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MCAT general Chem > Solutions > Flashcards

Solutions Flashcards

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1
Q

Are all mixtures solutions?

A

No

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2
Q

Are all solutions mixtures?

A

Yes

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3
Q

When is solvation exothermic?

A

When the new interactions are stronger than the old ones

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4
Q

What kind of temperature favors solubility of gas in liquid?

A

Lower temp

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5
Q

When is solvation endothermic?

A

When new interactions are weaker than old

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6
Q

When is endothermic solvation favored?

A

At higher temperatures

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7
Q

Ideal solution

A

Enthalpy of the dissolution/solvation = 0

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8
Q

Spontaneous processes do what to Gibb’s free energy?

A

Reduce Gibb’s free energy

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9
Q

Nonspontaneous processes do what to Gibb’s free energy

A

Increase Gibb’s free energy

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10
Q

Breaking bonds is

A

Endothermic

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11
Q

Making bonds is

A

Exothermic

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12
Q

Solubility

A

Maximum amount of the substance that can be dissolved in a particular solvent at a given temperature

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13
Q

Above what solubility are solutes considered soluble?

A

Above 0.1 M

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14
Q

Solubility rules

A

NH4+ and Group 1 are water soluble
Nitrates and Acetates are soluble
Cl, Br, I excluding F are soluble except for Ag, Pb, Hg2
All sulfates are soluble except Ca, Sr, Ba, Pb
All metal oxides are insoluble except alkali, ammonium, CaO, SrO,BaO
All hydroxides are insoluble except for alkali metals, ammonium, Ca, Sr, Ba
Carbonates, phosphates, sulfides, sulfites are insoluble except alkali metals and ammonium

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15
Q

Complex ion/Coordinated compound

A

a molecule in which a cation is bonded to at least one electron donoor moleules called ligands

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16
Q

Coordinate covalent bonds

A

Hold complexes together where an electron donor pair (Lewis base) and acceptor (Lewis acid) form a Lewis acid-base adducts

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17
Q

Chelation

A

Central cation bonded to same ligand in multiple places in a complex

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18
Q

Concentration of solution after dilution

A

MV=MV

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19
Q

Normality

A

mols solute/kg solvent

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20
Q

Saturation point

A

Equilibrium in creating a solution where solute concentration is max for given temp and pressure

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21
Q

Change in free energy at equilibrium

A

0

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22
Q

Solubility product constant

A

Ksp

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23
Q

Ksp equation

A

Ksp=[A^n+]^m[B^m-]^n

24
Q

Would a Ksp have a denominator?

A

No

25
Q

What happens to the Ksp as temperature rises for gas solutes?

A

Decreases

26
Q

What happens to the Ksp as temperature rises for gas solutes?

A

Increases

27
Q

Ksp at higher pressures for gases

A

Larger

28
Q

Ksp at lower pressures for gases

A

Higher

29
Q

Ion product (IP)

A

Similar to Q

30
Q

Unsaturated

A

IP

31
Q

Supersaturated

A

IP>Ksp

32
Q

Ksp equations used for what kind of problems?

A

Sparingly/insoluble

33
Q

Sparingly soluble salt formula MX has what Ksp?

A

x^2

34
Q

Sparingly soluble salt formula MX^2 has what Ksp?

A

4x^3

35
Q

Sparingly soluble salt formula MX3

A

27x^4

36
Q

Relative Ksp of complex?

A

High

37
Q

Kf

A

Formation constant of complexes

If very high, the final concentration of the complex ion will be very near to the limiting reagent

38
Q

Common ion effects

A

Reduced solubility due to same ion already in solution

No effect on solubility product constant, only on molar solubility of salt

39
Q

Colligative properties

A

Dependent on the concentration of dissolved particles but not their chemical identity

40
Q

Colligative property examples

A

Vapor pressure depression
Boiling point elevation
Freezing point depression
Osmotic pressure

41
Q

Raoult’s law

A

Vapor pressure depression caused by solutes in solution

As solute is added to solvent, vapor pressure decreases proportionally

42
Q

Raoult’s law expression

A

PA=XAPA not

PA=vapor pressure when solutes are present
XA=mol fraction of solvent A
PA not=vapor pressure of solvent A in pure state

43
Q

Lowering of solution’s vapor pressure means

A

Higher boiling point

44
Q

Boiling point elevation

A

When a nonvolatile solute is dissolved in a solvent to create a solution, boiling point greater than pure solvent

45
Q

Boiling point depression

A

Temperature where vapor pressure of the liquid equals ambient pressure
More energy/higher temp needed to to get vapor pressure to reach ambient pressure

46
Q

Boiling point depression expression

A

Delta(T)=iKbm
i=van’t Hoff factor=number of particles in which a compound dissociates (NaCl=2)
Kb=proportionality constant of the solvent
m=molality

Temperature in Kelvin

47
Q

Density of water

A

1 g/mL

48
Q

Freezing point depression

A

More temperature must be removed to create lattice structure

49
Q

Freezing point depression equation

A

Delta T f=iKfm

i=van t’Hoff
Kf=proportionality constant
m=molality

Temperature in Kelvin

50
Q

What is the effect of adding salt to roads?

A

Doesn’t change the rate of melting

Decreases the rate of freezing

51
Q

Osmotic pressure

A

Sucking pressure genenrated by solutions in which water is drawn into the solution
Must be applied to counteract attraction of water molecules for the solution

52
Q

Osmotic pressure equation

A

II=iMRT

i=van’t Hoff

53
Q

What predicts that Rasoult’s Law will apply?

A

When solute-solute, solvent-solvent, solute-solvents are all very similar

54
Q

Bond breaking

A

Endothermic

55
Q

Bond making

A

Exothermic

56
Q

Charge density

A

Which ions form higher charge numbers

MCAT general Chem (9 decks)

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