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
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-.
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.
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)
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)
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.