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

3. If , the hydroxide ion concentration is

4. The of (AgCl) is expressed as

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

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

7. For , the correct expression is:

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

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

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

11. Which statement about buffers is true?

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

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

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

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

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

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

18. The derivation of from assumes that:

19. When in an acidic buffer, the pH equals

20. The unit of for the reaction is

21. For , the value of at temperature (T) is governed by

22. In at equilibrium, , , and . What value provides evidence of dynamic equilibrium through rate equality?

23. The relationship between hydrolysis constant , degree of hydrolysis (h), and concentration (C) for a salt of a weak acid and strong base is

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

25. For most ionic solids dissolving endothermically in water , increasing temperature will:

26. In the Contact process, lowering the temperature increases the yield of because the reaction is

27. The conjugate acid of a strong base is

28. According to the Brønsted–Lowry concept, a base is a substance that

29. According to Arrhenius, an acid is a substance that

30. The reaction quotient is defined as

1. The common ion effect refers to

2. The principle of microscopic reversibility implies that:

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

4. The conjugate base of a strong acid is always

5. For , the value of at temperature (T) is governed by

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

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

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

9. In a homogeneous equilibrium, all the reactants and products are present in

10. The unit of for the reaction is

11. Strong bases are those that

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

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

14. Which observation best demonstrates that equilibrium is dynamic rather than static in a saturated solution of sugar at constant (T)?

15. For a general reaction , the expression for is

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

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

18. For most ionic solids dissolving endothermically in water , increasing temperature will:

19. In qualitative analysis, group II cations like , , and are precipitated as sulfides in acidic medium because

20. The relationship between hydrolysis constant , degree of hydrolysis (h), and concentration (C) for a salt of a weak acid and strong base is

21. The dielectric constant of a solvent affects the ionization of an electrolyte because it

22. The common ion effect is an application of

23. The relation between hydrogen ion concentration and the initial concentration ( C ) of a weak acid is

24. According to Ostwald’s dilution law, for a weak acid ( HA ), the dissociation constant is given by

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

26. In the reaction , the conjugate base of is

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

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

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

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

31. A reaction is spontaneous in the forward direction when

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

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

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

35. The concept of microscopic reversibility is supported by which scientific law?

36. For an endothermic reaction with , increasing temperature typically

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

38. The ionization equation for acetic acid is

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

40. 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:

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

42. Which change decreases the solubility of oxygen in water at equilibrium?

43. Which of the following compounds cannot be classified as an Arrhenius acid or base?

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

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

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

47. Which of the following is a correct example of physical equilibrium?

48. Which statement about buffers is true?

49. For , the correct expression for is:

50. Which of the following graphs best represents Ostwald’s dilution law?