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Questions and Answers
What is produced when an acid is placed in water?
What is produced when an acid is placed in water?
Which statement correctly defines a Bronstead Lowry acid?
Which statement correctly defines a Bronstead Lowry acid?
What does a buffer solution primarily resist?
What does a buffer solution primarily resist?
What is the characteristic of diprotic acids?
What is the characteristic of diprotic acids?
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What does the term 'conjugate base' refer to?
What does the term 'conjugate base' refer to?
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Study Notes
Acids and Bases
- Acids produce hydronium ions (H3O+) when placed in water.
- Bases produce hydroxide ions (OH-) when placed in water.
- Strong acids and bases dissociate completely (100%) in water.
- Weak acids and bases dissociate partially (less than 100%) in water.
Brønsted-Lowry Acids and Bases
- A Brønsted-Lowry acid is defined as a proton (H+) donor.
- A Brønsted-Lowry base is defined as a proton (H+) acceptor.
- An acid-base reaction is a proton transfer reaction.
Conjugate Acids and Bases
- Any pair of molecules or ions that can be interconverted by transfer of a proton (H+) is called a conjugate acid-base pair.
- The conjugate acid is formed when a proton (H+) is added to a base.
- The conjugate base is formed when a proton (H+) is removed from an acid.
Amphoteric Substances
- Amphoteric substances can act as both acids and bases.
pH
- pH is a measure of the acidity or basicity of a solution.
- pH = -log[H3O+]. Lower pH values indicate higher acidity.
Ion Product of Water (Kw)
- In pure water at room temperature, the ion product of water (Kw) is 1.0 x 10-14.
- Kw = [H3O+][OH-]
Buffer Solutions
- A buffer solution resists a change in pH when limited amounts of acid or base are added.
- Buffer solutions commonly consist of a weak acid and its conjugate base.
- The maximum amount of acid or base that can be added before the buffer stops working is the buffer's capacity.
Indicators
- Indicators are substances that change color at a specific pH.
Polyprotic Acids
- Monoprotic acids can give up only one proton (H+). Example: HCl
- Diprotic acids can give up two protons (H+). Example: H2SO4
- Triprotic acids can give up three protons (H+). Example: H3PO4
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Description
Test your knowledge of acids and bases with this quiz, focusing on key concepts such as the definitions of strong and weak acids, the Brønsted-Lowry theory, and pH calculations. Explore the properties of conjugate acid-base pairs and amphoteric substances to solidify your understanding of this vital topic in chemistry.
