Quiz on Brønsted-Lowry Acids and Buffers

What is a Brønsted-Lowry acid?

• A substance that accepts protons

• A substance that donates protons

• A substance that has a pH less than 7

• A substance that reacts with metals

What is a Brønsted-Lowry base?

• A substance that donates electrons

• A substance that accepts protons

• A substance that has a pH greater than 7

• A substance that reacts with acids

In the reaction HCl + NH3 -> NH4+ + Cl- which is the acid?

• NH₃

• HCl

• NH₄⁺

• Cl⁻

What is a conjugate acid-base pair?

• Two acids that can donate protons

• Two bases that can accept protons

• An acid and its corresponding base after proton transfer

• Two unrelated substances

How do strong acids differ from weak acids?

• Strong acids partially dissociate, weak acids completely dissociate.

• Strong acids completely dissociate, weak acids partially dissociate.

• Both types fully dissociate.

• Both types do not dissociate.

What role does water play in Brønsted-Lowry acid-base reactions?

• It acts as a catalyst.

• It acts as a solvent and can participate in proton transfer.

• It does not participate at all.

• It only absorbs heat.

In the reaction H2SO4 + H2O --> HSO4- + H3O+ what is the conjugate base of sulfuric acid?

• H₂O

• HSO₄⁻

• H₃O⁺

• SO₄²⁻

What is a buffer solution?

• A solution that changes color with pH.

• A solution that resists pH changes upon addition of small amounts of acid or base.

• A solution that only contains strong acids.

• A solution that evaporates quickly.

How does a buffer maintain pH when an acid is added?

• It increases the temperature.

• The weak base component reacts with the added acid.

• The buffer becomes neutral.

• It dilutes the acid.

What happens when a base is introduced to a buffer solution?

• The pH increases dramatically.

• The weak acid component donates protons to neutralize the base.

• The buffer loses its effectiveness.

• The buffer evaporates.