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General Chemistry 1 > Chapter 12 > Flashcards

Chapter 12 Flashcards

1
Q

what does solubility mean?

A

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

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2
Q

what does entropy mean?

A

a measure of energy randomization or energy dispersal

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3
Q

what does miscible mean?

A

the ability of two or more substances to be soluble in each other in all proportions

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4
Q

what are solvent-solute interactions?

A

the interactions between a solvent particle and a solute particle

  1. solvent-solute interaction > solute-solute solvent-solvent interaction SOLUTION FORMS
  2. solvent-solute interaction = solute-solute, solvent-solvent interaction SOLUTION FORMS
  3. solvent-solute interaction
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5
Q

what are solvent-solvent interactions?

A

the interactions between a solvent particle and another solvent particle

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6
Q

what are solute-solute interactions?

A

the interactions between a solute particle and another solute particle

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7
Q

what is a dynamic equilibrium?

A

the point at which the rate of reverse reaction is equal to the rate of the forward reaction

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8
Q

what is a saturated solution?

A

a solution in which the dissolved solute is in dynamic equilibrium with any undissolved solute; any added solute will not dissolve

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9
Q

what is an unsaturated solution?

A

a solution containing less than the equilibrium amount of solute; any added solute will dissolve until equilibrium is reached

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10
Q

what is a super saturated solution?

A

an unstable solution in which more than the equilibrium amount of solute is dissolved

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11
Q

what is recrystallization?

A

a technique used to purify solids in which the solid is put into hot solvent until the solution is saturated; when the solution cools, the purified solute comes out of the solution

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12
Q

what is Henry’s Law?

A

an equation that expresses the relationship between pressure and the solubility of a gas

Sgas = kH*Pgas
Sgas = solubility of gas in mol/L
kH = the constant of proportionality 
Pgas = the partial pressure of the gas
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13
Q

what is molarity (M)?

A

the amount of solute in moles divided by the volume of the solution in litres

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

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14
Q

what is molality (m)?

A

the amount of solute in moles divided by the mass of the solvent in kilograms

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

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15
Q

what is parts-by-mass?

A

the ratio of the mass of the solute to the mass of the solution, all multiplied by a multiplication factor

(mass solute / mass of solution)*multiplication factor

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16
Q

what is parts-per-million?

A

parts-by-mass multiplied by a multiplication factor of 10^6

17
Q

what is parts-per-billion?

A

parts-by-mass multiplied by a multiplication factor of 10^9

18
Q

what is parts-by-volume?

A

the ratio of the volume of the solute to the volume of the solution, all multiplied by a multiplication factor

19
Q

what is a mole fraction?

A

the amount of of solute in moles divided by the total amount of solute and solvent in moles

Xsolute = amount solute (mol) / total amount of solute and solvent (mol)

20
Q

what is mole percent?

A

it is simply mole fraction multiplied by 100%

21
Q

what is colligative property?

A

a property that depends on the amount of solute but not on the type

22
Q

what is Raoult’s Law?

A

The larger the solvent the larger the vapour pressure of the solution

An equation used to determine the vapour pressure of a solution

Psolution = Xsolvent*Psolvent
Psolution = vapour pressure of the solution
Xsolvent = mole fraction of solvent
Psolvent = the vapour pressure of the pure solvent
23
Q

define vapour pressure lowering?

A

the difference in vapour pressure between a pure solvent and a solution of the solvent

ΔP = Psolvent - Psolution
ΔP = Xsolute*Psolvent
24
Q

what is an ideal solution?

A

a solution that follows Raoult’s Law at all concentrations for both solute and solvent

25
Q

what is freezing point depression?

A

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

ΔTf = m*Kf
ΔTf = the change in temperature or the freezing point
m = the molality of the solution (mol/kg)
Kf = is the freezing point depression constant for the solvent
26
Q

what is boiling point elevation?

A

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

ΔTb = m*Kb
ΔTb = the change in temperature of the boiling point
m = the molality of the solution (mol/kg)
Kb = the boiling point elevation constant for the solvent
27
Q

what is the freezing point depression constant for water?

A

Kf = 1.86 Celsius/molality

28
Q

what is the boiling point elevation constant for water?

A

Kb = 0.512 Celsius/molality

29
Q

what is osmotic pressure?

A

The pressure required to stop osmotic flow

Π =MRT
M = molarity of the solution
T = is the temperature in kelvin K)
R = the ideal constant 0.08314barL/molK

30
Q

what is osmosis?

A

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

31
Q

what is the van’t Hoff factor (i)?

A

the ratio of particles in a solution to moles of formula units dissolved

i = moles of particles in solution / moles of formula units dissolved

32
Q

van’t Hoff’s corrections are applied to?

A

applied to the to freezing point depression, boiling point elevation and osmotic pressure determinations of IONIC solutions
ΔTf =imKf
ΔTb=imKb
Π =iMRT

33
Q

what is a colloid (colloidal dispersion)?

A

a mixture in which a dispersed substance is finely divided but not truly dissolved in a dispersing medium

34
Q

what is the Tyndall effect?

A

the scattering of light by a colloidal dispersion

General Chemistry 1 (11 decks)

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