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Questions and Answers
What is the primary reason why water is an excellent solvent?
What is the primary reason why water is an excellent solvent?
- Its molecular structure allows it to donate or accept hydrogen ions
- Its high boiling point enables it to dissolve a wide variety of substances
- Its polarity allows it to form ionic bonds with other molecules
- Its polarity allows it to dissolve a wide variety of substances (correct)
What is the defining characteristic of a strong acid?
What is the defining characteristic of a strong acid?
- It partially dissociates in water, releasing some hydrogen ions
- It only dissociates in organic solvents, not in water
- It completely dissociates in water, releasing all hydrogen ions (correct)
- It never dissociates in water, retaining all hydrogen ions
What is the pH of a solution with a hydrogen ion concentration of 10^-5 M?
What is the pH of a solution with a hydrogen ion concentration of 10^-5 M?
- pH 5
- pH 7
- pH 9
- pH 6 (correct)
What is the role of a base in a solution?
What is the role of a base in a solution?
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What occurs when an acid and a base combine in a neutralization reaction?
What occurs when an acid and a base combine in a neutralization reaction?
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What is the purpose of acid-base reactions in determining pH?
What is the purpose of acid-base reactions in determining pH?
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What is the effect of increasing the pH of a solution by one unit?
What is the effect of increasing the pH of a solution by one unit?
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Which of the following is an example of a weak base?
Which of the following is an example of a weak base?
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Study Notes
Water
- Water (H2O) is a polar molecule, meaning it has a slightly positive charge on the hydrogen atoms and a slightly negative charge on the oxygen atom.
- This polarity allows water to dissolve a wide variety of substances, making it an excellent solvent.
- Water is essential for life, making up approximately 60% of an adult human's body weight.
Acids
- Acids are substances that donate a hydrogen ion (H+) in solution.
- Acids have a pH below 7, with lower pH values indicating higher acidity.
- Strong acids completely dissociate in water, releasing all hydrogen ions, whereas weak acids only partially dissociate.
- Examples of strong acids:
- Hydrochloric acid (HCl)
- Sulfuric acid (H2SO4)
- Nitric acid (HNO3)
- Examples of weak acids:
- Acetic acid (CH3COOH)
- Citric acid (C6H8O7)
Bases
- Bases are substances that accept a hydrogen ion (H+) in solution.
- Bases have a pH above 7, with higher pH values indicating higher basicity.
- Strong bases completely dissociate in water, releasing all hydroxide ions (OH-), whereas weak bases only partially dissociate.
- Examples of strong bases:
- Sodium hydroxide (NaOH)
- Calcium hydroxide (Ca(OH)2)
- Examples of weak bases:
- Ammonia (NH3)
- Trimethylamine (N(CH3)3)
pH Scale
- The pH scale measures the concentration of hydrogen ions in a solution.
- pH ranges from 0 to 14, with:
- pH 7 being neutral (neither acidic nor basic)
- pH below 7 being acidic
- pH above 7 being basic
- Each step down the pH scale represents a tenfold increase in hydrogen ion concentration.
Acid-Base Reactions
- Acid-base reactions involve the transfer of a hydrogen ion from an acid to a base.
- Acid-base reactions can be neutralization reactions, where an acid and a base combine to form a salt and water.
- Acid-base reactions can also be used to determine the pH of a solution.
Water
- Water's polarity allows it to dissolve a wide variety of substances, making it an excellent solvent.
- Water is essential for life, making up approximately 60% of an adult human's body weight.
Acids
- Acids donate a hydrogen ion (H+) in solution.
- Acids have a pH below 7, with lower pH values indicating higher acidity.
- Strong acids completely dissociate in water, releasing all hydrogen ions.
- Examples of strong acids: Hydrochloric acid (HCl), Sulfuric acid (H2SO4), Nitric acid (HNO3).
- Weak acids only partially dissociate in water.
- Examples of weak acids: Acetic acid (CH3COOH), Citric acid (C6H8O7).
Bases
- Bases accept a hydrogen ion (H+) in solution.
- Bases have a pH above 7, with higher pH values indicating higher basicity.
- Strong bases completely dissociate in water, releasing all hydroxide ions (OH-).
- Examples of strong bases: Sodium hydroxide (NaOH), Calcium hydroxide (Ca(OH)2).
- Weak bases only partially dissociate in water.
- Examples of weak bases: Ammonia (NH3), Trimethylamine (N(CH3)3).
pH Scale
- The pH scale measures the concentration of hydrogen ions in a solution.
- pH ranges from 0 to 14, with pH 7 being neutral (neither acidic nor basic).
- pH below 7 is acidic, and pH above 7 is basic.
- Each step down the pH scale represents a tenfold increase in hydrogen ion concentration.
Acid-Base Reactions
- Acid-base reactions involve the transfer of a hydrogen ion from an acid to a base.
- Acid-base reactions can be neutralization reactions, where an acid and a base combine to form a salt and water.
- Acid-base reactions can be used to determine the pH of a solution.
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