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Chemistry > Ch 16: Solutions > Flashcards

Ch 16: Solutions Flashcards

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1
Q

The ____________ of the solvent and the solute determine whether a substance will dissolve.

A

compositions

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2
Q

What three things will determine how fast a substance will dissolve?

A
  1. Stirring (agitation)
  2. Temperature
  3. Particle size
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3
Q

To determine to the saturation of a solution, what do you do?

A

Add more solute.

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4
Q

Saturation–add more solute: dissolves.

A

Unsaturated

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5
Q

Saturation–add more solute: doesn’t dissolve.

A

Saturated

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6
Q

Saturation–add more solute: triggers a reaction.

A

Supersaturated

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7
Q

What has happened when equilibrium is reached and can’t hold anymore in amount of solvent at current temperature?

A

Saturated solution

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8
Q

Solubility is often expressed in _____ of solute per _____ of solvent.

A

grams

100g

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9
Q

What has happened when a solution can hold more solute at that temperature?

A

Unsaturated solution

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10
Q

What affects the solubility of solids, liquids, and gaseous solutes in a solvent?

A

Temperature

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11
Q

What two things affect the solubility of gaseous solutes?

A

Temperature and pressure

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12
Q

What has happened when there are more solute particles than the solvent can hold with stability; it is unstable?

A

Supersaturated solution

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13
Q

What does “like dissolves like” mean?

A

Polar dissolves polar and nonpolar dissolves nonpolar.

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14
Q

What is S1 / P1 = S2 / P2?

A

Henry’s law

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15
Q

What is Henry’s law?

A

S1 / P1 = S2 / P2

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16
Q

There is no universal ________ _______, like there is for polar solutions (water).

A

Nonpolar solvent

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17
Q

Concentration Affects Properties: the solution freezes at a _____ temperature than the _______.

A

lower

solvent

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18
Q

Concentration Affects Properties: lowers the ________ _____.

A

freezing point

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19
Q

Concentration Affects Properties: the ____ concentrated, the more the freezing point is ________.

A

more

reduced

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20
Q

What has happened when there is less solvent than concentrated (more solvent)?

A

Dilute

21
Q

What have relatively large amounts of acids?

A

Concentrated solutions

22
Q

What have relative amounts of solvent and solute?

A

Concentrated solutions

23
Q

How is molarity related to concentration?

A

The higher the molarity, the more concentration.

24
Q

How do you calculate the molarity of a solution?

A

Moles of solute / liters of solution

25
Q

What does moles of solute / liters of solution equal?

A

Molarity (M)

26
Q

Diluting a solution _______ the number of moles of solute per ____ ______, but the total number of moles of solute in solution ____ ___ ______.

A

reduces
unit volume
does not change

27
Q

What is M1 X V1 = M2 X V2?

A

Moles of solute

28
Q

In what two ways can the concentration of a solution in percent be expressed?

A
  1. As the ratio of the volume of the solute to the volume of the solution.
  2. As the ratio of the mass of the solute to the mass of the solution.
29
Q

What properties of a solvent change when mixed with a solute?

A

Physical

30
Q

Physical property changes depend only on what?

A

The concentration of the solute, not the type of solute.

31
Q

What interferes with vaporization and crystallization?

A

Intermolecular attractions between solute and solvent particles.

32
Q

What are three important colligative properties of solutions?

A
  1. Vapor-pressure lowering
  2. Boiling-point elevation
  3. Freezing-point depression
33
Q

Solution stays liquid over a wider temperature range when ______ is added.

A

Solute

34
Q

When solute is added, the solution freezes at a _____ temperature.

A

lower

35
Q

When solute is added, the solution boils at a ______ temperature.

A

higher

36
Q

The decrease in a solution’s vapor pressure is ____________ to the number of particles the ______ makes in a solution.

A

proportional

solute

37
Q

The magnitude of the freezing-point depression is ____________ to the number of solute particles dissolved in the solvent and does not depend upon their ________.

A

proportional

identity

38
Q

The magnitude of the boiling-point elevation is proportional to the number of ______ particles dissolved in the _______.

A

solute

solvent

39
Q

The ____ ________ and ____ _________ are two additional ways is which chemists express the concentration of a solution.

A

unit molality

mole fractions

40
Q

What is a ratio of solute to solvent?

A

Molality

41
Q

Solute to solvent is more precise than ________; used to calculate __ elevation and __ depression.

A

molarity
bp
fp

42
Q

What is moles of solute / kilogram of solvent?

A

Molality

43
Q

What is the formula for molality?

A

moles of solute / kilogram of solvent

44
Q

What is XA =nA / nA + nB XB = nB / nA + nB?

A

Mole fraction

45
Q

The magnitudes of the freezing-point depression and the boiling-point elevation are directly proportional to the _____ concentration, when the solute is _________, not _____.

A

molal
molecular
ionic

46
Q

What is Kf for the freezing-depression of water?

A

1.86°C

47
Q

What is the Kb for the boiling-elevation of water?

A

0.52°C

48
Q

What is the formula for freezing-point depression?

A

∆Tf = Kf X m

49
Q

What is the formula for boiling-point elevation?

A

∆Tb = Kb X m

Chemistry (19 decks)

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