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213 PHC Pharmaceutical Analytical Chemistry

213 PHC Pharmaceutical Analytical Chemistry. 1 st lecture Dr. MOna Alshehri. Introduction. Chemicals make up everything we use or consume. The knowledge of the chemical composition of a substance is important in our daily lives.

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213 PHC Pharmaceutical Analytical Chemistry

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  1. 213 PHCPharmaceutical Analytical Chemistry 1st lecture Dr. MOnaAlshehri

  2. Introduction

  3. Chemicals make up everything we use or consume. • The knowledge of the chemical composition of a substance is important in our daily lives. • Analytical chemistry plays an important role in all aspects (agricultural, clinical, environmental, forensic, manufacturing, and pharmaceutical). • Analytical chemistry consists of qualitative and quantitative analysis: • Qualitative analysis tells us what chemicals are present. • Quantitative analysis tells us how much.

  4. Acid-Base Equilibria (1)(1) Gary D. Christian, Analytical Chemistry, 6th edition.

  5. By the end of this lecture the student should be able to: • Describe the common acid-base theories. • Classify substances as acids and bases. • Understand acid-base equilibria in water.

  6. Acid-Base Theories

  7. Arrhenius Theory: Acid HA + H2O  H3O+ + A- Base B + H2O  BH+ + OH-

  8. Bronsted-Lowry Theory: acid = H+ + base Acid  donate a proton Base  accept a proton

  9. Lewis Theory: Electronic theory of acids and bases. Acid  accept electron pair Base  donate electron pair AlCl3 + :OR2  Cl3Al:OR2

  10. Identify the acid and the base: • HCl + NaOH → NaCl + H2O • NH3 + H2O → NH4+ + OH− • C6H5NH2 + CH3COOH  C6H5NH3++ CH3COO- • CH3COOH + NH3 → NH+4 + CH3COO−

  11. Acid-Base Equilibria in Water

  12. When an acid or base is dissolved in water, it will dissociate, or ionize. • A strong acid or base is completely ionized. • A weak acid or base is partially ionized.

  13. e.g. CH3COOH  H+ + CH3COO- Ka = [H+] [CH3COO-] / [CH3COOH]

  14. H2O  H+ + OH- Kw = [H+] [OH-] Kw = 1 x 10-14

  15. Questions?

  16. Summary: • Acid-Base Theories. • Arrhenius • Bronsted-Lowry • Lewis • Acid-Base Equilibria in water.

  17. Common names of some chemical compounds:

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