3.1.12 Acids and bases

Question 1

what is a Brønsted-Lowry acid?

Answer 1

a proton donor. e.g; Ammonium ions.

Question 2

what is a Brønsted-Lowry ​base?

Answer 2

a proton acceptor. e.g; hydroxide ions

Question 3

definition of a strong acid

Answer 3

an acid the completely dissociated to ions when in solution with pH 3-5

Question 4

definition of a weak acid

Answer 4

an acid that only slightly dissociated when in solution with pH 0-1

Question 5

what is a monoprotic acid?

Answer 5

an acid that donates one H+ from each molecule

Question 6

what is a diprotic acid?

Answer 6

an acid that donates two H+ from each molecule

Question 7

how do you find the pH of a strong acid?

Answer 7

pH = -log[H+]

Question 8

how do you find the concentration of a strong acid?

Answer 8

[H+] = 10^-pH

Question 9

how do you convert pKa into Ka?

Answer 9

Ka = 10^-pKa

Question 10

what is the value of Kw?

Answer 10

10^-14

Question 11

how do you find the concentration of a weak acid?

Answer 11

[HA] = [H+]^2

Question 12

how do you find the concentration of a weak acid?

Answer 12

[HA] = [H+]^2/ Ka

Question 13

what is the general equation for a weak acid before rearranging it?

Answer 13

Ka = [H+]^2/ [HA]

Question 14

how do you work out the concentration of a weak base?

Answer 14

[H+] = Kw/ [OH-]

Question 15

how do you work out the concentration of a strong base?

Answer 15

[OH-] = Kw/ [H+]

Question 16

what is the equation for the ionic product of water?

Answer 16

Kw = [H+][OH-]

Question 17

what affects the value of Kw?

Answer 17

the temperature

Question 18

what is the reaction equation between a weak acid and a weak base?

Answer 18

HA H+ + A-

Question 19

what is the equation for the reaction between a weak acid and a weak base?

Answer 19

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

Question 20

what is the equation when there is excess HA (H+) in a mixture of a weak acid and weak base?

Answer 20

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

Question 21

what does [HA] refer to in the equation: Ka = [H+][A-]/ [HA]

Question 22

if you are given the pH of a diprotic substance, what do you do?

Answer 22

half it

Question 23

if you are given the conc of a diprotic substance, what do you do?

Answer 23

double it

Question 24

what equation can be used for all aqueous solutions?

Answer 24

kW = [H+][OH-]

Question 25

what equation can be used for all solutions containing a weak acid?

Answer 25

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

Question 26

what equation can be used for a weak acid in water?

Answer 26

Ka = [H+]^2/ [HA]

Question 27

how do you convert pKa into Ka?

Answer 27

Ka = 10^-pKa

Question 28

what is the equation for excess [OH-] in a solution of a strong base and strong acid?

Answer 28

[H+] = Kw/ [OH-]

Question 29

what is the equation for excess [H+] in a solution of a strong acid and strong base?

Answer 29

[H+] = n/ v

Question 30

what does [H+] mean in Kw = [H+][OH-]

Question 31

give simple steps about how to find the pH when HA is in excess in a solution of a weak acid and weak base

Answer 31

use [HA] and [A-] along with the Ka (normally given) to find [H+], then pH [H+] = Ka [HA]/ [A-] pH = -log[H+]

Question 32

give simple steps about how to find the pH when A- is in excess in a solution of a weak acid and weak base

Answer 32

use Kw to find [H+], then pH Kw = [H+]^2 pH = -log[H+]

Question 33

give simple steps about how to find the pH when HA = A- in a solution of a weak acid and weak base

Answer 33

pKa = pH | find pKa

Question 34

equation for the dissociation of water

Answer 34

H20 H+ + OH- (in eqm)