Solutions Flashcards

1
Q

define a solution

A

one or more substances (solutes) mixed at the molecular level (dissolved) in a medium (solvent, usually liquid)

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2
Q

two properties of a solution

A
  • uniform mixing
  • constant composition throughout
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3
Q

percent A by mass =

A

mass of solute A/mass of solution x 100

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4
Q

parts per million (ppm) A =

A

mass of solute A/mass of solution x 10^6

or

moles of solute A/moles of solution x 10^6

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5
Q

mole fraction (Xa) =

A

moles of solute A/moles of solution

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6
Q

solutions that obey Raoul’s law are called

A

ideal solutions

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7
Q

Colligative properties

A

solution properties that depend on the concentration of a solute, not its identity

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8
Q

freezing point depression

A

solutes lower freezing point of the solvent

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9
Q

boiling point elevation

A

solutes raise boiling point of the solvent

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10
Q

vapour pressure lowering

A

solutes decrease vapour pressure of the solvent

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11
Q

osmotic pressure

A

pressure that must be applied to a solution to prevent osmosis from a sample of a pure solvent

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12
Q

how do non-volatile solutes act on the vapour pressure of the solvent?

A

they decrease it

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13
Q

Raoul’s law for non-volatile solute:

A

P = XP^0
P - vapour pressure of solvent in solution
X = mole fraction of the solvent
P^0 = vapour pressure of pure solvent

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14
Q

what needs to occur for substances to form a solution?

A

the solute-solvent interaction has to overcome both solute-solute interactions and solvent-solvent interactions

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15
Q

volatile

A

something that can evaporate

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16
Q

what is the difference between the effect of a volatile and non-volatile solute?

A

with a volatile solute, both the solvent and solute contribute to vapour pressure

17
Q

P total =

A

P sub 1 + P sub 2

18
Q

osmosis

A

net flow of solvent through a semi permeable membrane from a dilute solution to more concentrated solution

19
Q

semi-permeable membrane only allows

A

solvent to go through, not solvent

20
Q

osmotic pressure

A

pressure that must be applied to the solution to prevent osmosis from a sample of pure solvent

21
Q

how do you signify osmotic pressure?

A

pi

22
Q

equation for osmotic pressure

A

pi = MRT
pi - osmotic pressure
M - total molarity of all solutes
R - gas constant
T - temperature (K)

23
Q

how do you know which value of R to use?

A

whichever one the units cancel out for

24
Q

dissociation of 0.1M NaCl
dissociation of 0.1M CaCl2
dissociation of 0.1M glucose
state the osmotic pressure for all

A

Na+ and Cl-
Ca2+ and 2Cl-
stays same
0.200M, 0.100, 0.300M

25
Q

state van’t Hoff’s factor

A

i = moles of particles in solution/moles of solute dissolved

26
Q

substances with —– ——– —– form solutions

A

similar intermolecular forces

27
Q

formula for solubility

A

solubility = k P

P - partial pressure of gas over the solution
k - Henry’s Law constant - depends on gas and solvent (usually H2O)