Hydration and Acid-Base Balance Quiz

Study Notes

Water molecules contain hydrogen ions (H+) and hydroxide ions (OH-), influencing chemical reactions.
Natural salts in water undergo hydrolysis, impacting acidity or basicity.
Example: When dissolved, table salt (NaCl) dissociates into sodium ions (Na+) and chloride ions (Cl-), keeping the solution neutral (H+ = OH-).
Sodium bicarbonate (NaHCO3) causes hydrolysis that lowers H+ concentration and raises OH- concentration, resulting in a basic solution.
Ammonium chloride (NH4Cl) dissociates to decrease OH- and increase H+, creating an acidic solution.

Acid-base balance is defined by the relationship between H+ and OH- concentrations in water.
pH scale ranges from 0 to 14, measuring acidity (pH < 7) or basicity (pH > 7).
Water is neutral at pH 7, with equal concentrations of H+ and OH-.
pH varies across different water sources, affecting aquatic life.

Seawater: pH typically between 7.5 and 8.4; varies by location and environmental factors.
Freshwater rivers and lakes: pH generally ranges from 6.5 to 8.5; naturally occurring fluctuations.
Distilled water: pH about 7, devoid of impurities that alter acidity or basicity.
Groundwater: pH varies by rock composition; often neutral or basic, influenced by calcium or magnesium carbonate.
Clouds: slightly acidic pH between 4.5 and 5, resulting from dissolved carbon dioxide and acidic gases; environmental factors can affect this.

Strong Acids:
- Perchloric acid (HClO4)
- Hydroiodic acid (HI)
- Hydrochloric acid (HCl)
- Hydrobromic acid (HBr)
- Sulfuric acid (H2SO4)
- Nitric acid (HNO3)
Weak Acids:
- Carbonic acid (H2CO3)
- Phosphoric acid (H3PO4)
- Acetic acid (CH3COOH)
- Formic acid
- Citric acid
- Oxalic acid
- Lactic acid
Strong Bases:
- Potassium hydroxide (KOH)
- Sodium hydroxide (NaOH)
- Barium hydroxide (Ba(OH)2)
Weak Base:
- Ammonium hydroxide (NH4OH)