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MCAT Chemistry > Solutions > Flashcards

Solutions Flashcards

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1
Q

solution

A

homogenous mixture of two or more compounds in a single phase

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2
Q

solvent vs. solute

A

solvent = compound of which there is more
solute = less of
(both can be referred to as solvents)

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3
Q

general rule for dissolution

A

like dissolved like

-refers to polarity of solute and solvent

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4
Q

London dispersion forces

A
  • highly polar molecules held together by strong molecular bonds formed by attraction between their partially charged ends
  • nonpolar molecule held together by weak intermolecular bonds from instantaneous dipole moments
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5
Q

ionic compounds dissolved by ___

A

polar substances

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6
Q

solvation

A

ionic compounds break apart into cations and anions and are surrounded by the oppositely charged ends of the polar solvent

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7
Q

____ is good solvent for ionic substances

A

water

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8
Q

hydration

A

using water as a solvent…when several water molecules attach to one side of ionic compound, they can overcome ionic bonds and break apart compound, molecules surround ion

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9
Q

aqueous phase

A

something that is hydrated

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10
Q

electrolyte

A

compound that forms ions in aqueous solution, create solutions that conduct electricity

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11
Q

NO2(-)

A

nitrite

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12
Q

NO3(-)

A

nitrate

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13
Q

SO3(2-)

A

sulfite

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14
Q

SO4(2-)

A

sulfate

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15
Q

ClO(-)

A

hypochlorite

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16
Q

ClO2(-)

A

chlorite

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17
Q

ClO3(-)

A

chlorate

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18
Q

ClO4(-)

A

perchlorate

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19
Q

CO3(2-)

A

carbonate

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20
Q

HCO3(-)

A

bicarbonate

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21
Q

PO4(3-)

A

phosphate

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22
Q

Molarity

A

moles of the compound divided by the volume of the solution (mol/L)

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23
Q

molality

A

moles of solute divided by kilograms of solvent (mol/kg).

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24
Q

mole fraction

A

moles of a compound divided by total moles of all species in solution

25
Q

mass percentage

A

100 times the ratio of the mass of the solute to the total mass of the solution

26
Q

parts per million (ppm)

A

10^6 times the ratio of the mass of the solute to the total mass of the solution

27
Q

solution formation and heat of solution

A

step 1: breaking bonds of solute, endothermic, +delta H1
step 2: braking bonds of solvent, endothermic, +delta H2
step 3: formation of bonds between solvent and solute, exothermic, -delta H3
heat of solution = delta H1 + delta H2 + delta H3 ; overall change in energy of the reaction is equal to the change in enthalpy

28
Q

negative heat of solution

A

stronger intermolecular bonds, lower vapor pressure

29
Q

positive heat of solution

A

weaker intermolecular bonds, raise vapor pressure

30
Q

formation of solution usually involves ___ in entropy

A

increase in entropy….combined mixture is more disordered than the separated pure substances

31
Q

when gas dissolves in liquid or solid, entropy change is…

A

negative

32
Q

one condensed phase (liquid or solid) dissolving into another, ___ in entropy

A

increase

33
Q

vapor pressure

A

partial pressure of the compound necessary to create equilibrium between the liquid and gas phases of a compound

34
Q

vapor pressure is function of ___

A

temperature, increases with temp

35
Q

evaporates when…

A

vapor pressure of liquid phase is greater than partial pressure of gaseous phase

36
Q

condense when…

A

vapor pressure of liquid phase is smaller than partial pressure of gaseous phase

37
Q

boiling occurs when…

A

vapor pressure of liquid equals atmospheric pressure

38
Q

melting occurs when….

A

vapor pressure of solid phase equals vapor pressure of liquid phase
above melting point - liquid vapor pressure is greater than solid
below melting point - liquid vapor pressure is less than solid

39
Q

nonvolatile solute

A

solute with no vapor pressure

40
Q

Raoult’s law (general)

A

vapor pressure of solution is proportional to the mole fraction of the liquid and vapor pressure of the pure liquid
P_v = X_a * P_a
for when nonvolatile solute added to liquid
P_v = X_a * P_a + X_b * P_b

41
Q

volatile solute

A

solute with vapor pressure

42
Q

Raoult’s law for nonvolatile solutes

A

if 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of the pure solvent

43
Q

Raoult’s law for volatile solutes

A

if 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of the pure solvent plus 3% of the vapor pressure of the pure solute

44
Q

vapor pressure of ideal solution is

A

sum of the individual partial vapor pressures

45
Q

precipitation

A

reverse reaction of dissolving salt, slower rate than dissolution initially then equilibrate

46
Q

saturated

A

rate of dissolution and precipitation are equal, concentration of dissolved salt has reached a maximum

47
Q

solubility product K_sp

A

set equal to products over reactants raised to the power of their coefficients in the balanced equation, leave out pure solids and liquids
changes with temperature

48
Q

crystallization is (exo/endothermic)

A

exothermic

49
Q

solubility depends on

A

temperature and ions in solution

50
Q

common ion added to a saturated solution…

A

will shift the equilibrium increasing precipitate, does not affect K_sp

51
Q

common ion added to solution that is not saturated

A

will not shift the equilibrium (no equilibrium to shift)

52
Q

spectator ions

A

no effect on equilibrium

53
Q

pressure on a gas ___ solubility

A

increases

54
Q

solubility of a gas is proportional to….

A

its vapor partial pressure

55
Q

partial vapor pressure of a solution is always proportional to its ___

A

mole fraction

56
Q

if component predominates as solvent,

A

Raoult’s law says the partial vapor pressure is proportional to the pure vapor pressure

57
Q

if component represents tiny amount of solution,

A

vapor partial pressure is proportional to henry’s law constant

58
Q

as temp increases, solubility of gas …

A

decreases

MCAT Chemistry (7 decks)

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