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General Chemistry MCAT > Solutions > Flashcards

Solutions Flashcards

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1
Q

Solutions

A

Homogenous mixtures of two or more pure substances in the same phase

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2
Q

Solute

A

A substance that is dissolved in a solution

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3
Q

Solvent

A

A liquid substance capable of dissolving other substances

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4
Q

solvation

A

electrostatic interaction between solute and solvent molecules
aka dissolution, hydration
- breaking of IM interactions, forming of new ones

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5
Q

When new interactions (attractions) are stronger than the original ones, solvation is _____ and the process is favored at ____ temperatures

A

exothermic
low

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6
Q

When new interactions are WEAKER than the original ones, solvation is _____________; and the process is favored at _______ temperatures.

A

endothermic
high

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7
Q

ideal solution

A

a solution whose vapor pressure is directly proportional to the mole fraction of solvent present

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8
Q

at constant temp and pressure, entropy always ____ in solution

A

increases

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9
Q

spontaneous processes ______ free energy

A

decrease

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10
Q

overall dissolution of salt is

A

endothermic
favored at high temps

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11
Q

solubility

A

the maximum amount of solute that can dissolve in a given amount of solvent at a given temperature and pressure

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12
Q

saturated solution

A

a mixture that contains as much dissolved solute as is possible at a given temperature

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13
Q

if more solute is added to a saturated solution,

A

it will fall to the bottom and not dissolve
precipitate

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14
Q

when the change in Gibbs free energy for the dissolution run is negative (-)…

A

process is spontaneous
solute is soluble

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15
Q

sparingly soluble salts

A

Solutes that dissolve minimally in the solvent, molar solubility under 0.1 M.

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16
Q

aqueous solution

A

a solution in which water is the solvent

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17
Q

solubility rules

A
  1. all salts w ammonium and group I cations are soluble
  2. all salts w nitrate and acetate anions are water-soluble
  3. halides (except w Ag, Pb, Hg)
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18
Q

complex ion

A

charged species consisting of metal ion surrounded by ligands (electron pair donor)

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19
Q

complexes are held together w

A

coordinate covalent bonds where an electron pair donor and electron pair acceptor form a stable lewis acid base adduct

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20
Q

chelation

A

The process of binding metal ions to the same ligand at multiple points.

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21
Q

how to increase solubility of solids and gases

A

solids: inc temp
gas: dec temp, inc pressure of gas

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22
Q

percent composition by mass

A

mass of solute/mass of solution x 100%

23
Q

mole fraction of compound

A
24
Q

molarity

A

the number of moles of solute per liter of solution

25
Q

molality

A

the concentration of a solution expressed in moles of solute per kilogram of solvent

26
Q

normality

A

the number of equivalents of a substance dissolved in a liter of solution

27
Q

dilution equation

A

M1V1=M2V2

28
Q

saturation point

A

The equilibrium position for a solution where the solute concentration is at its maximum value for the given temperature and pressure

29
Q

when solution is diluted

A

dissolution favored

30
Q

as solution becomes more concentrated

A

rate of dissolution lessens and precipitation rate increases

31
Q

t/f: at equilibrium, neither dissolution or precipitation is favored.

A

true

32
Q

solubility product constant

A

an equilibrium constant applied to the solubility of electrolytes; it is equal to the product of the concentrations of the ions each raised to a power equal to the coefficient of the ion in the dissociation equation

33
Q

t/f: Ksp is temperature dependent

A

true

34
Q

Ksp increases what?

A

increases temperature for non-gas

35
Q

___ pressures favor dissolution

A

higher (gas)

36
Q

ion product

A

The product of the molar concentrations of dissociated ions in solution at a given point in a reaction, where each ion is raised to the power of its stoichiometric coefficient.

37
Q

IP < Ksp

A
  • solution is unsaturated
  • if more solute is added, it will dissolve
38
Q

IP = Ksp

A

saturated, solution is at equilibrium

39
Q

IP> Ksp

A

the solution is supersaturated, and a precipitate will form

40
Q

molar solubility

A

molarity of a solute in a saturated solution

41
Q

given molar solubility, how to find Ksp?

A

Ksp = [x][3x]^3 (for XF3)
- plug in molar solubility for X
- solve for Ksp

42
Q

formation of complex ions ____ solubility of a salt

A

increases

43
Q

complex ions tend to have ___ Ksp

A

larger

44
Q

stability constant

A

The equilibrium constant for an equilibrium existing between a transition metal ion surrounded by water ligands and the complex formed when the same ion has undergone a ligand substitution

45
Q

common ion effect

A

a decrease in the solubility of an ionic compound caused by the addition of a common ion

46
Q

raoult’s law

A

the vapor pressure of a solution is directly proportional to the mole fraction of solvent present
- presence of solute molecules blocks evaporation of solvent molecules but NOT condensation

47
Q

lower vapor pressure means ____ BP

A

higher

48
Q

boiling point elevation

A

the temperature difference between a solution’s boiling point and a pure solvent’s boiling point

49
Q

freezing point depression

A

the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent

50
Q

osmotic pressure

A

pressure that must be applied to prevent osmotic movement across a selectively permeable membrane

51
Q

water always flows to the

A

hypertonic area

52
Q

How are molality and molarity related for water? How are they related for other solvents?

A

water: the same bc 1 L = 1 kg water
other solvents: diff bc density is different

53
Q

formation of complex ions ______ solubility of insoluble ions

A

increases

General Chemistry MCAT (12 decks)

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