Pharmaceutical Analysis – I Important Questions with Answers – Unit Wise Guide (B pharma 1st semester solved)

Pharmaceutical Analysis – I Important Questions with Answers – Unit Wise Guide (B pharma 1^st semester solved)

Section A

Unit-I Questions

1. Calculate the normality of 20 g NaOH for a 100 ml solution.
2. Calculate the significant figures of 0.1 × 0.2 and 0.1 ÷ 0.2 up to three digits.
3. Define normality and explain how to prepare 0.1 N NaOH solution for 100 ml.
4. Differentiate between primary and secondary standards.
5. What do you mean by normality?
6. Define standard solution and its types.
7. Describe the fundamentals of volumetric analysis.
8. Write a note on significant figures.
9. Define mole and molarity.
10. Calculate the normality for 100 g of NaOH in 500 ml solution.
11. Differentiate between accuracy and precision.
12. Define the limit test.
13. How can you prepare a 1 molar oxalic acid solution?
14. Explain the principle behind the limit test of chlorides.

Unit-II Questions

1. Define acid and base according to Bronsted-Lowry theory.
2. Explain how phenolphthalein behaves in acidic and basic mediums.
3. Write about acid-base indicators.
4. Differentiate between acid and base.
5. What is a universal indicator? Give examples.
6. What is non-aqueous titration?
7. Explain acid and base according to Arrhenius theory.
8. Write about various solvents used in non-aqueous titration.
9. What do you understand from neutralization curves?

Unit-III Questions

1. What are masking and demasking agents?
2. Differentiate between co-precipitation and post-precipitation.
3. Write the principle of Mohr’s method.
4. Write the formula of EDTA.
5. Define digestion and Ostwald ripening.
6. What is the modified Volhard method? Give examples.
7. Explain the principle of gravimetric analysis.
8. Define a metal ion indicator with suitable examples.
9. Define diazotization.
10. Explain the principle of Volhard’s method.
11. How will you estimate calcium gluconate?

Unit-IV Questions

1. Oxidation involves the loss of electrons, and reduction involves the gain of electrons.
2. Define oxidizing and reducing agents.
3. Describe the mechanism of starch-KI paste as an external indicator.
4. Define iodimetry and iodometry.
5. Explore the term dichrometry.
6. Discuss the role of indicators in titrations.

Unit-V Questions

1. What is Ohm’s law? Define specific resistance.
2. Define protogenic and protophilic solvents.
3. What is polarography?
4. Differentiate between leveling and differentiating effects of solvents.
5. Define Kohlrausch’s law.
6. Explain the different types of current used in polarography.
7. What are electrochemical methods of analysis?
8. Write about Ilkovic action.
9. Define mole fraction.

Section B

Unit-I Questions

1. Write about various sources of errors.
2. Describe the various types of errors and methods for minimizing them.
3. Discuss the methods of expressing concentration in detail.
4. What are the different methods to express the concentration of a solution?

Unit-II Questions

1. Classify acid-base titrations. Provide an example of a strong acid and strong base titration.
2. Explain the significance of non-aqueous titrations. Differentiate between “levelling solvents” and “differentiating solvents” with suitable examples.
3. What is an acid-base indicator? Explain the theory of indicators.

Unit-III Questions

1. Give the principle and steps involved in gravimetric analysis.
2. Discuss in detail Mohr’s method and Volhard’s method.
3. Discuss Fajan’s method of precipitation titration. Explain co-precipitation and post-precipitation.
4. Discuss the basic principle, methods, and application of diazotization titration.

Unit-IV Questions

1. Explain the standardization of KMnO₄ using sodium oxalate.
2. What is redox titration? Write a short note on redox curves.
3. Explain the theory of redox titrations and provide the concept of oxidation and reduction.

Unit-V Questions

1. Provide the construction and working of reference electrochemical cells: standard hydrogen, silver chloride electrode, and calomel electrode.

Section C

Unit-I Questions

1. What is the role of quantitative analysis in quality control?
2. What is error? Differentiate between determinate and indeterminate errors.
3. Discuss the preparation and standardization of Oxalic acid or Sodium hydroxide.
4. Define limit test and describe the limit test of chloride in detail.
5. Classify errors and suggest ways to minimize them.
6. Outline the various techniques of analysis used in pharmaceuticals.
7. Describe the source of impurities in medicinal agents.

Unit-II Questions

1. Discuss the types of solvents used in non-aqueous titration.
2. What are indicators? Discuss the theory of indicators.
3. What is non-aqueous titration? Discuss the advantages and disadvantages of non-aqueous titration.
4. What are mixed indicators? Give examples and their advantages.
5. State the modern concept of acids and bases.
6. Derive the Henderson-Hasselbalch equation for a weak acid and its salt.
7. Write the theory of acid-base titrations.
8. Write a note on estimation of boric acid.
9. Write a note on alkalimetry and acidimetry.
10. Describe the types of non-aqueous solvents.
11. Discuss various neutralization curves in acid-base titrations.

Unit-III Questions

1. Discuss the types of complexometric titrations.
2. Define digestion or Ostwald ripening and give its significance in gravimetric analysis.
3. What is pM indicator? Discuss the theory of pM indicator.
4. Discuss the preparation and standardization of 0.1 N ceric sulphate solution.
5. What are the various steps involved in gravimetric analysis?
6. Write a note on Fajan’s method.
7. How is co-precipitation different from post-precipitation?
8. Discuss the estimation of Barium sulphate.
9. Describe masking and demasking reagents in complexometric titration.

Unit-IV Questions

1. Write a short note on Iodimetry and Iodometry.
2. Describe the concept of oxidation and reduction.
3. Write the principle and give an example of redox titration.

Unit-V Questions

1. Explain the types of conductometric titrations in detail.
2. Explain the mechanism of a dropping mercury electrode (DME).
3. Illustrate the principle, instrumentation, and applications of conductometry.
4. Draw the construction of an electrochemical cell. Describe the working of the standard hydrogen electrode and standard calomel electrode.
5. Write the methods to determine the endpoint of potentiometric titration.