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

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

3. Which statement about a catalyst and equilibrium is correct?

4. A solution with has hydrogen ion concentration

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

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

7. Consider in a closed vessel. The equilibrium constant depends on

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

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

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

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

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

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

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

15. In the Haber process, lowering the temperature will

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

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

18. Which of the following is a basic buffer?

19. If , the hydroxide ion concentration is

20. For the reaction , the relation between and will be

21. The units of for are

22. In dissolution equilibrium of a solid in a liquid (at fixed (T)), which action increases the amount of undissolved solid without changing solubility?

23. If at 298 K for with initial and , the reaction extent toward (B) at equilibrium will be

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

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

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

27. For the gaseous reaction , the relation between and is given by

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

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

30. The law of mass action at equilibrium for states that the ratio is:

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

2. The relation is valid only when

3. Strong bases are those that

4. For an endothermic reaction, increasing temperature shifts equilibrium

5. A salt of a weak acid and a strong base gives a solution that is

6. The Henderson–Hasselbalch equation is most useful for

7. For the heterogeneous equilibrium , the mass-action law gives:

8. The equilibrium condition can be derived from the expression

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

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

11. The unit of for the reaction is

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

13. For at , . If initially and , the reaction will:

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

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

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

17. Which of the following is a weak base?

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

19. In the Haber process , increasing the pressure will

20. The common ion effect is an application of

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

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

23. The degree of ionization of an electrolyte is higher in solvents having

24. For the decomposition reaction , the unit of is

25. For , if initial and , the equilibrium is

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

27. A salt formed by a strong acid and a weak base gives a solution that is

28. The (pH) of a (0.2,M) solution is

29. Ionization of weak acids like acetic acid increases when

30. The dissociation of is suppressed by adding

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

32. The pH of a solution of potassium nitrate is

33. The (pH) of a salt solution formed by a weak base and strong acid is given by

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

35. Which of the following best represents the neutralization of an acid and a base according to Arrhenius?

36. When in an acidic buffer, the pH equals

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

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

39. 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

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

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

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

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

44. Which condition is essential for establishing chemical equilibrium in the laboratory?

45. For the reaction , the units of are

46. The dielectric constant of water at 25°C is approximately

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

48. The pH of an acidic buffer can be calculated using

49. For the reaction , the value of is

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