Pharmaceutical Analysis-1 1st Semester MCQ Introduction To Pharmaceutical Analysis-Most Important

Introduction To Pharmaceutical Analysis Most Important 50 MCQs with Solutions

Pharmaceutical Analysis-1 1st Semester MCQ Introduction To Pharmaceutical Analysis


Multiple Choice Questions

1. Molality(M) of a solution is defined as:
a. Number of gram molecular wt. of solute/vol. of solution in litre
b. Number of gram molecular wt. of solute/wt. in one kg
c. Number of gram equivalent wt. of solute /vol. of solution in litre
d. None of the above

2. Molality (m) of a solution is defined as:
a. Number of gram molecular wt. of solute/vol. of solution in litre
b. Number of gram molecular wt. of solute/wt. in one kg
c. Number of gram equivalent wt. of solute/ volume of solution in litre
d. None

3. Normality of a solution is defined as:
a. Number of gram molecular wt. of solute/vol. of solution in litre
b. Number of gram molecular wt of solute/wt in one kg
c. Number of gram equivalent of wt. of solute/vol. of solution in litre
d. None of the above

4. Mole fraction is defined as:
a. The ratio of the volume of the solute in ml to 100 ml of the solution
b. The number of moles of one component divided by total the number of moles of all components in the solution
c. The number of grams of a constituent in 100 ml of solution or liquid preparation
d. The mass of the element or solute (gm) in 100 gm of compound

5. Volume/volume percentage (v/v%) is:
a. The ratio of the volume of the solute in ml to 100 ml of the solution
b. The number of moles of one component divided by total the number of moles of all components in the solution
c. The number of grams of a constituent in 100 ml of solution or liquid preparation
d. The mass of the element or solute (gm) in 100 gm of compound

6. Mass percentage (w/w %) is:
a. The ratio of the volume of the solute in ml to 100 ml of the solution
b. The number of moles of one component divided by total the number of moles of all components in the solution
c. The number of grams of a constituent in 100 ml of solution or liquid preparation
d. The mass of the element or solute (gm) in 100 gm of compound

7. Weight-in-volume percentage (w/v%) is:
a. The ratio of the volume of the solute in ml to 100 ml of the solution
b. The number of moles of one component divided by total the number of moles of all components in the solution
c. The number of grams of a constituent in 100 ml of solution or liquid preparation
d. The mass of the element or solute (gm) in 100 gm of compound

8. Parts per million (ppm) is:
a. The number of parts of the substance per 1000000 parts of the total mass
b. The number of parts of the substance per 1000000000 parts of the total mass
c. The number of parts of the substance per 100000 parts of the total mass
d. The number of parts of the substance per 100000 parts of the total mass

9. Parts per billion (ppb) is:
a. The number of parts of the substance per 1000000 parts of the total mass
b. The number of parts of the substance 1000000000 parts of the total mass
c. The number of parts of the substance per 100000 parts of the total mass
d. The number of parts of the substance per 10000 parts of the total mass

10. Equivalent weight (EW) of substance is:
a. Molecular weight of acid/basicity of acid
b. Molecular weight of base/acidity of base
c. Molecular weight of salt/charge present on ionic form
d. All of the above

11. Equivalent weight (EW) of HCI is:
a. 36.5
b. 49
c. 58.5
d. 31

12. Equivalent weight (EW) of H₂SO4is:
a. 36.5
b. 49
c. 58.5
d. 31

13. Equivalent weight (EW) of NaOH is:
a. 36.5
b. 40
c. 58.5
d. 31

14. Equivalent weight (EW) of KOH is:
a. 36.5
b. 49
C. 58.5
d. 56

15. Equivalent weight (EW) of NaCl is:
a. 36.5
b. 49
C. 58.5
d. 56

16. Equivalent weight (EW) of KMO, in acidic medium is:
a. 31.61
b. 36.5
c. 52.68
d. 58.5

17. Equivalent weight (EW) of KMO, in basic medium is:
a. 31.61
b. 36 5
c. 52.68
d. 58.5

18. HCI is:
a. Monoprotic acid
b. Monoprotic base
c. Diprotic acid
d. Diprotic base

19. H₂SO4 is:
a. Monoprotic acid
b. Monoprotic base
c. Diprotic acid
d. Diprotic base

20. Sodium Hydroxide (NaOH) is:
a. Monoprotic acid
b. Monoprotic base
c. Diprotic acid
d. Diprotic base

21. Carbonate ion (CO3²-) is:
a. Monoprotic acid
b. Monoprotic base
c. Diprotic acid
d. Diprotic base

22. Ionic product of water (KW) has value… at 25°C:
a. 1.0×10-¹⁰
b. 1.0×10‐¹⁴
c. 1.0×10-¹⁶
d. 1.0×10-⁷

23. The unit of Kw is:
a. Mole ¹litre-1
b. Mole ²litre²
c. Mole³litre³
d. None

24. 1M of HCI is equivalent to:
a. 1N HCl
b. 2N HCI
c. 0.5N HCl
d. 2 M HCI

25. 1M of H₂SO4 is equivalent to:
a. 1 N H₂SO4
b. 2N H₂SO4
c. 0.5 N H₂SO4
d. 4 N H₂SO4

26. The number of ml of a liquid solute per 100 ml of solution is:
a. % W/V
b. %V/V
c. PPM
d. Strength

27. Normality of acid is=
a. Molarity×Basicity
b. Molarity×Acidity
c. Molality×Acidity
d. Molality×Basicity

28. Normality of bases =
a. Molarity x Basicity
b. Molarity x Acidity
c. Molality × Acidity
d. Molality x Basicity

29. Relation between normality and molarity is:
a. Normality = Molarity × n
b. Molarity = Normality × n
c. Normality × Molarity = n
d. Normality + Molarity = n

30. For ionic solid solution molarity (M) may be called as:
a. Molality (m)
b. Mormality(N)
c. Formality (F)
d. Concentration(C)

31. Buffer solution consists of:
a. Weak acid and its conjugate base
b. Weak acid + Strong base
c. Weak acid + weak base
d. All of the above

32. The pH of pure water is neutral, the best
explanation for this is:
a. The pH of pure water is 7
b. In pure water the concentration of H* and OH‐ are same
c. Water do not contain free H* or OH ions
d. water will never ionize

33. After neutralization reaction between strong acid and strong base, what will be formed?
a. Acidic salt
b. Basic salt
c. Neutral salt
d. All of the above

34. After neutralization reaction between strong acid and weak base, what will be formed?
a. Acidic salt
b. Basic salt
c. Neutral salt
d. All of the above

35. After neutralization reaction between weak acid and strong base, what will be formed?
a. Acidic salt
b. Basic salt
c. Neutral salt
d. All of the above

36. After neutralization reaction between weak acid and weak base, what will be formed?
a. Acidic salt
b. Basic salt
c. Neutral salt
d. All of the above

37. Titrant is:
a. The solution of which concentration is accurately known
b. The substance whose concentration is to be determined
c. The substance which is added to detect the endpoint
d. The substance which is added to the solution to induce the chemical reaction

38. Titrand is:
a. The solution whose concentration is accurately known
b. The substance whose concentration is to be determined
c. The substance which is added to detect the end point
d. The substance which is added to the solution to induce the chemical reaction

39. Equivalence (stoichiometric) point is:
a. The point at which the completion of the reaction occurs
b. The point at which completion of reaction is practically observed
c. Both a and b
d. The point at which indicator is to be added

40. End point refers to:
a. The point at which the completion of the reaction occurs
b. The point at which completion of reaction is practically observed
c. Both a and b
d. The point at which indicator is to be added

41. Primary standard refers to:
a. A substance whose actual concentration is found by comparing with a primary standard
b. A compound of sufficient purity from which a standard solution can be prepared by direct weighing
c. A solution prepared from a primary standard substance in a known volume of the solution.
d. A solution whose concentration is known after standardization with primary standard

42. Secondary standard refers to:
a. A substance whose actual concentration is found by comparing with a primary standard
b. A compound of sufficient purity from which a standard solution can be prepared by direct weighing
c. A solution prepared from a primary standard substance in a known volume of the solution.
d. A solution whose concentration is known after standardization with primary standard

43. Which of the following is primary standard?
a. Na2S2O3
b. NaCl
c. C2H2O4
d. Both ‘a’ and ‘b’

44. Which is NOT a primary standard?
a. Na₂S₂O3
b. NaCl
c. Na₂B407
d. KCI

45. Which of the following is secondary standard?
a. C2H2O4
b. NaCl
c. Na2B4O7
d. KCI

46. Which of the following is NOT a theory of indicator?
a. Ostwald’s Theory
b. Arrhenius theory
c. Quinonoid Theory
d. Physiochemical theory

47. According to Ostwald’s theory, indicators are:
a. Weak acid
b. Strong acid
c. Weak base
d. Both a and c

48.pH range of methyl orange is:
a. 3.1-4.4
b. 2.8-4.4
c. 4.2-6.3
d. 8.3-10.5

49. pH range of methyl red is:
a. 3.1-4.4
b. 2.8-4.4
c. 4.4-6.2
d. 8.3-10.5

50. pH range of phenolphthalein is:
a. 3.1-4.4
b. 2.8-4.4
c. 4.2-6.3
d. 8.3-10


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