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CHEM > ACIDS + BASES > Flashcards

ACIDS + BASES Flashcards

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1
Q

Acids

A

proton/ H+ ion donor
monoprotic or polyprotic
Substances that dissociate + ionise
Form H+ ions

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2
Q

monoprotic

A

acid donates 1 proton

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3
Q

polyprotic

A

acid donates multiple protons

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4
Q

strength of acids

A

degree of ionisation at equilibrium in aq solutions

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5
Q

water

A

weak electrolyte
eq. constant- Kw = [H+][OH-] where Kw = 1 x 10^-14 at 25 0C

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6
Q

Kw

A

used to calc [H+] / [OH-] in solutions of strong acids/bases

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7
Q

Acid + base =

A

Salt + water

Net ionic- H+ + OH- = H20

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8
Q

Spectator ions

A

Occur both sides + cancel out

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9
Q

Disassociate

A

Compounds split into separate ions

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10
Q

Acid properties

A

conduct electricity
turn litmus red
sour taste
reacts with active metals to liberate H+
react with bases to neutralise properties

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11
Q

Base properties

A

conduct electricity
turn litmus blue
bitter taste/ slippery feeling
react with acids to neutralise properties

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12
Q

Alkali

A

Soluble/water base
basic

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13
Q

Bases

A

dissociate in water to produce OH- ions
accept protons from acids
form OH- ions

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14
Q

Ocean acidification

A

Decrease in pH due to absorption of CO2 from atmosphere

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15
Q

Anhydrous

A

contains no water

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16
Q

Acid + metal

A

salt + H2

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17
Q

Acid + metal hydroxide

A

salt + water

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18
Q

Acid + metal oxide

A

Salt + water

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19
Q

Acid + metal carbonate

A

Salt + water + CO2

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20
Q

Acid + metal hydrogen carbonate

A

Salt + water + CO2

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21
Q

Acidic oxide + base

A

Salt + water

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22
Q

H3O

A

= H+

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23
Q

pH scale

A

25 C
[H+] + [OH-] = pH 14

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24
Q

Electrolytes

A

solutions that carry an electric current

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25
Q

Finding [H+]

A

[H+] = 10^ -pH

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26
Q

Amphoteric

A

both acid + base

Eg: water

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27
Q

Arrhenius

A

Acid- H+ in H2O Base- OH- in H2O
only when dissolved in water

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28
Q

Bronsted-Lowry

A

Acid H+ donor + Base accepts H+

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29
Q

Lewis

A

Acid accepts e- pair
Base donates e- pair

30
Q

Strong acids

A

due to distance from nucleus
usually halogens

Eg: HNO3, H2SO4, HCl, HBr

31
Q

Strong bases

A

alkali/alkaline earth metals
metals usually

Eg: NaOH, KOH, LiOH

32
Q

Acetic acid

A

AKA ethanoic acid
vinegar
CH3COOH

33
Q

Ka

A

Acid dissociation constant
[H+][A-] / [HA]

HA <—> H+ + A-

HA- parent acid- name of acid
A- = acid - 1 H+ ion

weak acid = Ka less than 1

34
Q

pKa

A

= -log Ka
to describe strength of acids
smaller value, stronger acid
6 pKa = 10^-6 Ka

35
Q

strong acid + base

A

neutral salt

36
Q

Strong acid + weak base

A

acidic salt

37
Q

Strong base + weak acid

A

basic salt

38
Q

Weak acid + base

A

varies

39
Q

types of hydrolysis

A

salts
acid
base

40
Q

salts hydrolysis

A

sodium acetate + water = acetic acid + sodium + hydroxide

41
Q

acid hydrolysis

A

acetic acid + water = acetate + hydronium

42
Q

base hydrolysis

A

ammonia + water = ammonium + hydroxide

43
Q

hygroscopic substances

A

absorb moisture + do not dissolve/change physical state when exposed to atmosphere
may be amorphous solids/liq.

44
Q

deliquescence substances

A

do dissolve + change physical state when exposed to atmosphere at ordinary temp
crystalline solids

45
Q

anhydrous salt

A

ionic compound (salt) that attracts water molecules + forms loose chemical bonds with them
MN (metal + non-metal)

46
Q

Neutralisation

A

moles of H+ = moles of OH-

47
Q

Dilution

A

C1V1 = C2V2

moles do not change when diluted

48
Q

Titrant

A

known conc. + volume
in burette- ant- little drops

49
Q

Titrand/analyte

A

unknown conc.
known volume
in flask

50
Q

acid-base indicator

A

weak organic acid/base
ionised + non-ionised forms are dif. colours

51
Q

Phenolphthalein

A

acid clear, base pink
8-10

52
Q

methyl orange

A

acid red, base yellow
3-5

53
Q

litmus

A

acid red, basic blue
5-8

54
Q

acid-base strength

A

what degree dissociation of ions occur

55
Q

Buffer

A

mixture whose pH changes very little when small amount of strong acid/base added
weak conjugate acid-base pair
H+ / OH- ‘absorbed’ so resists pH change

56
Q

Buffer solution

A

aq. solution
mixture of weak acid + conjugate base / weak base + conjugate acid
used to keep pH nearly constant

57
Q

Buffer capacity

A

amount of acid/base it can effectively neutralise without significant change in pH

58
Q

Buffer range

A

pH range over which particular acid + conjugate base can be effective

59
Q

Factors affecting buffer capacity

A

conc. of buffer components- higher conc = greater capacity
ratio [A+]/[HA]- closer to 1, higher capacity

60
Q

Titration

A

to determine precise endpoint of a reaction + precise quantity of reactant in titration flask

61
Q

Titration curve

A

plot of pH of analyte solution vs volume of titrant added as titration progresses

62
Q

Equivalence point

A

point at which amount of titrant added is just enough to completely neutralise analyte solution
moles of base = moles of acid
solution contains only salt + water

63
Q

pH indicator in titration

A

show a colour change at equivalence point

64
Q

End point

A

end of titration process
when titrant stopped

65
Q

Titration accuracy

A

results within 0.2 mL of each other
end point close to equivalence point

66
Q

Why is equivalence point not always pH 7

A

depends on acid/base strength

67
Q

Polyprotic acid titrations

A

1 equivalence point for each H+ that can be donated

68
Q

Calc. titrand conc.

A

acid CV= base CV

69
Q

Purpose of back titration

A

solid analyte
impure analyte
slow reacting analyte with titrant in forward titration
weak acid-base reactions

70
Q

Back titration advantages

A

useful if endpoint easier to identify using back than normal titration
useful if working out amount of acid/base in non-soluble solid

71
Q

What gives buffer highest capacity

A

highest concentration & equimolar amounts of acid and conjugate base

CHEM (6 decks)

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