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Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

What is a Brønsted-Lowry acid

A

proton donor (H+)

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2
Q

What is a Brønsted-Lowry base

A

proton acceptor

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3
Q

How to identify a conjugate base

A

it will have one less H

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4
Q

How to identify a conjugate acid

A

it will have one more H

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5
Q

What is an amphiprotic substance

A

it can donate and accept protons

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6
Q

Examples of amphiprotic substances

A

H20, H2PO4-, HCO3-, NH3

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7
Q

metal + acid

A

salt + hydrogen

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8
Q

metal oxide + acid

A

salt + water

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9
Q

metal hydroxide + acid

A

salt + water

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10
Q

metal carbonate + acid

A

salt + water + carbon dioxide

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11
Q

what is neutralisation

A

when an acid and a base react together to form a salt and water

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12
Q

How do you calculate the Ph

A

-log[H+]

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13
Q

What does the Ph tell you

A

Ph > 7: basic, more OH- than H+
Ph <7: acidic, more H+ than OH-
Ph = 7: neutral

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14
Q

The Ph scale

A

x10 when going down the Ph scale
/10 when going up the Ph scale

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15
Q

What is the equilibrium constant of water

A

Kw = [H+] [OH-] = 1.0 x10^-14

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16
Q

When do you use the equilibrium constant of water

A

when calculating the PH or POH of strong acids and bases

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17
Q

What is the most accurate way to measure pH

A

using a Ph meter

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18
Q

Why is the universal indicator not used in titrations

A

it only gives a relatively slow gradual colour changes, that are not precise enough to determine an end point accurately

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19
Q

What is a strong acid

A

an acid that dissociates in water completely

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20
Q

What is a strong base

A

a base that dissociates in water completely

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21
Q

What is a weak acid

A

an acid that dissociates partly in water

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22
Q

What is a weak base

A

a base that dissociates partly in water

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23
Q

Examples of strong acid

A

HCl, HNO3, H2SO4, HBr, HI

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24
Q

Examples of weak acids

A

CH3COOH, H2CO3, H3PO4, propanoic acid

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25
Q

examples of weak bases

A

NH3, CH3CH2NH2,

26
Q

Examples of strong bases

A

NaOH, LiOH, KOH, Ba(OH)2

27
Q

How to determine the strength of a base or acid

A
  • ability to conduct electricity (strong acids and bases are good conductors of electricity)
  • rate of reaction (strong acids&bases will increase the rate of reaction)
  • PH (strong acids lower Ph, strong bases higher PH)
  • reactivity (strong acids&bases are more reactive)
28
Q

Conjugate Pairs & Acid-Base Strength

A

strong acid will have a weak conjugate base
Weak acid will have a strong conjugate base

29
Q

Why is rain naturally acidic

A

because of the dissolved CO2 and has a pH of 5.6

30
Q

How does acid deposition occur

A

when nitrogen oxides and sulphur oxides dissolve in water to produce HNO2, H2SO4 and H2SO3

31
Q

How are sulphur oxides made

A

Sulfur oxides can be formed from various natural processes, including the burning of sulfur containing fuels

32
Q

How are nitrogen oxides made

A

Nitrogen oxides can be produced in combustion (coal, gas, oil fueled power stations)

33
Q

The effect of acid deposition

A

Corrodes marble, limestone buildings and statues, leaching of soils and harms plants, causes the poisoning of fish, acidification of lakes

34
Q

What is a Lewis acid

A

a substance that acceptors a pair of electrons

35
Q

What is a Lewis base

A

a substance that donates a pair of electrons

36
Q

Define amphiprotic

A

acts as both a proton donor and proton acceptor

37
Q

Define amphoteric

A

acts as an acid and base

38
Q

How to calculate the concentration or PH of a strong acid/base

A

using the water product

39
Q

Outline the formation of sulfur based acids

A

S + O2 → SO2
SO2 + H2O → H2SO3

40
Q

Outline the formation of nitrous and nitric acid

A

2NO2 + O2 → 2NO3
2NO2 + H2O →HNO2 + HNO3

41
Q

What is the effect of acid deposition

A
  • leaching in soils
  • acidification of oceans
  • corrodes buildings
42
Q

How to reduce SO2 emissions

A
  • removal of sulphur from natural gas
  • renewable energy
43
Q

List examples of lewis acids

A
  • central metal ion in complex ions
  • electrophiles
44
Q

List examples of lewis bases

A
  • ligands
  • nucleophiles
45
Q

Give two-named examples of electron-deficient compounds

A

BF3 and NH3
- use them when proving a compound acts as a Lewis base

46
Q

What is the relationship between Kw and temperature

A

Kw is temperature-dependent
- an increase in temp. will decrease the PH of water but the concentration of H+ and OH- remain the equal

47
Q

State one assumption with calculations involving weak acids/bases

A

the salt concentration exits in a 1:1 ratio (equal concentration) with H+/OH-

48
Q

Outline the relationship between Ka and pKA

A

the greater the value of Ka, the smaller the pKa value
- high Ka value stronger weak acid

49
Q

What is the point of equivalence

A

the point at which the concentration of acid and base have been neutralised (only salt and water are present)
- mols of base = mols of acid

50
Q

What is the pH of the point of equivalence for strong acids and bases

A

7

51
Q

What is the half-equivalence point

A

the concentration of weak acid/base is equal to the concentration of conjugate base/acid
- pka = pH

52
Q

What is the pH of the equivalence point for weak acids and strong bases

A

ph>7

53
Q

What is the pH of the equivalence point for strong acids and weak bases

A

ph<7

54
Q

What is the endpoint

A

the point at which the colour changes in a titration

55
Q

What is the effect of an acidic solution on the equilibrium of an indicator

A

if solution acidic, the equilibrium shifts to the left (Hln)

56
Q

What is the effect of an alkaline solution on the equilibrium of an indicator

A

if solution is alkaline, the equilibrium shifts to the right (H+ + In-)

57
Q

What is a buffer

A

a solution that is resistant to changes in pH on the addition of small amounts of acid/alakali

58
Q

Outline the formation of an acidic buffer

A

1:1 ratio of weak acid and strong conjugate base
1:2 ratio of strong base and weak acid

59
Q

What is the Equation for an acidic buffer

A

CH3CH2COO- + H+ → CH3CH2COOH

60
Q

What is the equation for a basic buffer

A

CH3CH2COOH + OH- → H2O + CH3CH2COO-

61
Q

What is the half-equivalence point

A

half the volume needed to reach the equivalence point

62
Q

What are the products at the equivalence point

A

salt and water

Chemistry (12 decks)

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