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Chemistry > Chapter 12: Water as a Solvent > Flashcards

Chapter 12: Water as a Solvent Flashcards

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1
Q

What is water often described as ..

A

“universal solvent”

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2
Q

WhAT IS water an excellent solvent for?

A

Many ionic and polar substances.

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3
Q

What does a readily dissolved substance depend on?

A

The polar nature of the water molecules

The nature of substance that dissolves in it.

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4
Q

What happens to molecular compounds mixed with water?

A

Some dissolve: Some Ionic compounds

Some are insoluble: Oil

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5
Q

What are the key factors of substances mixing with water?

A
  • Biological
  • Domestic
  • Industrial situations
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6
Q

What is a precipitation reaction?

A

Two solutions reacts and produce an insoluble product

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7
Q

Solute meaning?

A

Substance that is dissolved

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8
Q

Solvent meaning?

A

Liquid that the solute is dissolved in

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9
Q

Together was does Solute & Solvent form?

A

A homogenous solution

uniform composition and properties throughout the whole solution.

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10
Q

Aqueous solution meaning?

A

Solvent is water..thats what the solution is called

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11
Q

Solubility meaning?

A

Extent to which SOLUTE can dissolve in a solvent.

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12
Q

What is Solubility also determined by?

A

Polar or non-polar nature of the solute and the solvent.

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13
Q

‘like dissolve like’ according to chemist mean

A

Strongly polar and ionic solutes tend to dissolve in polar solvents,

and non-polar solutes tend to dissolve in non-polar solvents

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14
Q

Process of dissolving also depend on..

A

Strength of the attraction or bonds between the solute particles, and

the attraction between the solvent particles and the new bonds that form between the solute and the solvent.

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15
Q

What is strength related to..?

A

Size of the energy required to break these bonds, compared to the energy released when the new attractions or bonds are formed.

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16
Q

Why is water an effective solvent?

A

Due to its polarity and ability to form hydrogen bonds.

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17
Q

What is energy used for?

A

Energy is required to break bonds

Energy is released when new bonds form

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18
Q

what happens when ionic compounds dissolve in water.

A

Cations attract to ned end of water and anions attract pos end of water.

If strong enough it breaks bonds between cation and anions,
compound dissolves

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19
Q

when ion dissolves in water its called

A

described as hydrated (contain water molecules within structure )

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20
Q

interaction between water ( any polar ) molecule and ion is

A

ion-dipole attraction

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21
Q

dissociation meaning

A

ions seperate when an ionic compound dissolves in a solvent

ions are surrounded by water molecules and cannot recombine

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22
Q

when ionic substances dissolve in water..

A

they dissociate (ions separates )

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23
Q

What if strength of ions are very strong?

A

The water molecules are unable to seperate the ions and the salt is insoluble

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24
Q

insoluble meaning

A

will NOT DISSOLVE

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25
Q

molecular meaning

A

group of atoms bonded together covalently

many do not dissolve in water

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26
Q

What is it called when molecules dissolve in water

A

Are highly polar, and described as dipoles

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27
Q

diff between polar and non-polar

A

non-polar: even distribution of charge

polar: uneven distribution of charge due to differences in electronegativity of the atoms

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28
Q

Polar molecules will dissolve in water cause they either (2)..

A
  1. Form ions in water

2. Form hydrogen bonds with water

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29
Q

Molecular compounds that ionise in water example

Why does it happen

A

HCl = hydrogen chloride ( highly polar )

Hydrogen ions combine with water = hydronium ions H3O+

Aqueous solution = hydrochloric acid

Attraction of the polar water molecule increase polarity of H-Cl bond … neg attracts H and so and pulls it away.

H atom covalently bonds with water ( aqueous )
Cl becomes aqueous ( the anion dissolves ) ( aqueous )

Both ions are hydrated and dorm ion-dipole interactions

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30
Q

Ionisation meaning

A

Process polar molecules compounds form ions when dissolved in water

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31
Q

What does highly polar molecular substances usually do?

A

They ionise in water when they dissolve.

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32
Q

What are the other molecular compounds that are soluble in water?

A

Molecules usually having hydrogen atom bonded to one F, O or N.. they dissolve by forming hydrogen bonding with water.

example: NH3 ammonia

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33
Q

Simplify four molecular compounds that dissolve in water.

A
  1. Ions : cation and anion
  2. Ionisation of molecular ( ion and hydrogen )
    UNLESS THE BOND IS TOO STRONG LIKE AgCl
  3. Hydrogen bond with F, O , N
  4. Alcohol molecules
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34
Q

Why are alcohol molecules soluble?

A

Form hydrogen bonding such AS with CH3OH

CH3-OH : methanol

the OH is highly polar + water = hydrogen bonding
however hydrogen bonding does not occur with CH3 due to small electronegativity / not very polar

so bond is like CH3-OH-0HH

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35
Q

Interesting about water & alcohol molecules interaction?

A

They take up less volume due to rearrangement of the molecules.

The volume of combined liquids is less than the sum of individual volumes.

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36
Q

Miscible meaning?

A

Two liquids able to be mixed and form a solution

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37
Q

Immiscible meaning?

A

Two substances are unable to form a homologous solution = form seperate layers

38
Q

Example of Immiscible?

A

Oil and vinegar ( aqueous sol )

Oil is non polar molecules will only dissolve in non-polar solvents.

39
Q

Why don’t polar and non-polar mix?

A

Non-polar molecules have weak dispersion forces and little energy required to seperate them.

WATER IS strongly bonded and tend to stick together and not interact with non-polar

40
Q

Rules for polar and non-polar mixes (3)

A

Polar + polar = solution
non-polar + non-polar = solution
polar+ non-polar = suspension ( wont mix evenly )

41
Q

What does carbon dioxide and water form?

A

Weakly acidic solution, so if soft drink have been open it loses carbon dioxide gas and result is flat taste.

42
Q

What else influences the amount of has that dissolved in water?

A

Temperature

Increase = temp causes decreases the solubility of gases in liquids.

43
Q

What does dissolved oxygen do in sea water?

A

The dissolved oxygen in sea water decreases as the temp increases

and this has significant implication for survival of seas organisms.

44
Q

The solubility of gas in liquid decreases…

A

with increasing temperature

45
Q

What is Electrical conductivity used to test?

A

What is useful to test the quantity ions formed in a solution

46
Q

When does a substance conduct electricity?

A

Contains charged particles that are able to move

47
Q

Does water conduct electricity? why

A

No, even though the molecules move freely in liquid state,

the covalent bonding in water molecules, results in a neutral molecules

pure water might sometimes conduct slightly

48
Q

Why might pure water conduct electricity?

A

Slightly as it has small number of ions ( called self ionisation )

h2o(i) + h20(i) = h3o + oh-

49
Q

double reversible arrows?

A

reaction simultaneously reacting in the forward direction and in the reverse direction.

50
Q

electrolytes?

A

substances that produce ions when dissolved

51
Q

conductivity of solutions can be used..

A

to compare the quantity of ions present

52
Q

Why is water a good solvent for ionic compounds?

A
  • Water molecule had polar arrangement pf oxygen and hydrogen atoms
  • h = pos , o=neg charge….
  • “disrupt attractive forces that hold the ionic compounds” together = dissolves it
53
Q

what needs to be broken, to form ion-dipole interaction between ions and water

A
  1. ions must be broken

2. hydrogen bonds between water molecules

54
Q

compare water and oil molecules

A

oil:
- non- polar
- weak dispersion forces

water:
- polar
- hydrogen bonding

55
Q

when talking about molecules mention:

PSI
polarity, strength, intermolecular

A

polar or not
WEAK or STRONG
intermolecular : dipersion, dipole, or hydrogen

56
Q

INTERACTION when dissolve in water

1: ionic compound
2: polar molecular compound
3: molecular compound:

A

1: ion-dipole interaction
2: ion-dipole interaction
3: hydrogen bonding

57
Q

differences and similarities of gases

NH3 & HCl

A

BOTH: polar molecules

diff:
NH3 -> dissolves by forming hydrogen bonds with water

HCl -> H+ Cl- ——> ionises in water & ions become hydrates

58
Q

precipitate

A

solid with low solubility formed in a liquid

59
Q

solubility

A

grams of substance that will dissolve in an amount of solvent at a particular temperature

60
Q

precipitation reaction

A

reaction where two solutions are mixed and a solid is formed

unreacted ions remained in the solution

61
Q

why can’t water dissolve some substances

A

water is unable to dissociate the ionic lattice structure and they are therefore insoluble

62
Q

what ion is most commonly soluble with water

A

nitrate!! NO3-

also K+ AND Na+

63
Q

(aq) meaning

A

each ion is separated and has become surrounded by water molecules

64
Q

spectator ions

A

ions that take no part in reaction but maintain electrical neutrality in a solution

65
Q

step for balanced perception full equation

6 STEPS

A
  1. write reactants
    optional ( write out products of each react )
  2. write out overall product ( switching )
  3. write skeleton equation ( reactant and products )
  4. Balance equation
  5. Use solubility table
  6. ADD STATE
66
Q

ionic equations

A

equation without the spectator ions

a simpler equation, that only show the species that are formed or changed in a reaction

67
Q

why does spectator ions not included in ionic equations?

A

because they remain in solution unchanged in the reaction

68
Q

steps for writing ionic equations

A
  1. write the balance full chemical equation
  2. expand equations by dissociating all the SOLUBLE compounds into their free ions (( check if any substances such as acids or bases that react with water to produce ions ))
    replace the formula by ions that are formed
  3. cancel free ions that are uncharged in both sides of the equation ( spectator ions )
  4. write ions and formula remaining ( this is ionic equation )
  5. make sure equation is balanced in charge as well as in number of atoms and add symbols of state
  6. spectator ions are still in solution so write these with commas between
69
Q

what happens to spectator ions in ionic equations?

A

they are omitted

70
Q

precipitate remains in filter paper is called

A

residue

71
Q

clear solution in the conical flask is

A

filtrate and contains spectator ions

72
Q

solvent properties of water in biological contexts?

A

for body
rivers
plants

73
Q

solvent properties of water in domestic contexts?

A

garden
beverages
personal care products

74
Q

solvent properties of water in industrial contexts?

A
  • water facilitates
  • electrolysis reactions
  • many chemicals
  • manufacturing industries ( production of foods, medicines, fertiliser, detergents etc )

surfactants: contain molecules that are polar at one end and non-polar at the other. this allows to dissolve both water and pil. making suited cleaning agents where oil-and grease needs to be removed.

75
Q

water benefit human body

A

transport nutrients ans soluble chemicals
around body to different cells
and carries waste

76
Q

dissolved substances keep plants and fish alive in ponds

A

oxygen and carbon dioxide slightly soluble in water
fish can have oxygen for respiration
plants can have carbon dioxide for photosynthesis

77
Q

how does water act as a solvent in a meal?

A

vinegar is ethanoic acid in water

soft drinks has dissolved sugar etc

78
Q

why is it important that fertilisers are soluble in water

and problem it results

A

fertilisers can be sprayed on crops
solution absorbed through plant roots

excess nutrients can be washed into rivers, lakes etc
oxygen used in the decay process so fish are unable to survive.

79
Q

how is water useful in the industrial production of materials?

A

chemicals can be diluted with water for reasons of safety.

80
Q

disadvantages there is in the use of water in chemical industries?

A

contaminated water may be difficult to dispose
it might enter waterways
cause pollutions

81
Q

what does oxygen and nitrogen have

A

non-polar gases have low solubility, but enough sustain aquatic life

82
Q

an increase in pressure generally

A

decreases the solubility of a gas in liquid

83
Q

what is not a characteristic of solution

A

solute particles can be separated by filtering

84
Q

ions dissolve in water ..

A

pos ion goes with neg end
neg ions goes with pos end in ionic lattice
ion-dipole bonds are formed
ions are separated by water molecules that surround ions
ions are described as hydrated

85
Q

as an ionic formular such as KCl (aq) , is mixed with water and is evaporated?

A

the solution will form solid crystals of potassium chloride.

86
Q

Why can water have no net charge but have slight charges in different parts of the molecule?

A

The oxygen end is slightly negative and the hydrogen end is slightly positive

87
Q

Fish need oxygen from which molecule?

A

O2

88
Q

A water strider can skate along the top of a pond because:

A

hydrogen bonds result in water cohesion (surface tension)

89
Q

Attractions between water molecules are called

A

Hydrogen bonds

90
Q

Which of these would LEAST affect turbidity?

A

Salt

Chemistry (3 decks)

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