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Chemistry 11U - 2023 > Unit 4 Review - Chemistry of Solubility > Flashcards

Unit 4 Review - Chemistry of Solubility Flashcards

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1
Q

Pure Substance

A

-a substance that contains only one kind of particle with definite physical and chemical properties
-either an element or a compound
ex. compound (H20)

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2
Q

Homogeneous Mixture

A

-a uniform mixture of only one phase
ex. tea, vinegar

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3
Q

Heterogenous Mixture

A

-a non-uniform mixture with 2 or more visible phases
ex. salad dressing, cereal, soil

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4
Q

Solute

A

-a substance that can dissolve in another substance

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5
Q

Solvent

A

-the substance that dissolves in another substance
-the compound in largest percentage is the solvent

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6
Q

Solution

A

-a homogeneous mixture of substances composed of at least one solute and one solvent
-always transparent if in liquid or gas form
ex. sugar water, air, bronze

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7
Q

Aqueous Solution

A

-solutes dissolved in water

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8
Q

Electrolyte

A

-compound that dissociates into ions when dissolved in a solvent enabling it to conduct electricity

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9
Q

Non-electrolyte

A

-compound that when dissolved in a solvent does not conduct electricity

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10
Q

What is behind the chemistry of solubility?

A

-the process of a solute dissolving in a solvent to make a solution is physical change
-the ability of a solvent to dissolve a solute depends on the forces of attraction between the particles
(properties some must be similar)

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11
Q

What is the rule governing solubility?

A

“like dissolves like”
-polar solvents only dissolve polar solutes
-non-polar solvents only dissolve non-polar solutes

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12
Q

Why is water the universal solvent?

A

-water is the universal solvent because it is capable of dissolving a variety of substances
-its success as a solvent is due to its size, high polar nature (polar bonds), capacity for hydrogen bonding
-a force of attraction between two polar molecules, where an electropositive hydrogen atom from one polar molecule is attracted to an atoms with a high electronegativity (ex. O, N, F) of another polar molecule

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13
Q

Explain the solubility of polar molecules in H20

A

-polar molecules, having areas of slight positive charge and areas of slight negative charge, can attract one another due to electrostatic attraction
-this attraction allows a polar solvent to dissolve a polar solute
ex. water dissolves ammonia

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14
Q

Solubility of ionic compounds in H20

A

-when an ionic compound dissolves in water they separate (dissociate) into individual ions
-this separation is illustrated using a dissociation equation
-the cation will attract the slightly negative regions of the water molecules
-the anion will attract the slightly positive regions of water molecules
(opposites attract)

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15
Q

Insolubility of non-polar molecules in H20

A

-unlike water, non-polar molecules lack positively and negatively charged regions
-thus water molecules have a much greater attraction to one another than non-polar molecules, and as a result do not mix
ex. water cannot dissolve gasoline

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16
Q

Solubility of non-polar solutes in non-polar solvents

A

-the absence of strong repulsive forces and the presence of small attractive forced between non-polar molecules allow them to intermingle easily and thus dissolve in one another
ex. oil dissolves gasoline

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17
Q

Can ionic compounds be considered polar?

A

yes

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18
Q

How do you determine if compounds are soluble in H20?

A

-use solubility table
(aq) = soluble
(s) = insoluble

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19
Q

Can soluble compounds act as electrolytes (conduct electricity) because they are soluble in water?

A

yes as this indicates they dissociated into ions, therefor conduct electricity within the solution of H20

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20
Q

How do you see if substances can dissolve in one another?

A

see if they are alike (polar and non-polar), and if they are, they will dissolve in one another

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21
Q

What is the definition of solubility?

A

-the amount of solute that can dissolve in a given quantity of solvent at a certain temperature or pressure

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22
Q

What are the three different classes of solution that can exist based on on the amount of dissolved solute?

A

1) Saturated Solution: a solution that contains the maximum amount of solute that can dissolve in a given amount of solvent, and excess solute may be present, the rate at which solute dissolves is equal to the rate at which solute crystallizes

2) Unsaturated Solution: a solution that contains less the maximum amount of solute that can dissolve in a given amount of solute, all the solute molecules are dissolved and there is no crystallization

3) Supersaturated Solution: a solution that contains more dissolved solute than it would if it were saturated, unstable solution (any small agitation may initiate crystallization), achieved by gently heating and careful cooling of solution

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23
Q

Factors affecting solubility: size and charge

A

1) Ionic compounds
-generally the greater the charge on ions the less soluble the ionic compound due to a greater electrostatic attraction holding the ions together
-the larger the size of an ion the greater the solubility since the force of attraction between the cation and anion decreases as radius increases

2) Molecular Compounds
-the more polar bonds in a molecule generally the more soluble in water due to more attractive sites for water
-generally the smaller a molecule the more soluble due to a greater surface area in contact with solvent

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24
Q

Factors affecting solubility: temperature

A

Solid solute: solubility increases as the temperature increases, energy is required to break the bonds between the particles if solute and when temperature is higher the solute particles have more kinetic energy

Liquid solute: solubility is largely unaffected by changes by changes in temperature, bonds between particles in a liquid are not as strong as those between particles in a solid

Gas solute: solubility decreases as temperature increases, when dissolved in liquid the gas loses some energy, as temperature increases the dissolved gas gains anergy and comes out of a solution more easily

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25
Q

Factors affecting solubility: pressure

A

Solid and liquid solute: solubility is largely unaffected by changes in pressure

Gas solute: solubility of a gas is directly proportional to the pressure of the gas above the liquid
-high pressure above the liquid increases gas solubility
-low pressure above the liquid decreases gas solubility

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26
Q

What is electronegativity?

A
  • the relative ability of an atom to attract a shared electron pair
    -generally, metals have lower electronegativity values evidenced by their tendency to lose electrons to achieve stability
    -non-metals have greater electronegativity values evidenced by their tendency to gain electrons to achieve stability
    the type of bond that forms between two atoms can be determined by calculating electronegativity difference
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27
Q

When a non-polar (molecular) compound is being labelled, what is the extra step needed to take to ensure that the compound is actually molecular?

A

-calculating electronegativity difference between both elements
0 - 0.4 : non-polar
0.4 - 0.7 : polar
0.7 - 1.4 : ionic bond

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28
Q

What is solution concentration within solution preparation?

A

-concentration of a solution refers to the ratio between the quantity of solute dissolved per quantity of solution

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29
Q

Dilute VS. Concentrated solution

A

dilute: has a relatively small amount of solute dissolved in the solvent
concentrated: has a relatively large amount of solute dissolved in the solvent

30
Q

What is a standard solution?

A
  • a solution with a concentration that is known precisely and accurately
    -prepared in volumetric flask (flask calibrated to measure and hold a fixed volume of solution)
31
Q

What is the equation used for preparation of a standard solution from solid, using molar concentration formula to calculate mass?

A

C = n/V
V = n/C
n = C x V

MASS FORMULAS!!!
m= nxMx
Nx = nxNA

32
Q

What is the materials and apparatus list for a standard solution / concentration problem for mass problem?

A

MATERIALS
-compound, grams
-distilled water

APPARATUS
-volumetric flask, volume
-electronic balance
-funnel

33
Q

What is solution dilution within solution preparation?

A

-the process of decreasing the concentration of a solution by adding additional solvent
-requires the transfer of a precise volume of liquid
(with dilution only the volume of solution changes, the amount of solute stays the same)

34
Q

What is the difference between a volumetric transfer pipette and a graduated transfer pipette?

A

volumetric: calibrated to measure and deliver one fixed volume of liquid
ex. 11mL

graduated: calibrated to measure and deliver a range of volumes of a liquid
ex. 0.32 mL

35
Q

What is the solution dilution formula used for calculating solutions as stocks?

A

CiVi = CfVf

Ci: initial concentration
Vi: initial volume

Cf: final concentration
Vf: final volume

36
Q

What is the materials and apparatus list for a solution dilution formula used for calculating solutions as stock problem?

A

MATERIALS:
-compound, volume and concentration INITIAL
-distilled water

APPARATUS:
-volumetric flask, volume FINAL
-funnel
-graduated transfer pipette

37
Q

Are acids the only molecular compounds that act as electrolytes?

A

yes and this is because they break apart into ions when dissolved in H20

38
Q

Do all molecular compounds conduct electricity?

A

no, only acids, molecular compounds do not dissolve in H20 and therefor cannot dissociate into ions and conduct electricity

39
Q

What do dissociation equations show?

A

the process of ionic compounds dissolving in water into individual cations and anions

40
Q

In a dissociation equation, are the ions reacting or the compounds?

A

the ions

41
Q

Ionic equation

A

equation where all the high soluble ionic compounds are dissociated into ions

42
Q

Net ionic equation

A

equation that identifies specifically which ions participate in the overall chemical reaction

43
Q

How do you determine if a reaction has occurred in a solution?

A

write double displacement reaction with states
ionic equation
net ionic equation

44
Q

What are spectator ions?

A

ions that do not take part in a reaction, ions that exist on both sides of an equation, cancelling them out is what creates a net ionic equation

45
Q

Why do net ionic equations form?

A

the attraction to the ions between one another is stronger than water attraction to the other ions

46
Q

What is dissociation?

A

the separation of an ionic compound into its component cations and anions when dissolved in H20

47
Q

What is ionization

A

the formation of ions when a neutral molecule is dissolved in H20

48
Q

What is Arrhenius’ theory of acids and bases?

A

ACID:
molecular substance that ionizes in water to release one or more hydrogen ions (H+ aq)

BASE:
ionic substance that dissociates in water to release one or more hydroxide ions (OH+ aq)

49
Q

What is Arrhenius’ theory of strong vs weak acids and strong bases?

A

Strong acid:
an acid that completely ionizes (>99%) in H20 to release hydrogen (H+) ions

Weak acid:
an acid that partially ionizes (<50%) in H20 to release hydrogen (H+) ions, they exist along others in the form of molecules, or exist in the presence of oxygen

Strong base:
an ionic hydroxide that dissociates completely (>99%) in H20 to release (OH-) ions

50
Q

What is the difference between strong and weak vs concentrated and dilute?

A

-strong and weak refer to the degree of ionization or dissociation of particles in water
-concentrated and dilute refer to the amount of solute in the solvent
-a strong acid and base can be made into both concentrated and dilute solutions as can a weak acid and base

51
Q

List the properties of an acid

A

taste: sour
feel of solution: astringent
electrical conductivity: conducts
pH: less than 7
litmus paper colors: blue turns red, red stays red
phenolphthalein: colourless
reactions with alkali metals: produce hydrogen gas
reactions with carbonate compounds: produces carbon dioxide gas
examples of acids: citrus fruits, vinegar, carbonated beverages

52
Q

List the properties of a base

A

taste: bitter
feel of solution: slippery to touch
electrical conductivity: conducts
pH: greater than 7
litmus paper colors: blue stays blue, red turns blue
phenolphthalein: magenta
reactions with alkali metals: no characteristic reaction
reactions with carbonate compounds: no characteristic reaction
examples of bases: soap, toothpaste, oven cleaner

53
Q

What does pH stand for and what does it do?

A

-power of Hydrogen
-measures the acidity of a solution
-range is 0-14

tools sed to measure pH:
-pH meter (determines [H+]
-universal indicator paper (paper reacts with [H+] and changes color

54
Q

Describe how you interpret pH

A

-the pH scale is based on a logarithmic scale
-the logarithm of a number is the power to which 10 is raised to, each step up or down the pH is a jump of 10

ex. pH of 12 is 10,000 times greater than pH of 8

55
Q

Name the range within a pH scale

A

0 - 4: strong acid
4 - 7: weak acid
7: neutral
7 - 10: weak base
10 - 14: strong base

56
Q

Acid base titration
What is the useful function of titration

A

-determining concentration of a solution for which the concentration is not known
-verifying the concentration of an existing labeled solution (quality control)

57
Q

What is the titration procedure

A

-the concentration of the solution of interest is determined by observing its reaction with a solution of known concentration (standard solution)

58
Q

What is equivalence point?

A

-the aim of titration is to find the point at which the number of moles of the standard solution is stoichiometrically equal to the number of moles of the unknown solutions (represents complete reaction)
-this quantitative point is called the equivalence point
-the equivalence point marks when neutralization has occurred (the moles of H+ from the acid have reacted with an equal amount of OH- from the base)

59
Q

What is the endpoint?

A

-provides qualitative evidence that the equivalence point has been achieved
(no visible sign indicates the occurrence of a neutralization reaction so an acid/base indicator is added which changes color in an acidic compares to a basic solution
-the indicator changing color shows that the endpoint has been achieved, signifying neutralization occurring

60
Q

What are the endpoint indicators when phenolphthalein are added?

A

acid: colorless
base: magenta
neutral: pale pink

61
Q

What are the differences in endpoint and equivalence point when referring to titration?

A

endpoint:
-observable
-sudden observable change (color pH)
-occurs when an acid-base indicator
-reacts with the titrant to produce lasting color change
-depends on the type of indicator used

equivalence point:
-theoretical
-cannot be observed
-occurs when an acid and a base have completely neutralized each other
-depends on the stoichiometry of the neutralization

62
Q

How do you read a burette?

A

reading is recorded to two decimal places (second is an estimate)

63
Q

What is the mathematical formula for calculating pH?

A

pH = -log [H+]

64
Q

What is the mathematical equation for calculating [H+]

A

[H+] = 10^-pH

65
Q

What are the three unique properties of water and how are they advantageous to living organisms?

A

high surface tension: pulls water into round droplets and allows small insects to “walk on water”

expansion when cooling from 4 to 0: causes water to freeze from the top down, allowing life to continue below it as ice floats

inability to mix with non-polar compounds: enables organisms to retain water because of a waterproof coating

66
Q

Define potable

A

the term used to describe water that is suitable for drinking, several natural processes purify water as it passes through the water cycle (evaporation results in source of potable water as when water evaporates existing solutes are left behind, and when this evaporated water condenses it is very pure)

67
Q

What are the three categories of water contaminants?

A

Physical contaminant:
-floating debris (twigs)
-fine suspended particles (sand)

Biological contaminant:
-micro-organisms (bacteria, viruses)
(e. coli bacteria)

Chemical contaminant:
-fertilizers and pesticides
(nitrates, phosphates)

68
Q

Define leachate

A

a liquid contaminated with dissolved or suspended substances picked up as the liquid passed through old mines or dump sites, it pollutes nearby bodies of water or underground aquifers

69
Q

Define water footprint

A

measure of the total volume of freshwater used to produce services consumed by an individual

70
Q

Why do some waters taste different?

A

not all water is created equal, composition is dependent on where it comes from (aquifers or lakes) will vary

Chemistry 11U - 2023 (4 decks)

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