UNIT- 2 Pharmaceutical Inorganic Chemistry PPT/PDF

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UNIT-2 Pharmaceutical Inorganic Chemistry PPT/PDF (BP-104T, Semester I)

Download a PPT or PDF presentation covering UNIT-2 of Pharmaceutical Inorganic Chemistry (Subject Code: BP-104T) for Semester I students. This resource covers Acids, Bases and Buffers (including buffer equations, buffer capacity, pharmaceutical systems, and isotonic solutions), Major extra and intracellular electrolytes, and Dental products. Includes information on Sodium chloride, Potassium chloride, Calcium gluconate, Oral Rehydration Salt (ORS), and the role of fluoride. Pharmaceutical Inorganic Chemistry Notes / MCQs / PPT / PDF available.

Keywords: Pharmaceutical Inorganic Chemistry, Acids, Bases, Buffers, Electrolytes, Dental Products, Buffer Equations, Isotonicity, Sodium Chloride, Potassium Chloride, Calcium Gluconate, Oral Rehydration Salt (ORS), Fluoride, BP-104T, Semester I, PPT, PDF

Unit 2: Mastering Acids, Bases, Electrolytes, and Dental Components in Pharmaceutical Inorganic Chemistry

Unit 2 of Pharmaceutical Inorganic Chemistry (BP-104T) builds upon foundational concepts to explore the vital roles of acids, bases, buffers, and electrolytes in pharmaceutical systems and the human body. It also introduces the inorganic chemistry relevant to dental products. This guide will help you navigate this content effectively.

Key Topics and Concepts:

1. Acids, Bases, and Buffers:
   • Theories: Arrhenius, Bronsted-Lowry, and Lewis definitions.
   • Buffer Systems: Solutions that resist changes in pH. Crucial for maintaining drug stability and physiological pH.
   • Buffer Equations: The Henderson-Hasselbalch equation (pH = pKa + log([A-]/[HA])) is key. Understand how to use it to calculate buffer pH and predict buffer behavior.
   • Buffer Capacity: The ability of a buffer to resist pH changes. Affected by concentration and the ratio of acid to base.
   • Pharmaceutical Systems: Common buffer systems used in formulations (e.g., phosphate, acetate, citrate buffers).
   • Preparation and Stability: Factors affecting buffer stability (temperature, light, ionic strength).
   • Buffered Isotonic Solutions: Crucial for injectable and ophthalmic products to prevent cell damage.
   • Tonicity Measurements: Methods to measure tonicity (e.g., freezing point depression).
   • Adjusting Isotonicity: Calculations for adding substances (e.g., NaCl, dextrose) to achieve isotonicity.
2. Major Extra- and Intracellular Electrolytes:
   • Physiological Functions: Roles of Na+, K+, Ca2+, Cl-, HCO3- in:
     • Fluid balance
     • Nerve impulse transmission
     • Muscle contraction
     • Acid-base balance
   • Replacement Therapy: Understanding when and how to use:
     • Sodium Chloride (NaCl)*: For hyponatremia (low sodium).
     • Potassium Chloride (KCl): For hypokalemia (low potassium).
     • Calcium Gluconate (Ca Gluconate)*: For hypocalcemia (low calcium).
     • Oral Rehydration Salt (ORS): For dehydration due to diarrhea/vomiting. Know its components.
   • Acid-Base Balance: How the body maintains blood pH (7.35-7.45) via:
     • Buffers
     • Respiratory system (CO2 regulation)
     • Renal system (HCO3- regulation)
3. Dental Products:
   • Dentifrices (Toothpastes): Components and their roles:
     • Abrasives: Cleaning and polishing (e.g., calcium carbonate).
     • Fluoride: Prevents dental caries.
     • Surfactants: Foaming agents.
     • Humectants: Prevent drying.
   • Fluoride and Dental Caries: Mechanism by which fluoride strengthens enamel.
   • Desensitizing Agents: Examples like potassium nitrate.
   • Specific Compounds: Functions of Calcium Carbonate, Sodium Fluoride, and Zinc Eugenol Cement in dental applications.

Study Strategies:

1. Memorize Key Equations: Henderson-Hasselbalch is essential.
2. Electrolyte Profiles: Create tables summarizing each electrolyte's:
   • Normal range
   • Functions
   • Causes of imbalances
   • Symptoms of imbalances
   • Treatment strategies
3. Practice Calculations: Work through problems involving:
   • Buffer pH
   • Isotonicity adjustments
   • Electrolyte replacement dosages
4. Relate to Clinical Scenarios: Think about how these concepts apply to real patients.

Potential Exam Questions:

• Explain how a buffer solution resists changes in pH.
• Calculate the pH of a buffer containing [HA] and [A-] given the pKa.
• Describe the steps involved in making an isotonic solution of a given drug.
• What are the symptoms of hypokalemia? How is it treated?
• Explain the role of fluoride in preventing tooth decay.
• List the components of ORS and explain why each is important.
• How does the respiratory system contribute to acid-base balance?

By understanding these concepts, mastering the equations, and relating them to clinical applications, you can succeed in Unit 2 of Pharmaceutical Inorganic Chemistry.

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