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Questions and Answers
What is the pH range typically found in fresh water rivers and lakes?
What is the pH range typically found in fresh water rivers and lakes?
- 7.0 to 9.0
- 5.5 to 7.5
- 4.0 to 5.0
- 6.5 to 8.5 (correct)
What is the approximate pH value of distilled water?
What is the approximate pH value of distilled water?
- 7.0 (correct)
- 5.5
- 8.0
- 6.0
Which factor most significantly affects the pH of groundwater?
Which factor most significantly affects the pH of groundwater?
- Proximity to agricultural areas
- Water temperature
- Rock composition (correct)
- Presence of dissolved gases
What is the pH range of clouds, and what causes their acidity?
What is the pH range of clouds, and what causes their acidity?
Which of these is classified as a weak acid?
Which of these is classified as a weak acid?
What happens to the concentration of hydrogen ions when sodium bicarbonate (NaHCO3) undergoes hydrolysis?
What happens to the concentration of hydrogen ions when sodium bicarbonate (NaHCO3) undergoes hydrolysis?
What is the pH value of pure water?
What is the pH value of pure water?
How does the hydrolysis of ammonium chloride (NH4Cl) affect the concentration of hydroxide ions?
How does the hydrolysis of ammonium chloride (NH4Cl) affect the concentration of hydroxide ions?
Which of the following pH values indicates an acidic solution?
Which of the following pH values indicates an acidic solution?
What occurs when table salt (NaCl) is dissolved in water?
What occurs when table salt (NaCl) is dissolved in water?
What is the range of pH values for seawater?
What is the range of pH values for seawater?
What indicates that a solution is basic?
What indicates that a solution is basic?
Which ions are involved in determining the acidity or basicity of water?
Which ions are involved in determining the acidity or basicity of water?
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Study Notes
Hydration and Hydrolysis
- 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
- 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.
pH Levels in Water Sources
- 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.
Types of Acids and Bases
-
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)
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