8.1 Theories of acids and bases

Consider the equilibrium below.
CH3CH2COOH(aq) + H2O(l)  $\longrightarrow$    CH3CH2COO–(aq) + H3O+(aq)
Which species represent a conjugate acid-base pair?

• CH3CH2COOH and H2O

• H2O and CH3CH2COO–

• H3O+ and H2O

• CH3CH2COO– and H3O+

According to Bronsted-Lowry acid base theory, an acid is a.....

• Proton donor
• Proton acceptor
• Produces H+ when added to water
• Made of H+

According to Lewis acid-base theory, a Lewis base is.....

• an electron pair acceptor
• an electron pair donor
• an oxidising agent
• a reducing agent

According to Arrhenius acid-base theory, an acid is....

• an H+ acceptor
• a H+ donor
• a substance that produces H+ in water
• anything with an H+

What is the conjugate acid in the following equation?

• PO₄^3- 
• HNO₃ 
• NO₃^- 
• HPO₄^2-
  

HSO₄^-(aq)+H₂O(l)      →       H₃O⁺(aq)+SO₄^2-(aq)
Identify the Acid in the above reaction.

• HSO₄^-
• H₂O
• H₃O⁺
• SO₄^2-

CO₃^2-(aq)+H₂O(l)      →              HCO₃^-(aq)+OH^-(aq)
Using the above reaction, which compound is the conjugate base?

• CO₃^2-
• H₂O
• HCO₃^-
• OH^-

Which is not a conjugate acid-base pair?

• HNO3 and NO3–

• CH3COOH and CH3COO–

• H3O+ and OH–

• HSO4– and SO42–

Which statement about acids is correct?

• A Brønsted-Lowry acid donates an electron pair.

• A Lewis acid donates a proton.

• A Brønsted-Lowry acid accepts a proton.

• A Lewis acid accepts an electron pair.