Chemistry Acids and Bases Quiz

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