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chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

Bronsted- Lowry Acid

A

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

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2
Q

Bronsted- Lowry Base

A

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

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3
Q

Arrhenius Acid

A

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

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4
Q

Arrhenius Base

A

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

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5
Q

Amphoteric/ Amphiprotic

A

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

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6
Q

Strong Acid

A

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
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7
Q

strong bases

A

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

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8
Q

The strongest acids/bases have the…

A

… weakest conjugate base/acids (kw)

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9
Q

Kw

A

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

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10
Q

pH/ pOH

A

pH = -log [H3O+]

pOH = -log [OH-]

pH + pOH = 14

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11
Q

pKa / pKb

A

pKa = =log [Ka]

pKb = -log [Kb]

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12
Q

the species with more protons…

A

is the acid.

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13
Q

Doubling the [of a weak acid]…

A

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

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14
Q

the greater the ka/ kb value…

A

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

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15
Q

the position of equilibrium favours…

A

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

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16
Q

the equilibrium mixture contains more…

A

weaker acid/ base and less stronger acid/base.

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17
Q

Weak Acids

A

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

18
Q

weak bases

A

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

19
Q

Percent ionization

A

% = (concentrations ionized ÷ original concentration) x 100

20
Q

the stronger the acid…

A

the greater the percent ionization

21
Q

polyprotic acid

A

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

22
Q

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

A

will not affect the pH as it is a spectator ion

23
Q

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

A

it will cause an increase in pH.

24
Q

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

A

it will decrease the pH.

25
Q

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

A

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).

26
Q

what is the common ion effect?

A

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.

27
Q

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

A

a weak acid and a soluble salt of that acid.

28
Q

salt

A

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

29
Q

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

A
  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.
30
Q

Buffer solutions

A

*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.

31
Q

how are buffers prepared?

A

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

32
Q

Calculations in pH of a buffer we use…

A
  1. Common ion method with ICE table and ka constant
  2. Henderson- hasselbalch equation
    pH = pka + log [base] ÷[ Acid]
33
Q

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

A

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

34
Q

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

A

it will cause an increase in the pH

35
Q

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

A

will not affect the pH ( they are spectator ions)

36
Q

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

A

will cause a decrease in the PH

37
Q

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

A

it will not affect the pH.

38
Q

Methyl red

A

pH= 4-6
red to yellow

39
Q

Bromothymol blue

A

pH= 6 -8
yellow to blue

40
Q

Phenolphthalein

A

pH = 8-10
colourless to pink/magenta

chemistry (5 decks)

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