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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?
What is the defining characteristic of a strong acid?
What is the defining characteristic of a strong acid?
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?
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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Description
Explore the properties of water, its polarity, and its role as an excellent solvent. Learn about acids, their definition, and pH values.
