ionic compounds depends mainly on its

19. For liquid–vapour equilibrium of benzene at , which observation verifies molecular exchange despite constant vapour pressure?

20. The equilibrium condition can be derived from the expression

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

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

23. Which of the following acids is weak?

24. For , with and initial , equilibrium is

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

26. For the reaction with and initial concentrations , , the equilibrium concentration of (B) is

27. For an endothermic reaction, decreasing temperature causes

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

29. A solution has . The pOH and pH values are

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

31. Ostwald’s dilution law applies to

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

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

34. At the melting point of a pure solid in a closed system, solid–liquid equilibrium is characterized by:

35. The pH of a solution of ammonium chloride is

36. In the reaction , the conjugate base of is

37. The reaction conditions in the Haber process are typically

38. Henry’s law for a sparingly soluble gas in a liquid is correctly written as:

39. Which of the following salts forms a neutral solution in water?

40. The degree of ionization of a weak monoprotic acid (HA) in water is defined as

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

42. If the of is , then the of its conjugate acid is

43. The pH of a solution of sodium acetate is

44. In the Haber process, lowering the temperature will

45. A beaker with solid and saturated solution at shows constant conductivity. Which experiment proves dynamic equilibrium at the solid–solution boundary?

46. According to Arrhenius theory, neutralization occurs when

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

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

49. For an endothermic reaction with , increasing temperature typically

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