5.1.3 acids bases and buffers

Question 1

Bronsted lowry acid

Answer 1

a substance that can donate a proton

Question 2

Bronsted-Lowry base

Answer 2

Substance that can accept a proton

Question 3

Bigger ka

Answer 3

stronger acid

Question 4

Acid + metal

Answer 4

Salt + hydrogen

Question 5

Acid + alkali

Answer 5

Salt + water

Question 6

Acid + carbonate

Answer 6

Salt + water + co2

Question 7

Ph equation

Answer 7

PH = -log [H+]

Question 8

Strong acids

Answer 8

Completely dissociate in aqueous solutions

E.g. HCl, HNO3

Question 9

[H+] equation from pH

Answer 9

[H+]= 1x10^-pH

Question 10

Ionic product for water

Answer 10

Kw = [H+] [OH-]

Used for finding pH of pure water or pH of strong base when given [OH-]

1x10^-14 mol2 dm-6

At 25C

Question 11

PH of strong base

Answer 11

[H+] = Kw / [OH-]

PH = - log [H+]

Question 12

Weak acids

Answer 12

Partially dissociate in aqueous solutions

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

Question 13

pKa

Answer 13

pKa = -log [Ka]

Ka = 10^-pKa

Question 14

PH of diluted strong acid

Answer 14

[H+] = [H+]old x (old volume/new volume)

Ph= -log [H+]

Question 15

PH of diluted base

Answer 15

[OH-] = [OH-]old x (old volume/new volume)

[H+] = kw / OH-

PH = -log [H+]

Question 16

Acidic buffer

Answer 16

Weak acid and salt of that weak acid

Question 17

Basic buffer

Answer 17

Weak base and salt of that weak base

Question 18

Adding small amounts of acid to buffer

Answer 18

Equilibrium shifts to left removing H+ ions added

Large concentration of salt ion in buffer so ratio stays constant and pH stays constant

Question 19

Adding small amount of alkali to buffer

Answer 19

OH- ions react with H+ to form water

Equilibrium shifts to right to produce H+ ions

Concentrations of H+ ions and pH remains constant