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Questions and Answers
Define the Arrhenius theory of acids and bases.
Define the Arrhenius theory of acids and bases.
Arrhenius theory states that an acid dissociates in water to produce hydrogen ions (H+), while a base dissociates in water to form hydroxide ions (OH-).
Which theory defines an acid as a substance that donates a hydrogen ion (H+)?
Which theory defines an acid as a substance that donates a hydrogen ion (H+)?
A strong acid ______ dissociates in water.
A strong acid ______ dissociates in water.
completely
A weak base completely dissociates in water.
A weak base completely dissociates in water.
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What is the pH value of a solution with a [H3O+] concentration of 1.5 x 10^-5 mol/L?
What is the pH value of a solution with a [H3O+] concentration of 1.5 x 10^-5 mol/L?
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What does 'amphoteric' mean?
What does 'amphoteric' mean?
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Study Notes
Acids and Bases
- Non-metal oxides react with water to produce acids, which have a sour taste (acidus means "sour" in Latin).
- Acids have the following properties:
- Can cause indicators to change color.
- Produce hydrogen gas when reacting with metals.
- Produce carbon dioxide with carbonate compounds.
- Conduct electricity as they ionize in water.
Arrhenius Theory of Acids and Bases (1887)
- Acids dissociate in water to produce one or more hydrogen ions (H+).
- Bases dissociate in water to form one or more hydroxide ions (OH-).
Limitations of Arrhenius Theory
- Hydrogen ions (H+) are always hydrated, forming hydronium ions (H3O+).
- Not all bases contain hydroxide ions (e.g., ammonia).
- Not all acid-base reactions occur in water.
Other Acid-Base Theories
- Bronsted-Lowery:
- Acids: substances that donate a proton (H+).
- Bases: substances that accept a proton.
- Conjugate acid-base pairs differ by a proton.
- Lewis:
- Acids: accept an electron pair.
- Bases: donate an electron pair.
- Allows for a broader definition of acid-base reactions.
Strong and Weak Acids
- Strong acids: completely dissociate in water, producing hydronium ions (H3O+).
- Weak acids: partially ionize, with only a fraction of molecules producing hydronium ions.
Strong and Weak Bases
- Strong bases: completely dissociate in water, producing hydroxide ions (OH-).
- Weak bases: partially dissociate, with only a fraction of molecules producing hydroxide ions.
pH and pOH
- pH: measures the concentration of hydronium ions (H3O+).
- pOH: measures the concentration of hydroxide ions (OH-).
- pH + pOH = 14.
Calculating pH
- pH = -log[H3O+].
- If the concentration of [H3O+] is known, the pH can be calculated.
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Description
Learn about the properties and reactions of acids, including their taste, effect on indicators, and conductivity in water. Understand the ionization of acids in water and their reactions with metals and carbonate compounds.
