BMI_Lab3Buffers - Biomed I Lab 3 pH, Buffers, and Titration...

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Biomed I Lab 3 pH, Buffers, and Titration
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Objectives To understand the concepts of ionization of acids and bases and of equilibrium biochemical solutions. To understand the concepts of pH and buffer. To understand Henderson Hasselbach Equation and use it to calculate drug ionization and drug absorption.
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Br Ø nsted-Lowry theory Acid: a substance that donates* a proton * refers to a hydrogen atom which has lost its electron and now has a + charge Base: a substance which accepts a proton Electrolyte: a substance that dissolves in water to produce ions (charged particles)
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Examples of acids and bases Consider the equations below: NH 3 + HCL NH 4 + + Cl - H 2 O + HCl H 3 O + + Cl - NH 3 + H 2 O NH 4 + + OH - Can you determine which is the acid and base in each of the equations? What do you note about water?
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Examples of acids and bases NH 3 (base) + HCL (acid) NH 4 + + Cl - H 2 O (base) + HCl (acid) H 3 O + + Cl - NH 3 (base) + H 2 O (acid) NH 4 + + OH - Water is amphoteric. It can act as either an acid or base NH 3 (base) + HCL (acid) NH 4 + (conj acid) + Cl - (conj base) The equation above shows conjugate acid and base pairs.
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Strengths of Acids and Bases HCl + H 2 O H 3 O + + Cl - HCl is a strong acid and the equation goes almost completely to the right. Similarly, NaOH is a strong base NaOH + H 2 O Na + + OH - In contrast, a weak acid (HA), goes only a few percent to the right HA + H 2 O H 3 O + + A - When no further dissociation occurs, the reaction is at equilibrium
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BMI_Lab3Buffers - Biomed I Lab 3 pH, Buffers, and Titration...

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