Lecture 5

Question 1

What is a Bronsted Lowry acid?

Answer 1

A proton donor

Question 2

What is a Bronsted Lowry base?

Answer 2

A proton acceptor

Question 3

Why does a base need to have a lone pair?

Answer 3

1. Bronsted Lowry: need lone pair to accept proton
2. Lewis: need lone pair to donate

Question 4

What is a Lewis acid?

Answer 4

Accepts and shares a pair of electrons

Question 5

What is a Lewis base?

Answer 5

Donates and shares a pair of electrons

Question 6

A weak acid has a ______– Ka value?

Answer 6

Lower

Question 7

How do you calculate Ka?

Answer 7

Ka = [A-][H30+] / [HA]

(Ka = K[H20])

Question 8

How do you calculate pKa?

Answer 8

pKa = -lg (Ka)

Question 9

A strong acid has a ________ pKa

Answer 9

low

Question 10

If the difference between the pKa of A and B is 2, how much stronger is A than B?

Answer 10

10^2 = 100

Question 11

The stronger the acid, the ____________ its conjugate base

Answer 11

weaker

Question 12

How do you calculate Keq?

Answer 12

Keq = 10 ^ (change in pKa)

Question 13

The equilibrium will always favor the formation of the _____________ acid

Answer 13

weaker

Question 14

How do you calculate pH of a acid?

Answer 14

pH = -lg [H+]
pH = pKa + lg [A-]/[HA]

Question 15

How do you calculate the pH of a weak base?

Answer 15

pH= pKa + lg[B]/[BH+]

Question 16

What is the concentration of the acid and its conjugate base when pH = pKa?

Answer 16

both are 50%