Unit 2: Biochemistry Chapter 2

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Presentation transcript:

Unit 2: Biochemistry Chapter 2 pH Scale Unit 2: Biochemistry Chapter 2

pH Scale In an aqueous solution some water and other molecules tend to ionize Ex: H2O  H+ (hydrogen ion) and OH- (hydroxide ion) The concentration of H+ is used to calculate pH The pH scale ranges from 0.1 - 14

Acids Solution that has a high concentration of H+ ions Chemical formula usually begins with H Has a pH of 6.9 or less Examples: HCl, H2SO4, HNO3, HCH3O3

Bases Solution that has a low concentration of H+ (high concentration of OH-) Chemical formula usually ends with OH Has a pH of 7.1 or higher Examples: NaOH, KOH, Mg(OH)2

Water Water is neutral (pH = 7) If an acid is added to water…? If a base is added to water…?

Buffers Substance that keeps the pH relatively stable when an acid or base is added. Most biological solutions have a natural ability to buffer: blood, milk, saliva, egg white Chemical reactions in living things depend on a stable pH

Additional Resources http://www.youtube.com/watch?v=Xeuyc55LqiY