Biology: Biochemistry TPR Review Acids & Bases

Question 1

Acids (Bronsted Lowry) Def

Answer 1

Proton (H+) donors

Question 2

Bases (Bronsted Lowry) Def

Answer 2

Proton (H+) acceptors

Question 3

conjugate base trick

Answer 3

one less H atom and one more - charge than the acid that formed it

Question 4

Conjugate acid trick

Answer 4

one more H atom and one more + charge than base that formed it

Question 5

Strength of an acid is related to:

Answer 5

How much of the products are favored over the reactants

Question 6

Ka/kb

Answer 6

acid/base-ionization (acid or base-dissociation constant) - determines relative strengths of acids

Question 7

The larger the Kb or Ka value (and vise versa)

Answer 7

the stronger the base or acid

Question 8

amphoteric

Answer 8

acts as acid or base (like water)

Question 9

Formula for pH

Answer 9

pH = -log[H+], where [H+] = 10^-ph

Question 10

[H+] = ^-7

Answer 10

neutral ph (pure water)

Question 11

[H+] > ^-7

Answer 11

ph is less than 7 and is acidic

Question 12

[H+] < ^-7

Answer 12

ph is greater than 7 and is basic

Question 13

low ph means high :

Answer 13

H+, acidic

Question 14

High ph means low:

Answer 14

H+, basic

Question 15

Formula POH

Answer 15

POH= -log[OH-], where [OH] = 10^-POH

Question 16

formula of PH and POH

Answer 16

PH + POH = 14

Question 17

Pka and Pkb formula

Answer 17

Pka = -logKa
Pkb = -logKb

Question 18

“P” means

Answer 18

take the negative log of

Question 19

Ka and Pka values are opposite. Explain

Answer 19

The > the Ka value, the stronger the acid. The lower then Pka value, the stronger the acid.

Question 20

When a acid or base is stronger, what happens chemically?

Answer 20

More molecules dissociate into ions in aqueous solution

Question 21

Buffers

Answer 21

solution that resists changing pH when acid or base amounts are added

Question 22

Most important buffer system in blood plasma (and for the MCAT)

Answer 22

bicarbonate buffer system

H2CO3 –> H+ + HCO3-