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

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

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

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

5. For an endothermic reaction with , increasing temperature typically

6. The pH of a solution of potassium nitrate is

7. The (pH) of a (0.01,M) (NaOH) solution is

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

9. The reversible decomposition of calcium carbonate is an example of:

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

11. If an inert gas is added at constant pressure, the equilibrium shifts

12. When a reversible reaction attains equilibrium, what remains constant?

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

14. If for a reaction and , the reaction will

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

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

17. If an inert gas is added at constant volume to a gaseous equilibrium mixture, the equilibrium position

18. The conjugate acid of the base is

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

20. For , if and initial concentrations , the equilibrium is approximately

21. The pOH of a solution is defined as

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

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

24. In a buffer containing and , the pH is calculated using

25. Which statement about buffers is true?

26. Which of the following is an example of an acidic buffer?

27. The base ionization constant expresses

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

29. When in a basic buffer, the pH equals

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

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

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

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

4. The pH of a basic buffer is given by

5. The conjugate base of a strong acid is always

6. The unit of for the reaction is

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

8. The ionization equation for acetic acid is

9. For a weak acid with and , the degree of ionization is

10. In predicting reaction direction, the value of or depends on

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

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

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

14. For a gaseous equilibrium involving equal moles of reactants and products, a change in pressure

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

16. The variation of the degree of ionization with concentration (( C )) for a weak electrolyte is represented by

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

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

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

20. The Arrhenius concept is limited to

21. When a reversible reaction attains equilibrium, what remains constant?

22. The reversible decomposition of calcium carbonate is an example of:

23. If an inert gas is added at constant volume to a gaseous equilibrium mixture, the equilibrium position

24. A catalyst affects equilibrium by

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

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

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

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

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

30. Consider the reversible reaction . If the concentration of is increased at equilibrium, what happens initially?

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

32. Le Chatelier’s principle states that when a system at equilibrium is subjected to a change,

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

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

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

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

37. In the Haber process, the catalyst used is

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

39. For , the correct expression is:

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

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

42. The optimum temperature for the Contact process is around

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

44. The principle of microscopic reversibility implies that:

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

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

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

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

49. Which of the following acids is weak?

50. When pressure on a gaseous equilibrium is increased, the system shifts