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Bettel Plus Chang Chemistry > 7. Solutions And Colloids > Flashcards

7. Solutions And Colloids Flashcards

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1
Q

Homogeneous mixture/ Solution

A

-mixture uniform throughout molecular level
-air, sea
-all gas mixtures are homogeneous
-homogeneous solid mixture: alloy

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2
Q

Heterogeneous mixture

A

-distinct regions separated from each other by well-defined boundaries
-most solid mixture are heterogeneous

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3
Q

Alloy

A

-i.e. brass, steel
-melting solids ➡️ mixing molten components ➡️ allowing misture to solidify

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4
Q

Most common types of solutions

A

•Gas in liquid- carbonated water
•Liquid in liquid- wine
•Solid in liquid- salt water (saline soln)
•Gas in has- air
•Solid in solid- 14-carat gold

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5
Q

Properties of solution

A
  1. Distribution of particles is uniform
    -every part of solution has exactly same composition and properties
  2. Components of a solution do not separate on standing
  3. Solution cannot be separated into its components by filtration
  4. For any given solute and solvent, it is possible to make solutions of many different compositions
  5. Solutions are almost always transparent/clear (except solid solutions)
  6. Solutions can be separated into pure components (distillation, chromatography)
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6
Q

Acid rain

A

-raindrops contain CO2, O2, N2, SO2
CO2 + H2O ➡️ H2CO3 (carbonic acid)
SO2 + H2O ➡️ H2SO3 (sulfurous acid)
SO3 + H2O ➡️ H2SO4 (sulfuric acid)

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7
Q

Smelting

A

-melting or fusing an ore as part of separation process
-produces soluble gases
-acid rain

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8
Q

Solubility

A

-maximum amount of solid that will dissolve in a given amount of a particular solvent at a given temperature
-physical constant like melting point and boilinf point

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9
Q

Insoluble solids

A

-very low solubility in particular solvent

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10
Q

Soluble solids

A

-high solubility on particular solvent

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11
Q

Ethanol and water

A

-miscible in all proportions
-form solution no matter what quantities of each are mixed

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12
Q

Saturated solution

A

-solvent contains all the solute it can hold at a given temperature

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13
Q

Unsaturated solution

A

-solution containing lesser amount of solute than maximum

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14
Q

Supersaturated solution

A

-solution that contains more than the equilibrium amount of solute at a given temperature and pressure

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15
Q

Factors affecting solubility
1. Nature of solvent and solute

A

-polar compounds dissolve in polar solvents
-nonpolar compounds dissolve in nonpolar solvents

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16
Q

Factors affecting solubility
2. Temperature

A

-for most solids and liquids,
⬆️ Temperature ⬆️ Solubility (i.e. Glycerine, NaCl in water)
•exemptions: Li2SO4 in water

-for gases
⬆️ Temperature ⬇️ Solubility

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17
Q

Seeding

A

-molecules need a seed (surface on which to begin crystallizing) to precipitate
-addition of crystal of the solute to solution to provide surface onto whuch solute molecules can converge

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18
Q

Factors affecting solubility
3. Pressure

A

-little effect on solubility of liquids and solids
-for gases ⬆️ Pressure ⬆️ Solubility in a liquid

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19
Q

Henry’s law

A

-The solubility of a gas in a liquid is directly proportional to the pressure

-explains why carbonated beverage foams when it is opened
•bottle sealed under greater than 1 atm of pressure
•when opened at 1 atm, pressure decreases, solubility decreases
•excess CO2 is released, forming bubbles

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20
Q

Concentration

A

-amount of solute dissolved in a given quantity of solvent

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21
Q

Common units of concentration
1. Percent concentration

A

% w solute / v solvent
% w / w
% v / v

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22
Q

Common units of concentration
2. Molarity

A

M = moles solute / volume solution

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23
Q

Common units of concentration
3. Dilution

A

-only solvent is added in dilution
-moles of solute remain unchanged

M1V1 = M2V2

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24
Q

Common units of concentration
4. Parts per million

A

-for very dilute solution
ppm = (g solute / g solvent) x 10^6
ppb = (g solute / g solvent) x 10^9

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25
Q

Hydrated (for water only) or solvated ions

A

-when the combined force of attraction to solvent molecules is greater than the ionic bond of the crystal
-ions removed from crystals is surrounded by solvent molecules ,(solvated)

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26
Q

Water of hydration

A

Water molecules in a crystal

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27
Q

Hydrates

A

-Substances that contain water in their crystals
i.e. Gypsum CaSO4.2H2O
Plaster of Paris (CaSO4)2.H2O

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28
Q

Anhydrous crystals

A

-crystals without water

29
Q

Hygroscopic substance

A

-substance able to absorb water vapor from air

30
Q

Electrolytes

A

-substances that conduct electric current when dissolved in water or when in molten state
-i.e. NaCl

31
Q

Cathode

A

Negative electrode where cations migrate

32
Q

Anode

A

-positive cathode where anions migrate

33
Q

Non-electrolytes

A

-substances that do not conduct electricity
i.e. distilled water

34
Q

Electric conductance and concentration of ions

A

⬆️ion concentration ⬆️ electric conductance

35
Q

Strong electrolyte

A

-compounds that dissociate completely and conduct electricity

36
Q

Weak electrolyte

A

Compounds that dissociate into ions only partially and slighty conduct electricity

37
Q

Electrolytes in body

A

-important since it maintains acid-base balance and water balance
•cations: Na+, K+, Ca2+, Mg2+
•anions: HCO3-, Cl-, HPO4^(2-), H2PO4-

38
Q

Ionic solutions

A

-can be made from ionic compounds and covalent compounds as long as it is completely converted to ions in dilute aqueous solution
-conducts current

39
Q

When will covalent compounds dissolve in water

A

-if they can form hydrogen bonds eith water, provided that solute molecules are fairly small (no more than 3C atoms for each O,N,F atoms)

-covalent molecules that do not contain O,N,F are almost always insoluble in water (except for rare cases where covalent compound react with water, i.e. HCl)

40
Q

Importance of water in body

A

-dissolves ionic substances
-hydrates all polar molecules in body
-serves as vehicle to carry most of organic compounds, nutrients, and fuels as well as waste material

41
Q

True solution

A

-maximum diameter of the solute particles is about 1nm

42
Q

Colloid/ colloidal dispersion/ colloidal system

A

-diameter of solute particles ranges from 1-1000 nm (large particles)
-particles of this size have very large surface area
-stable (i.e. mayonnaise stays emulsified and does not separate into oil and water)
-not filterable by ordinary paper
-borderline homogeneous

43
Q

Basic characteristics of colloidal system

A
  1. Scatter light, appear turbid, cloudy, milky
  2. Form stable dispersions, do not form separate phases that settle out
44
Q

Tyndall effect

A

-light passing through and scattered by a colloid viewed at a right angle

*Light beam
@solution- not visible
@colloid- visible
@suspension- visible

Visible due to light scattering ability of colloid sized particles

45
Q

Suspensions

A

-size of colloidal particles is larger than about 1000 nm
-unstable; separate into phases
-filterable with ordinary paper
-transluscent or opaque

46
Q

Types of colloidal system

A

Gas in gas- none
Gas in liquid- whipped cream
Gas in solid- marshmallow
Liquid in gas- clouds, fog
Liquid in liquid- mayo, milk
Liquid in solid - cheese, butter
Solid in gas- smoke
Solid in liquid- jelly
Solid in solid- dried paint

47
Q

Brownian motion

A

-random, chaotic motion of any colloidal particles suspended in a solvent

48
Q

Why colloidal particles remain in solution despite all the collisions due to Brownian motion

A
  1. SOLVATION LAYER
    Most colloidal particles carry a large solvation layer
    -colloidal particle is surrounded by solvent molecules which move together with colloidal particle and cushion them; particles do not stick together when colliding
  2. SURFACE CHARGE
    Large surface area of colloidal particles acquires charges from the solution; colloidal particles repel each other due to like charges
49
Q

Solvation layer

A

-surrounding shell of solvent molecules

50
Q

Emulsion

A

-system, such as fat in milk, consisting of a liquid with or without emulsifying agent in an immiscible liquid, usually as droplets larger than colloidal size

51
Q

Emulsifying agent

A

-prevents immiscible solute and solvent from separating
-i.e. milk protein casein (oil droplets in milk)
Egg yolk in oil droplets in water

52
Q

Colligative property

A

-property of solution that depends only on the number of solute particles and not on the chemical identity of solute

53
Q

Colligative property
1. Freezing point depression

A

-the DECREASE in freezing point of a liquid caused by ADDING a solute

-application:
•Use of salts like NaCl and CaCl2 to melt snow in streets (lowers freezing point; mas mahirap ifreeze since need mas malamig)
•Use of antifreeze (i.e. ethylene glycol C2H6O2) in automobile radiators

54
Q

Colligative property
2. Osmotic pressure

A

-the amount of external pressure applied to the more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane

Normally, π=i.M.R.T for osmotic pressure

PERO!! if OSMOLARITY hinahanap (osmol unit)

Osmolarity=i.M

55
Q

Osmotic permeable

A

Very selective semipermeable membrane that only allows solvent molecules, and nothing else, to pass through

(Small molecules: solvent; large molecules: solute)

56
Q

Diffusion

A

-molecules will always diffuse from higher concentration to lower concentration

57
Q

Osmosis

A

-passage of solvent molecules from dilute solution to concentrated solution across semipermeable membrane

IMAGINE
May beaker tapos may semipermeable membrane (osmotic membrane) sa gitna

RIGHT PART: Pure water
LEFT PART: Solution (solute with water)

Water moves from dilute to concentrated (right to left) kasi higher concentration of water sa right tapos lower concentration of water sa left (since may solute)

Left side higher level sa right side kasi nag move na yung water molecules, pero hindi pwede masyadong malaki height difference due to gravity

Osmosis stops at unequal level. Level can be made equal if external pressure is applied to higher side

External pressure required: Osmotic pressure

58
Q

Concentration and osmotic pressure

A

⬆️ concentration ⬆️ osmotic pressure

59
Q

Reverse osmosis

A

-solvent flows from concentrated to dilute solution
-this happens when applied pressure in concentrated solution is GREATER THAN osmotic pressure
-used to make drinkable water from sea water or brackish water

60
Q

Osmotic pressure in biological organisms

A

-important since cell membranes are semipermeable; biological fluids must have proper osmolarity

61
Q

Isotonic

A

-two solutions with same osmolarity
-used in intravenous (IV) injections
-i.e. red blood cells in plasma; same osmolarity, no osmotic pressure is generated

62
Q

Hemolysis

A

-if red blood cells is suspended of distilled water instead of plasma
-rbc: 0.3 osmol; water: 0 osmol
-water flows to rbc; volume of rbc increases and swells
-membrane cannot resist osmotic pressure and rbc eventually burst, spilling contents in water

63
Q

Hypotonic solutions

A

-solutions in which osmolarity is lower than that suspended cells
-hypotonic solution will kill rbc by hemolysis

64
Q

Hypertonic solution

A

-solution has greater osmolarity than suspended cells

65
Q

Crenation

A
  • if rbc is placed in hypertonic soln (glucose solution); water flows from cells into glucose solution
    -shrivels cells
66
Q

Dialysis

A

Process in which a solution containing different sizes is placed in a bag of a semipermeable membrane. The bag is placed into a solvent or solution containing small molecules. The solution in the bag reaches equilibrium with the solvent outside allowing small molecules to diffuse across the membrane but retaining large molecules.

67
Q

Hemodialysis

A

-kidney’s main function is to remove toxic waste products
-if not functioning, perform hemodialysis

-patient’s blood circulates through a long tube of cellophane membrane suspended in ISOTONIC SOLUTION and then returns to patient’s vein
-cellophane membrane retains large molecules (i.e. proteins) but allows toxic wastes to pass through

68
Q

Ionization

A

Separation of acids and bases into ions

Bettel Plus Chang Chemistry (19 decks)

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