Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > Module Six - Acid/Base Reactions > Flashcards

Module Six - Acid/Base Reactions Flashcards

Properties of Acids and Bases Using Brønsted–Lowry Theory Quantitative Analysis

1
Q

what is an oxyanion?

A

inorganic acid that has an oxygen attached to an element (S, N, P, C)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what is the name of HNO3?

A

nitric acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is the name of HCl?

A

hydrochloric acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is the name of HNO2?

A

nitrous acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what is the name of HCN?

A

hydrocyanic acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what is a binary acid?

A

acid that has a monoatomic ion attached

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

how are binary acids named?

A
  1. prefix - ‘hydro-‘
  2. identify the anion
  3. replace ‘-ide’ with ‘-ic’
    e. g. cyanide –> cyanic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what is a monoatomic ion?

A

has a charge of +1/-1

e.g. Cl-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what is a polyatomic ion?

A

has a charge greater than 1

e.g. SO4(2-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

how is an inorganic acid with a polyatomic ion named?

A
  1. replace polyatomic ion suffix
    i.e. ‘-ite’ –> ‘-ous’
    i.e. ‘-ate’ –> ‘-ic’
  2. add ‘acid
    e.g. nitrite –> nitrous
    nitrate –> nitric
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what are the common properties of inorganic acids?

A
  • sour taste
  • conducts electricity
  • turns blue litmus to RED
  • react with and dissolve active metals with the release of a gas
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what are the common properties of inorganic bases?

A
  • soapy feel (aqueous)
  • bitter taste
  • conducts electricity
  • turns red litmus BLUE
  • do not react with carbonates
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

define acid.

A

substance that produced hydrogen ions (H+) in solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what does the H+ ion do when released from an acid in solution?

A

attaches to a water molecule to form hydronium ions (H3O+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

define base.

A

e that either contains oxide (O2-) or hydroxide ion (OH-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what is an acid-base reaction called?

A

neutralisation reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what is the general formula for an acid-base reaction?

A

acid + base –> salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what is an example of a base containing the oxide ion?

A

MgO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is an example of a base containing the hydroxide ion?

A

NaOH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what is the reaction between HCl and NH3?

A

HCl(aq) + NH3(aq) –> NH4Cl(aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

why is ammonia considered a base?

A

NH3(g) + H2O(l) –> NH4-(aq) +OH-(aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

why is the ammonium ion considered an acid?

A

will react with a base to form salt and water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what is the general formula for an acid-carbonate reaction?

A

acid + carbonate –> salt + carbon dioxide + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

what is the general formula for an acid-metal reaction?

A

acid + metal –> hydrogen gas + salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

what is an example of an acid-metal reaction?

A

2HCl(aq) + Mg(s) –> MgCl2(aq) +H2(g)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

what is an example of an acid-carbonate reaction?

A

2HCl(aq) + CaCO3(s) –> CaCl2(aq) + H2O(l) + CO2(g)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what is the general formula for an acid-hydrogen carbonate reaction?

A

acid _ hydrogen carbonate –> salt + water + carbon dioxide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

what is an example of an acid-hydrogen carbonate reaction?

A

HCl(aq) + NaHCO3(s) –> NaCl +H2O(l) +CO2(g)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

what is the hydrogen carbonate ion?

A

HCO3-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

what is the difference between a carbonate ion and a hydrogen carbonate ion?

A

carbonate : HCO3

hydrogen carbonate: CO3(2-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

what is enthalpy?

A

measure of the total energy possessed by a substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

is energy required to break bonds or form bonds?

A

break bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

is energy released when breaking bonds or forming bonds?

A

formation of bonds babey

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

is the enthalpy change of an exothermic reaction positive or negative?

A

negative!!

∆H= -ve

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

is the enthalpy change of an endothermic reaction positive or negative?

A

positive

∆H= +ve

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

how can ∆H be calculated using the enthalpy of species in a reaction?

A

∆H = ∑(enthalpy of products) - ∑(enthalpy of reactants)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

is the enthalpy of the reactants greater or lower than the products in an exothermic reaction?

A

greater (energy is lost in reaction)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

is the enthalpy of the reactants greater or lower than the products in an endothermic reaction?

A

lower (energy is absorbed)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

what is the standard enthalpy of neutralisation?

A

∆H when an aqueous acid and base react to form 1 mole of water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

what is the specific heat capacity of water?

A

4.18J/K/g

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

what is the specific heat capacity unit?

A

J/K/g

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

what is specific heat capacity?

A

joules of energy required to rise the temperature of the substance by 1˚C

43
Q

how is the quantity of heat (q) calculated?

A

q = mC∆T

44
Q

how is change in enthalpy (∆H) calculated from quantity of heat (q)?

A

∆H = (-q)/n

q must be in KJ

45
Q

is the reaction between NaOH and HCl endothermic or exothermic?

A

exothermic

46
Q

can neutralisation be both endothermic and exothermic?

47
Q

is neutralisation endothermic or exothermic?

A

always exothermic

48
Q

what an application of neutralisation in everyday life?

A
  • antacid to assist with heartburn/indigestion

- toothpaste

49
Q

how does heartburn occur?

A
  • too much HCl in the stomach

- begins to travel up oesophagus and burn the tissues

50
Q

how do antacids help with heartburn?

A

neutralises the stomach acids

51
Q

how do antacids relate to neutralisation?

A
  • contains a base [e.g. Mg(OH)2]

- neutralises extra acid

52
Q

is toothpaste acidic or alkaline?

53
Q

why is toothpaste alkaline?

A

neutralises acids in food we eat to prevent teeth enamel from breaking down

54
Q

how can neutralisation be used in industry?

A
  • neutralisation of soil

- neutralisation of waste waters

55
Q

why is neutralisation of soil important?

A
  • plants ability to grow is affected

- some plants can survive in acidic/basic environments though

56
Q

why is neutralisation of waste waters important?

A

if acidic/alkaline waters enter creeks and rivers, habitats and aquatic life will be hurt

57
Q

who are the five acid and base theorists?

A
  • Lavoisier
  • Davy
  • Arrhenius
  • Brønsted–Lowry
  • Lewis
58
Q

what did Antoine Lavoisier (1776) discover ?

A
  • the oxygen theory

- he demonstrated that non-metal oxides react (dissolved) with water to form acidic solutions

59
Q

what was Laviosier’s conclusion from his discovery?

A

concluded that an acid must contain oxygen

60
Q

what is a limitation of Lavoisier’s theory?

A

not all acids contain oxygen!!
e.g. HCl
He could also not explain why metal oxides were not acidic

61
Q

what did Humphry Davy (1810) discover?

A
  • the hydrogen theory
  • he observed that when HCl gas and H2S gas dissolved in water they produced acidic solutions. These molecules had no
  • recognised that the key element in acids was hydrogen
  • metals with oxygens were bases
  • acid + base –> salt + water
62
Q

what was Davy’s theory?

A

acids are substances which contain replaceable hydrogens which could be displaced by metals in solution

63
Q

what are the limitations to Davy’s theory?

A
  • not all substances that contain hydrogen are acids
  • some acid-base reactions don’t produce salt and water
  • no distinction between weak and strong acids
64
Q

what is Arrhenius’ definition of an acid?

A

substances that dissociate and ionise in water (produce H+)

65
Q

what is Arrhenius’ definition of a base?

A

substances that dissociate in water to produce hydroxide ions (OH-)

66
Q

what are the limitations to Arrhenius’ theory?

A
  • could not explain why ammonia (NH3) was a base

- does not apply to non-aqueous solvents

67
Q

what is an example of Arrhenius’ acid-base model?

A

HCl dissociates in water to produce H+ and Cl- ions

68
Q

what is Brønsted–Lowry’s definition of an acid?

A

acids are proton donors

69
Q

what is Brønsted–Lowry’s definition of a base?

A

bases are proton acceptors

70
Q

what limitation of Arrhenius did Brønsted–Lowry’s theory work out?

A

able to explain why NH3 was a base

71
Q

what is an example of a Brønsted–Lowry acid?

A

HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq)

- HCl accepts a proton!

72
Q

what is an example of a Brønsted–Lowry base?

A

NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq)

- NH3 accepts a proton!

73
Q

how is a conjugate base formed?

A

when an acid loses a proton

74
Q

how is a conjugate acid formed?

A

when a base gains a proton

75
Q

how many protons do conjugate acid-base pairs differ from?

76
Q

will a strong acid produce a strong or weak conjugate base?

77
Q

will a weak acid produce a strong or weak conjugate base?

78
Q

will a strong base produce a strong or weak conjugate acid?

79
Q

will a strong acid produce a strong or weak conjugate base?

80
Q

what is the conjugate base of HCl?

81
Q

what is the conjugate acid of NH3?

82
Q

what are the limitations of Brønsted–Lowry’s theory?

A
  • solvent must be present (allows transfer of protons)
  • unable to explain reactions between acidic oxides and basic oxides w/o a solvent
  • unable to explain reaction between non-protonic (no H+) solvents
83
Q

what are examples of acidic oxides?

A

CO2, SO2, SO3

84
Q

what are examples of basic oxides?

A

CaO, BaO, MgO

85
Q

what is an example of non-protonic solvents?

86
Q

what is Lewis’ definition of an acid?

A

an acid is an electron pair acceptor

87
Q

what is Lewis’ definition of a base?

A

a base is an electron pair donator

88
Q

what are the limitations of Lewis’ theory?

A
  • all acid-base reactions do not involve coordinate bond formation (e.g. HCl, H2SO4)
  • does not explain strength of acids and bases
89
Q

what is the pH scale used for?

A

to quantitatively measure the acidity of a solution

90
Q

what does pH stand for?

A

hydrogen power

91
Q

how is the pH value calculated from the [H+]?

A

pH = -log[H+]

92
Q

how is [H+] calculated from the pH value?

A

10^-n

n is the pH value

93
Q

how is concentration different from strength in acids and bases?

A

concentration : amount of solute in a solution (concentrated - diluted)
strength : degree of ionisation (strong - weak)

94
Q

what makes an acid/base strong?

A

ability to ionise completely

95
Q

what makes an acid/base concentrated?

A

less solute in solution

96
Q

what are examples of a strong acid?

A

HCl, H2SO4

97
Q

what are examples of a weak acid?

A

CH3COOH. H2CO3

98
Q

what are examples of a strong base?

99
Q

what are examples of a weak base?

A

NH3, CH3NH2

100
Q

what is a polyprotic acid?

A

acids that can give up more than one proton!

101
Q

What is the pH range of methyl orange?

A

pH range between 3.2 (red) and 4.4 (yellow)

102
Q

What is the pH range of bromothymol blue?

A

pH range from 6.0 (yellow) to 7.6 (blue)

103
Q

What is the pH range of phenolphthalein?

A

8.2 (colourless) to 10 (pink)

104
Q

How is the acidity of soil measured?

A

White barium sulfate is added to a wet soil sample in a petri dish. When the universal indicator is added to the white later the colour change reveals the pH of the soil water.

Chemistry (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions