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Chem 262 > Ch. 13 The Properties of Mixtures > Flashcards

Ch. 13 The Properties of Mixtures Flashcards

1
Q

What is a solution

A

a homogenous mixture of two or more substances in a single phase

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2
Q

What is a solvent

A

the component present in the largest amount

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3
Q

What is a solute

A

the component in a mixture that is the lesser amount

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4
Q

What is a colligative property

A

properties of solution that depend only on the number of solute particles per solvent molecule and not on the identity of the solute

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5
Q

What are the two units of concentration

A

molarity and molality

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6
Q

What is molality

A

mole of solute over mass of solvent
does not change with temp
masses are additive

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7
Q

What is the formula for mass percent

A

mass of solute over mass of solute + mass of solvent x 100

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8
Q

What is the formula for parts per million for mass

A

mass of solute over mass of solution x 10^6

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9
Q

What is the formula for parts per billion for mass

A

mass of solute over mass of solution x 10^9

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10
Q

What is the formula for volume percent

A

volume of solute over volume of solution x 100

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11
Q

What is the formula for parts per million for volume

A

volume of solute over volume of solution x 10^6

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12
Q

What is the formula for parts per billion for volume

A

volume of solute over volume of solution x 10^9

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13
Q

What is the solubility of a solution

A

the maximum amount that dissolves in a fixed quantity of solvent at a given temp, where an excess of solute is present

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14
Q

What kind of polarity does alcohol have

A

dual polarity

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15
Q

Which parts of the alcohol are polar and which parts are non polar

A

-OH group is polar and the hydrocarbon is non polar

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16
Q

What are the three steps in the heat of solution (enthalpy of solution)

A
  1. separation of solute particles, 2. separation of solvent particles, 3. mixing of solute and solvent particles
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17
Q

What does an ion depend on during heat of hydration

A

depends on the charge density, the ratio of charge to volume

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18
Q

What happens to the radius as the charge gets stronger

A

the radius gets smaller

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19
Q

How are freedom of motion and kinetic energy related

A

the more freedom of motion, the more ways kinetic energy can be disperse change in entropy

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20
Q

Which has a higher entropy, a solution or pure solute/solvent

A

solution

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21
Q

What is a saturated solution

A

contains the maximum amount of dissolved solute at a given temp in the presence of undissolved solute

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22
Q

How are undissolved solute and dissolved solute related

A

they are in equilibrium with each other

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23
Q

What is an unsaturated solution

A

contains less than the equilibrium concentration of dissolved solute. if more solute is added, it will dissolve

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24
Q

What is a supersaturated solution

A

contains more than the equilibrium concentration of solute

25
Q

What two factors affect solubility

A

temp and pressure

26
Q

How does temp affect solubility

A

most solids are more soluble at a higher temp, gasses become less soluble as temp increases

27
Q

How does pressure affect solubility

A

gases become more soluble at a higher pressure

28
Q

How is the solubility of gas and the partial pressure of a gas related

A

the solubility of a gas is directly proportional to the partial pressure of the gas above the solution

29
Q

What is the formula for Henry’s Law and what are the units

A

Sgas= Kh X Pgas

the units for Kh are M/atm

30
Q

What are colligative properties

A

they are properties that depend on the number of solute particles, not their chemical identity
ex. vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure

31
Q

What happens to electrolytes in water

A

they separate into ions when dissolved in water

32
Q

What is the difference between strong and weak electrolytes in water

A

strong- dissociate completely

weak- dissociate very little

33
Q

What does a non electrolyte do in water

A

does not dissociate to form ions

34
Q

What type of electrolyte is NaCl

A

strong

35
Q

What type of electrolyte is Sucrose (C12H22O11)

A

non electrolyte

36
Q

What type of electrolyte is NaOH

A

strong

37
Q

What type of electrolyte is Acetic Acid (CH3COOH)

A

Weak

38
Q

What type of electrolyte is HNO3

A

strong

39
Q

What type of electrolyte is Na2CO3

A

strong

40
Q

What type of electrolyte is NH3

A

weak

41
Q

What type of electrolyte is Ethylene Glycol (C2H6O2)

A

non electrolyte

42
Q

Which has a lower vapor pressure, a nonvolatile non electrolyte or a pure solvent

A

nonvolatile non electrolyte

43
Q

How are vapor pressure and mole fraction of a solute related

A

vapor pressure lowering is proportional to the mole fraction of the solute present

44
Q

Which has a higher boiling point, a solution or a pure solvent

A

solution

45
Q

How are boiling point elevation and molality related

A

boiling point elevation is proportional to the molality of the solution

46
Q

What is osmosis

A

the movement of solvent particles from a region of higher to a region of lower concentration through a semipermeable membrane

47
Q

How does the solvent flow in osmosis

A

the solvent will always flow from a more dilute solution to a more concentrated one

48
Q

What is osmotic pressure

A

the pressure that must be applied to prevent the net flow of solvent

49
Q

What must a solution contain to be a volatile non electrolyte

A

the vapor of the solution contains both solute and solvent

50
Q

The presence of each volatile component does what to the vapor pressure of the other side

A

lowers

51
Q

The vapor will have a ______ mole fraction to the more volatile component

A

higher

52
Q

The vapor has a _______ composition of the solution

A

different

53
Q

The formula of the compound indicates what of the particles in the solution

A

the expected number of particles

54
Q

The van’t Hoff factor takes in to account what

A

the dissociation of a strong electrolyte to predict the effect on the solution

55
Q

What is the formula for i

A

i equals the measured value for electrolyte solution over expected value of non electrolyte solution

56
Q

What is an ionic atmosphere

A

ions in solution may remain clustered near ions of opposite charge

57
Q

What is a colloid

A

a dispersion of particles of one substance throughout another substance or solution

58
Q

What is the Tyndall effect

A

colloids appear to be homogenous but can be distinguished from solutions by its ability to scatter light

Chem 262 (3 decks)

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