Acids and Bases Quiz

Acids and Bases

• Acid: Produces hydronium ions (H3O+) when placed in water.
• Base: Produces hydroxide ions (OH-) when placed in water.
• Brønsted-Lowry Acid: Donates a proton (H+).
• Brønsted-Lowry Base: Accepts a proton (H+).
• Amphoteric (amphiprotic): Substance that can act as both an acid and a base.
• Conjugate Acid: Formed by adding a proton (H+) to a base.
• Conjugate Base: Formed by removing a proton (H+) from an acid.
• Conjugate Acid-Base Pair: Any pair of molecules or ions that can be interconverted by the transfer of a proton (H+).

Acid-Base Reactions

• Acid-Base Reaction: A proton (H+) transfer reaction.

Strength of Acids and Bases

• Strong Acid/Strong Base: Dissociates completely (100%) in water.
• Weak Acid/Weak Base: Dissociates partially (less than 100%) in water.

pH

• pH: Measures the acidity or alkalinity of a solution.
• pH = -log[H3O+]
• Hydronium Ion: H3O+

Ion Product of Water

• Ion Product of Water (Kw): Describes the equilibrium constant for the autoionization of water.
• At 25°C, Kw = 1.0 x 10^-14

Buffer Solutions

• Buffer Solution: Resists changes in pH when small amounts of acid or base are added.
• Common Example: An aqueous solution containing a weak acid and its conjugate base.
• Buffer Capacity: The maximum amount of acid or base that can be added before the buffer stops working.

Polyprotic Acids

• Monoprotic Acid: Can give up only one proton (H+). Example: HCl (Hydrochloric Acid).
• Diprotic Acid: Can give up two protons (H+). Example: H2SO4 (Sulfuric Acid).
• Triprotic Acid: Can give up three protons (H+). Example: H3PO4 (Phosphoric Acid).
• Indicator: Changes color at a specific pH.