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Chemistry 2 > Chapter 13 Solutions > Flashcards

Chapter 13 Solutions Flashcards

1
Q

Define Solution

A

A homogeneous mixture of 2 or more substances

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2
Q

Define Solvent

A

The MAJOR component in a solution

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3
Q

Define Solute

A

The MINOR component in a solution

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4
Q

T/F In a solution, the molecules that are more present in the solution is the solvent

A

True

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5
Q

Define Solution Equilibrium

A

The dissolution of a solute in a solvent is an equilibrium process

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6
Q

Define Saturated Solutions

A

Dissolved solute is in dynamic equilibrium with the excess undissolved solute

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7
Q

T/F In saturated solutions, additional solutes will continue to dissolve

A

False ; will not

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8
Q

Where on a graph are saturated solutions located?

A

On the line

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9
Q

Define Unsaturated Solutions

A

Solution containing less than the equilibrium amount of solute

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10
Q

Where on a graph are unsaturated solutions located?

A

Below the curve

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11
Q

Define Supersaturated Solutions

A

Solution containing more than the equilibrium amount of solute

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12
Q

T/F Supersaturated solutions are unstable

A

True

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13
Q

Where on a graph are supersaturated solutions located?

A

Above the curve

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14
Q

T/F The solubility of most solids in water increases with increasing temperature

A

True

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15
Q

T/F The solubility of gas in water increases with increasing temperature

A

False ; decreases

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16
Q

The solubility of a gas depends on _____________

A

Pressure

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17
Q

T/F The larger the partial pressure of a gas in contact with a liquid, the more stable the gas is in the liquid

A

True

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18
Q

Define Henry’s Law

A

States that the solubility of gas (S gas) is directly proportional to its partial pressure (P gas)

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19
Q

Define Solubility

A

The amount of the substance that will dissolve in a given amount of solvent

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20
Q

T/F For solids when temperature increases, solubility increases

21
Q

T/F For gas when temperature increases solubility increases

A

False ; decreases

22
Q

T/F For gas when pressure increases solubility increases

23
Q

Define Concentration

A

The amount of solute in a given amount of solution/solvent

24
Q

Is Molarity or Molality dependent on temperature?

25
Q

T/F Molarity depends on volume

26
Q

What is the equation for Molarity?

A

Molarity (M) = amount of solute (mol) / volume solution (L)

27
Q

What is the equation for Molality?

A

Molality (m) = amount of solute (mol) / mass solvent (kg)

28
Q

What is the equation for Mole Fraction?

A

Mole Fraction (x solute) = amount of solute (mol) / solute + solvent (mol)

29
Q

What is the equation for Percent by Mass?

A

Percent by Mass = mass of solute / mass of solution X 100%

30
Q

Define Colligative Properties

A

Properties that depend on the amounts of particles dissolved in solution, not on the type of particle

31
Q

The number of ________ ____________ determines its vapor pressure

A

Gaseous particles

32
Q

More solute results in increased or decreased vapor pressure

33
Q

What is the equation for Raoult’s Law?

A

Psolution = x solvent X P solvent

34
Q

How do you find x solvent in Raoult’s Law?

A

Use mol fraction

35
Q

What is the equation for Boiling Point Elevation?

A

DeltaTb = m X Kb

36
Q

Define Boiling Point Elevation

A

The effect of a solute that causes a solution to have a higher boiling point than the pure solvent alone

37
Q

Define Freezing Point Depression

A

The effect of a solute that causes a solution to have a lower freezing point than the pure solvent alone

38
Q

What is the equation for Freezing Point Depression?

A

DeltaTf = m X Kf

39
Q

Define Osmosis

A

The flow of solvent from a solution of lower solute concentration to one of higher solute concentration

40
Q

Define Osmotic Pressure

A

The pressure required to prevent the net movement of solvent across a semipermeable membrane

41
Q

What is the equation for Osmotic Pressure?

42
Q

Define Electrolyte

A

Substance that dissociates into ions to conduct electricity when dissolved in water

43
Q

Define Non-Electrolyte

A

A compound that DOES NOT dissociated into ions when dissolved in water

44
Q

What i value will non-electrolytes always have?

45
Q

Define Van’t Hoff Factor

A

(i) the ratio of moles of particles in solution to moles of formula units dissolved

46
Q

Does boiling point decrease or increases when more solute is added?

47
Q

T/F The presence of a solute could hinder a particle from entering another phase

48
Q

What are the 4 colligative properties?

A
  • Vapor pressure
  • Freezing point depression
  • Boiling point elevation
  • Osmotic pressure
49
Q

What is the equation for Henry’s Law?

A

S(gas) = Kh X P(gas)

Chemistry 2 (10 decks)

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