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Chem Exam 1 > Ch. 12 Solutions > Flashcards

Ch. 12 Solutions Flashcards

1
Q

solution

A

a homogenous mixture of 2 or more substances

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2
Q

solvent

A

majority component in solution; i.e. water

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3
Q

solute

A

minority component in solution; i.e. salt

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4
Q

solubility

A

the amount of the substance that will dissolve in a given amount of solvent; max concentration possible

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5
Q

entropy

A

measure of energy randomizations or energy dispersal in a system

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6
Q

greater dispersal of solution means

A

greater entropy

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7
Q

miscible definition

A

when two substances are soluble in each other in all proportions

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8
Q

solvent-solute > solvent-solvent and solute-solute

A

solution forms

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9
Q

solvent-solute = solvent-solvent and solute-solute

A

solution forms

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10
Q

solvent-solute

A

solution may or may not form, depending on relative disparity

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11
Q

common polar solvents

A

water, acetone, methanol, ethanol

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12
Q

common non polar solvents

A

hexane, diethyl ether, toluene, carbon tetrachloride

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13
Q

mass fraction equation

X = ?

A

mass part divided by mass whole (grams)

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14
Q

unsaturated

A

less amount of solute is present than solubility would indicate; more will still be able to dissolve

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15
Q

saturated

A

max amount of solute is dissolved in solvent; no more will dissolve

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16
Q

dynamic equilibrium definition

A

point at which the rate of the reverse reaction equals the rate of the forward reaction;
rate of dissolution = rate of precipitation

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17
Q

supersaturated

A

more solute is present than the max amount allowed by the solubility

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18
Q

vapor pressure

A

solubility of a solvent’s gas in C=air expressed as a partial pressure

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19
Q

Dalton’s Law of Pressure

A

Total pressure = sum of partial pressures

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20
Q

covalent bonds

A

sharing of electrons

21
Q

dispersion force (London force)

A

an intermolecular force that is always present because it is an interaction of electrons

22
Q

polar =

A

asymmetry

23
Q

non polar =

A

symmetry

24
Q

2nd Law of Thermodynamics

A

a spontaneous process has a net increase in entropy

25
Q

3rd Law of Thermodynamics

A

a perfect crystal at O Kelvin has zero entropy

26
Q

Molarity units

A

Mol/L

27
Q

Molality units

A

mol solute/kg solvent

28
Q

hydrogen bonding definition

A

bonding of H atom to O, N, or F

29
Q

3 characteristics that favor solubility

A
  1. presence of ions
  2. presence of dipole moment
  3. presence of dispersion forces
30
Q

Henry’s Law equation (in terms of concentration)

A

C=kP

C=concentration (M)
k=Henry’s law constant (mol/L*atm)
P=pressure (atm)

31
Q

Henry’s Law equation (in terms of solubility)

A

s=kP

s=solubility (M)
k= Henry’s law constant
P=pressure (atm)

32
Q

mole fraction

A

moles solute / moles solution

33
Q

Raoult’s Law for nonvolatile solutions

A

Pa=Xa * P∘a

Pa=vapor pressure of soln
Xa=mole fraction of solvent
P∘a=vapor pressure of pure solvent

34
Q

Deviations from Raoult’s law for volatile solutions

A

Psoln=Psolv × Xsolv where Psolv is equal to vapor pressure of the pure solvent

35
Q

According to Raoult’s law, if molecules interact less favorably, they will deviate…

A

positively

36
Q

According to Raoult’s law, if molecules interact more favorable, they will deviate…

A

negatively

37
Q

Freezing Point Depression (ΔTf) equation

A

ΔTf=Kf⋅m

Kf=constant
m=molality (mol solute/kg solvent)

38
Q

osmotic pressure equation

A

Π=MRT

M=molarity
R= 0.08206
T=temperature

39
Q

Total pressure of a solution containing 2 volatile components according to Raoult’s Law

A

Ptotal = Pa × Xa + Pb × Xb

40
Q

Boiling Point Elevation (ΔTb) equation

A

ΔTb=Kb⋅m

41
Q

Equation for ΔTf or ΔTb for an electrolyte that dissociates

A

ΔT=i⋅K⋅m

42
Q

Equation for osmotic pressure (Π) for an electrolyte that dissociates

A

Π=iMRT

43
Q

type(s) of forces typically present in ionic or polar compounds

A

ion-dipole and dispersion

44
Q

type(s) of forces typically present is nonpolar compounds

A

dispersion forces

45
Q

heat of hydration equation

A

D Hsoln = D Hsolute + D Hhydration

where D Hsolute = -D Hlattice

46
Q

Vapor Pressure definition

A

solubility of a solvent’s gas in air expressed as a partial pressure

47
Q

colligative properties definition

A

property that depends on the number of solute particles in a solution, not on the identity of those particles

48
Q

Van’t Hoff Factor, i=

A

moles solute particles / moles solute dissolved

49
Q

osmosis definition

A

the flow of solvent through a semi-permeable membrane from a region of low solute concentration to a region of high solute concentration

Chem Exam 1 (2 decks)

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