In this worksheet, we will practice classifying acids and bases as weak or strong based on their dissociation constants.
The relative acid strengths of and can be determined by comparing their acid and base dissociation constants, and . has a of and , the conjugate base of , has a of . Given that the self-ionization constant of water is , which compound is the stronger acid?
- A and are equally strong acids.
- B is the stronger acid.
- CMore information is needed.
- D is the stronger acid.
The odor of vinegar is due to the presence of acetic acid, , a weak acid. For a solution of acetic acid, which of the following is false?
- A >
- C >
- D >
- E >
Household ammonia is a solution of the weak base in water. For a solution of ammonia, which of the following is false?
- A >
- C >
- E >
Which base, or , is the stronger base at ? The of at this temperature is and the of is .
- AThey are both amines, and therefore they are equally strong bases.
- CIt is impossible to tell without knowing at what concentration their basicity is measured.
The active ingredient formed by aspirin in the body is salicylic acid, . The carboxyl group acts as a weak acid. The phenol group (an group bonded to an aromatic ring) also acts as an acid but a much weaker acid.
Which one of the following is false for a 0.001 M aqueous solution of salicylic acid?
Which is the stronger base, or ? The of is and the of is
- AIt is impossible to tell without knowing at what concentration their basicity is measured.
- C and are equally strong bases.
A 5.16 g sample of was added to 20.0 mL of and the resulting solution diluted to 0.100 L. The of is . Is the solution acidic, neutral, or basic?