Chapter 2: Acids and Bases

Question 1

[2.1] Bronsted-Lowry Acids must contain what atom?

Answer 1

Hydrogen

Question 2

[2.1] Bronsted-Lowry bases must have an available what?

Answer 2

Electron pair via lone pairs or pi bonds

Question 3

[2.2] A Bronsted-Lowry acid-base reaction is the transfer of a proton from a ____ to a ____?

Answer 3

Acid; base

Question 4

[2.2] This product is due to a loss of a proton from an acid

Answer 4

Conjugate base

Question 5

[2.2] This product is due to a gain of a proton by a base

Answer 5

Conjugate acid

Question 6

[2.2] Explain why Bronsted-Lowry acids tend to also accept electrons from the electron-rich Bronsted-Lowry base.

Answer 6

Because the HA bond gives it a partial positive charge, making it electrophilic.

Question 7

[2.3] What constant measures acidity?

Answer 7

Equilibrium constant (Keq), or acidity constant (Ka)

Question 8

[2.3] Explain the relationship between acid strength and Ka and pKa.

Answer 8

The larger the Ka (= the smaller the pKa), the stronger the acid.

Question 9

[2.4] Does the equilibrium favor the formation of the stronger or weaker acid?

Answer 9

Weaker

Question 10

[2.4] How can you predict if a Bronsted-Lowry base can deprotonate an acid given Ka, pKa values?

Answer 10

An acid can be deprotonated by the conjugate base of any acid having a higher pKa because it is the weaker acid. The formation of the weaker acid is favored by equilibrium.

Question 11

[2.8] Explain the difference between a Bronsted-Lowry acid and a Lewis acid.

Answer 11

All Bronsted-Lowry acids must contain a hydrogen atom, but Lewis acids only need to be electron deficient.

Question 12

[2.8] Are all Lewis acids Bronsted-Lowry acids? Explain why.

Answer 12

No, because some Lewis acids lack a hydrogen atom and are only electron deficient because their valence shells aren’t filled.

Question 13

[2.8] Explain the difference between a Bronsted-Lowry base and a Lewis base.

Answer 13

They differ in to who they give the electron pair to.

Bronsted-Lowry base - donates an electron pair to a proton only
Lewis base - donates an electron pair to anything that is electron deficient

Question 14

[2.8] In a Lewis acid-base reaction, which is the electrophile and which is the nucleophile?

Answer 14

Electrophile - Lewis acid
Nucleophile - Lewis base

Question 15

[2.3] A strong acid has an equilibrium that lies in what direction (left or right)?

Answer 15

To the right