Acid-Base Reactions and Definitions

The video explains conjugate acid-base pairs using the Bronsted-Lowry definition, where acids donate protons and bases accept them. It illustrates this concept with examples of acetic acid and ammonia reactions, showing how substances can act as acids or bases depending on the reaction direction. The video also highlights the amphiprotic nature of water, which can act as both an acid and a base in different reactions.

What is the Bronsted-Lowry definition of an acid?

• A substance that accepts a proton

• A substance that donates a proton

• A substance that accepts an electron

• A substance that donates an electron

What is a conjugate acid-base pair?

• Two substances that differ by one proton

• Two substances that differ by one electron

• Two substances that differ by one molecule

• Two substances that differ by one neutron

In a conjugate acid-base pair, what does the acid have compared to the base?

• One more hydrogen ion

• One more electron

• One less hydrogen ion

• One less electron

What happens to acetic acid in the forward reaction with water?

• It accepts an electron

• It accepts a proton

• It donates a proton

• It donates an electron

In the reverse reaction of acetic acid and water, what role does H3O+ play?

• It acts as a catalyst

• It acts as an acid

• It acts as a base

• It acts as a neutral molecule

In the reaction between NH3 and water, what role does water play?

• It acts as a catalyst

• It acts as a neutral molecule

• It acts as an acid

• It acts as a base

What is the conjugate acid in the reaction between NH3 and water?

• H2O

• NH3

• OH-

• NH4+

What is the term for a substance that can both donate and accept a proton?

• Amphiprotic

• Amphiphilic

• Amphibious

• Amphoteric

In the first example, how does water behave?

• As an acid

• As a catalyst

• As a base

• As a neutral molecule

In the second example, how does water behave?

• As a catalyst

• As an acid

• As a neutral molecule

• As a base