Acids and Bases

Question 1

Bronsted- Lowry Acid

Answer 1

A proton donator (H+). must have a H atom that it can lose as H+ ion

Question 2

Bronsted- Lowry Base

Answer 2

A proton acceptor (H+). Must have a non-bonding pair of electrons that it can bind the H+ ion.

Question 3

Arrhenius Acid

Answer 3

Produces H+ ions in in solution. Increases the [H+] in water

Question 4

Arrhenius Base

Answer 4

Produces OH- ions in solution. increases the [OH] in solution

Question 5

Amphoteric/ Amphiprotic

Answer 5

a species that can act as an acid and a base.

Question 6

Strong Acid

Answer 6

completely dissociates in water. These are also strong electrolytes existing in aqueous solutions entirely as ions.

1. HCl- hydrochloric acid
2. HBr- hydrobromic acid
3. HI- hydroiodic acid
4. HNO3- nitric acid
5. HClO4- perchloric acid
6. H2SO4- sulfuric acid
7. HClO3- chloric acid

Question 7

strong bases

Answer 7

Strong electrolytes in aquoes solutions.
1. LiOH- lithium hydroxide
2. NaOH- sodium hydroxide
3. KOH- potassium hydroxide
4. RbOH- rubium hydroxide
5. CsOH - cesium hydroxide
6. Ca(OH)2- calcium hydroxide
7. Sr(OH)2- strontium hydroxide
8. Ba(OH)2 - barium hydroxide

Question 8

The strongest acids/bases have the…

Answer 8

… weakest conjugate base/acids (kw)

Question 9

Kw

Answer 9

ion product constant of water.
kw = 1,0 x 10^ -14
ka x kb = kw

Question 10

pH/ pOH

Answer 10

pH = -log [H3O+]

pOH = -log [OH-]

pH + pOH = 14

Question 11

pKa / pKb

Answer 11

pKa = =log [Ka]

pKb = -log [Kb]

Question 12

the species with more protons…

Answer 12

is the acid.

Question 13

Doubling the [of a weak acid]…

Answer 13

does not double the [H30+]
the higher the [ ] the lower the extent of ionization.

Question 14

the greater the ka/ kb value…

Answer 14

the stronger the acid/ base ( hence pka/ pkb is smaller)

Question 15

the position of equilibrium favours…

Answer 15

the transfer of the proton from the stronger acid to the stronger base to form the weaker acid and the weaker base.

Question 16

the equilibrium mixture contains more…

Answer 16

weaker acid/ base and less stronger acid/base.

Question 17

Weak Acids

Answer 17

only partially ionize in solution.
1. HF - hydroflouric acid
2. HNO2- nitrous acid
3. C6H5COOH - benzoic acid
4. CH3COOH- acetic acid
5. HClO- hypochlorous acid
6.HOC6H5- phenol acid

Question 18

weak bases

Answer 18

only partially ionize in solution.
1. NH3 - ammonia
2. C5H5N- pyridine
3. C03- carbonate ion
4. HS- hydrosulfide ion
5. ClO -hypochlorite ion
6. H2NOH - hydroxylamine
7. NH2CH3 - methylamine

Question 19

Percent ionization

Answer 19

% = (concentrations ionized ÷ original concentration) x 100

Question 20

the stronger the acid…

Answer 20

the greater the percent ionization

Question 21

polyprotic acid

Answer 21

An acid that can donate more than one proton (H+)

Question 22

What effect will the Anion that is the conjugate base of a strong acid have on the pH?

Answer 22

will not affect the pH as it is a spectator ion

Question 23

what effect will the Anion of a weak acid have on the pH?

Answer 23

it will cause an increase in pH.

Question 24

What effect will a cation that is the conjugate acid of a weak base have on the pH?

Answer 24

it will decrease the pH.

Question 25

what effect does cations of strong Arrhenius bases have on the pH?

Answer 25

these will not affect the pH as they are spectator ions. these include cations of group 1A and heavier group 2A cations ( Ca; Sr; Ba).

Question 26

what is the common ion effect?

Answer 26

whenever a weak electrolyte and a strong electrolyte contain a common ion, the weak electrolyte ionizes less than it would if it were alone in solution. This is important in buffer solutions.

Question 27

what do we need in order to create a common ion?

Answer 27

a weak acid and a soluble salt of that acid.

Question 28

salt

Answer 28

substance produces in an acid and base reaction. are generally strong electrolytes.

Question 29

what happens when you add a strong electrolyte to a weak acid? according to Le chateliers principle

Answer 29

1. An increase in the [ of weak acid] 2. this causes equilibrium to shift to the left 3. the H+ ions are used up and there is a decreases in the [H+] ions. 4. pH increases (making it less acidic) as it ionizes less.

Question 30

Buffer solutions

Answer 30

*solutions that contain a weak conjugate acid-base pair. *It resists drastic changes in the pH when small amounts of strong acids or bases are added. Because it has both an acid to neutralize OH ions and a base to neutralize H ions * keep the pH nearly constant.

Question 31

how are buffers prepared?

Answer 31

by mixing a weak acid or a weak base to a salt of that acid or base.

Question 32

Calculations in pH of a buffer we use...

Answer 32

1. Common ion method with ICE table and ka constant 2. Henderson- hasselbalch equation pH = pka + log [base] ÷[ Acid]

Question 33

as the [weak acid] increases what happens to the equilibrium concentration oh [H+] and the % ionization?

Answer 33

the equilibrium concentration oh H+ increases, however the % ionization decreases as the concentration increases

Question 34

how is pH affected with an anion that is the conjugate base of a weak acid

Answer 34

it will cause an increase in the pH

Question 35

how is pH affected with an anion that is the conjugate base of a strong acid?

Answer 35

will not affect the pH ( they are spectator ions)

Question 36

how is pH affected by the cation that is the conjugate acid of a weak base?

Answer 36

will cause a decrease in the PH

Question 37

how does the cations of group 1A and heavier group 2A affect pH?

Answer 37

it will not affect the pH.

Question 38

Methyl red

Answer 38

pH= 4-6 red to yellow

Question 39

Bromothymol blue

Answer 39

pH= 6 -8 yellow to blue

Question 40

Phenolphthalein

Answer 40

pH = 8-10 colourless to pink/magenta