2.4 Cells Have an Optimum pH

Cells Have an Optimum pH

  • Importance of H+ Ions

    • H+ ions (protons) play a critical role in living systems.

    • Imbalance in H+ concentration can disrupt molecular shapes and cellular functions, potentially leading to cell death.

  • Source of H+ Ions

    • Pure water can spontaneously dissociate into H+ and OH- ions:

      • H₂O ⇌ H+ + OH-

    • In pure water, concentrations of H+ and OH- ions are equal (neutral solution).

Acids and Bases

  • Acids

    • Substances that increase the concentration of H+ ions in a solution, lowering the pH.

    • Examples:

      • Hydrochloric acid (HCl)

      • Vinegar and lemon juice

    • Reaction with water: HCl → H+ + Cl-

  • Bases

    • Substances that increase the concentration of OH- ions or decrease H+ ions, raising the pH.

    • Common bases include:

      • Baking soda

      • Sodium hydroxide (NaOH): NaOH → Na+ + OH-

  • Neutralization

    • When mixed, acids and bases neutralize each other:

      • Acid releases protons; base absorbs H+ or releases OH-.

pH Scale

  • Measuring Acidity and Basicity

    • pH scale ranges from 0 to 14:

      • 7 is neutral (pure water).

      • pH < 7 indicates acidic solutions.

      • pH > 7 indicates basic solutions.

    • Strongly acidic solutions are closer to 0; strongly basic solutions are closer to 14.

H+ Concentration and pH Relationship

High H+ Concentration

  • 10⁰ HCl (strong acid) has the highest H+ concentration.

  • Acids have lower pH values:

    • Stomach acid (pH 1.6-1.8)

    • Lemon juice (pH 2.0)

    • Cola and similar drinks (pH 3.0)

    • Coffee (pH 5.0)

Neutral pH=7

  • Examples of Neutral and Alkaline Solutions:

    • Pure water (pH 7.0)

    • Blood and tears (pH 7.35-7.45)

    • Pancreatic juice (pH 7.5-8.0)

Alkaline (Basic) Solutions

  • Basic substances have higher pH values:

    • Baking soda (pH 8.1)

    • Laundry detergent (pH 9.0)

    • Ammonia (pH 11.5)

    • Bleach (pH 12.5)

  • pH Changes and Organisms

    • Each pH unit on the scale represents a tenfold change in H+ concentration.

    • Organisms have specific pH requirements and use buffers to maintain homeostasis against pH fluctuations.

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