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Chemistry 1110 > Lecture 8 - Solutions > Flashcards

Lecture 8 - Solutions Flashcards

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1
Q

True/False: water has the ability to dissolve a wide variety of substances

A

True

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2
Q

aqueous solution = homogeneous or heterogeneous mixture

A

homogeneous

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3
Q 
7 types of solutions:
gas/gas
gas/liquid
liquid/liquid
liquid/solid
solid/liquid
solid/solid
gas/solid
A 
air (O, N, and other gases)
soda pop (CO2 in H2O)
vinegar (acetic acid in H2O)
dental fillings (Hg in Ag)
sea water (NaCl in H2O)
brass (Zn in Cu)
nitrogen in steel
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4
Q

the measure of how much solute will dissolve in a solvent

A

solubility

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5
Q

solutions that contain the max amount of solute for the given conditions - cannot dissolve additional state

A

saturated solutions

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6
Q

why does the temperature always need to be specified when describing a saturated solution

A

because the solubility depends on temperature and temperature must be specified because of the “temperature effect” on solubility

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7
Q

most solids become more soluble in aqueous solution with _____ temperature

A

increasing

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8
Q

gas solubility decreases with _____ temperature for aqueous solutions

A

increasing

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9
Q

solutions that contain less than the max amount of solute - can dissolve additional state

A

unsaturated solutions

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10
Q

if a substance does not dissolve in a solvent

A

insoluble

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11
Q

contain a small amount of solute relative to what could dissolve

A

dilute solutions

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12
Q

contain a large amount of solute relative to what could dissolve

A

concentrated solutions

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13
Q

all solutes that dissolve in water can be divided into two categories

A

electrolyte

nonelectrolyte

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14
Q

a substance that dissolves in water to give an electrically conducting solution

A

electrolyte

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15
Q

a substance that dissolves in water to give a solution that conducts electricity poorly

A

nonelectrolyte

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16
Q

when an ionic substance dissolves in water it _____ into its ions

A

dissociates

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17
Q

component present in the greatest amount

A

solvent

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18
Q

component present in the relatively smaller amount

A

solute

19
Q

substance that dissolve in each other in all proportions

A

miscible

20
Q

what are gases always miscible

A

because the intermolecular attractions in the gas phase are always weak

21
Q

when a dissolved solute forms a solid

A

crystallization

22
Q

when the rate of dissolution and crystallization are equal

A

equilibrium

23
Q

4 concepts for understanding equilibrium:

A

equilibrium is

  • time dependent
  • dynamic
  • reversible
  • temperature dependent
24
Q

3 factors affecting the rate of solution formation and establishment of equilibrium

A
  1. surface area
  2. agitation
  3. temperature
25
Q

increasing the pressure will _____ the solubility of a gas in a solvent

A

increase

26
Q

decreasing the pressure will _____ the solubility of a gas in a solvent

A

decrease

27
Q

the amount of solute dissolved in a given amount of solvent or solution

A

concentration

28
Q

concentration equation:

A

concentration = (amt. solute/amt. solution)

29
Q

% mass (solute) =

A

(mass solute/total mass solution) x 100

30
Q

the ratio of the volume of a solute to the volume of the solution, multiplied by 100

A

volume-volume percent

31
Q

% mass-volume =

A

(mass solute (g)/volume solution (mL)) x 100

32
Q

Dilution Equation

A

CsVs = CdVd

33
Q

properties that depend only on the number of solute particles in a solution and not on the nature of the solute particles

A

colligative properties

34
Q

4 colligative properties

A
  1. vapor pressure lowering
  2. boiling point elevation
  3. freezing point depression
  4. osmotic pressure
35
Q

the pressure required to stop osmosis

A

osmotic pressure

36
Q

one solution has a lower osmotic presure

A

hypotonic

37
Q

the solution with higher osmotic pressure

A

hypertonic

38
Q

a concentration unit used to compare the osmotic pressures of different solutions

A

osmolarity

39
Q

have similar properties to solutions but they are not true solutions

A

colloids

40
Q

are colloids heterogeneous or homogeneous

A

heterogeneous

41
Q

the scattering of light by colloidal-size particles

A

tyndall effect

42
Q

collectively, the particles suspended in a colloid

A

dispersed phase

43
Q

substance containing the colloid particles

A

dispersing medium

44
Q

caused by collisions between the suspended particles and the molecules of the dispersing medium

A

brownian movement

Chemistry 1110 (9 decks)

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