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CHEMISTRY-HAWAN > solutions > Flashcards

solutions Flashcards

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1
Q

this is a homogeneous mixture that disperses uniformly throughout another

A

solution

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2
Q

effect that does not scatter a light beam, properly observed for suspensions

A

Tyndall effect

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3
Q

maximum amount of a substance that can be dissolved in a volume of solvent

A

solubility

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4
Q

describes 2 liquids when it is soluble in each other

A

miscibility

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5
Q

give an example of immiscible liquids

A

oil and water

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6
Q

FACTORS AFFECTING SOLUBILITY

“like dissolves like”
- the higher the difference of this factor, the lower the solubility

A

polarity

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7
Q

FACTORS AFFECTING SOLUBILITY

the factor that determines heat increases solubility

A

temperature

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8
Q

FACTORS AFFECTING SOLUBILITY

pressure has high effects on gaseous soluted

ture or false

A

true

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9
Q

DEGREE OF SOLUBILITY

when the rates of dissolution ad preceipitation are equal

A

equilibrium

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10
Q

DEGREE OF SOLUBILITY

contains maximum amount of a solute that will dissolve in a given solvent and temperature

A

saturated

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11
Q

DEGREE OF SOLUBILITY

when the solution contains less solute than its capacity to dissolve

A

unsaturated

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12
Q

DEGREE OF SOLUBILITY

contains more solute and is not stable. some solute will come out as crystals over time

A

supersaturated

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13
Q

DEGREE OF SOLUBILITY

in the phamaceutical industry, most drugs are supersaturated to allow precise doses/deliver drugs with low solubility in water

true or false

A

true

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14
Q

in the formations of solutions, what holds liquid and solid molecules together

A

intermolecular solutions

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15
Q

when solvent particles surround/ wrap around particles to create a solution

A

solvation

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16
Q

DISOLUTION

when more energy is released in making bonds than is used in breaking bonds
- releases energy, temp increases

A

exothermic

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17
Q

DISOLUTION

when more energy is being used than is being released
- absorbs energy and temperature decreases

A

endothermic

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18
Q

which law states that “regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes”

A

hess’ law

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19
Q

formula of hess’ law

A

DHsoln = DH1+DH2+DH3

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20
Q

which law states that “the solubility of gasses is directly proportional to the partial pressure of gas above liquid”

A

henry’s law: gases

21
Q

FORMULAS

mass percentage

A

mass (g) of solute / total mass (g) of solution x100

22
Q

FORMULAS

parts per million

A

mass of solute / mass of solution x 1,000,000

23
Q

FORMULAS

mole fraction

A

moles of component / total moles of solution

24
Q

FORMULAS

moles

A

mass of a substance / molar mass of the substance

25
Q

FORMULAS

molarity

A

moles of solute / liter of solution

26
Q

FORMULAS

molality

A

moles of solute / kg of solvent

27
Q

FORMULAS

dilution

A

C1 V1 = C2 V2

C1 V1 + C2 V2 = C3 V3

28
Q

properties that depend only on the number of solute particles in the solution and not in the nature of the solute particles
- depends on the ratio of the solute and solvent amount

A

colligative properties

29
Q

what are the 3 major colligative properties

A
  • vapor pressure lowering
  • freezing point depression
  • boiling point elevation
    (note* all properties are inversely proportional to solute molar mass)
30
Q

provides more solutes to solution via dissociation; hence, the colligative properties are considerably changed
- depend on the amount of solute regardless of the nature of solute

A

electrolytes

31
Q

provides low solute to the solution since there is no dissociation; hence the colligative properties are not considerably changed

A

nonelectrolytes

32
Q

ELECTROLYTE OR NONELECTROLYTE

sodium chloride

A

electrolyte
- it dissociates, so 1 would yeild 1 molar Na+ ion and 1 molar Cl- ion

33
Q

a unitless constant, directly associated with the degree of dissociation

A

Van’t Hoff Factor

34
Q

TRUE OR FALSE

the vant hoff factor for non electrolytes is always 0

A

FALSE
- it is always 1 or greater because it does not dissociate

35
Q

vant hoff is equal to the number of atoms formed in an aqueous solution
what is i of :
- NaCl
- AlCl3
- HCl

A
  • NaCl: 2 VHF
  • AlCl3: 4 VHF
  • HCl: 2 VHF
36
Q

when vapor is a mixture of solvent and solute

A

volatile solutes

37
Q

when vapor is pure solvent

A

non volatile solute

38
Q

formula for Raoult’s law for nonvolatile vapor pressure lowering

A

P solution =X solvent (P solvent)

39
Q

formula for Raoult’s law for volatile vapor pressure lowering

A

P solution = X solvent P solvent + X solute P solute

40
Q

when does boiling point elevation occur

A

when the BP of a solution becomes higher than the BP of a pure solvent

41
Q

formula for Boiling Point elevation

A

change in temp = i Kb m

i = Vant Hoff constant
Kb = celsius per molal (ebullioscopic constant)
m = molaltity

42
Q

when pure solvent particles become more ordered as the intermolecular forces that opperate between molecules become more permanent

A

freezing point depression

43
Q

selective path if solvent molecules through a porous membrane from a dilute solution to a more concentrated one

A

osmosis

44
Q

allows the passage of solvent molecules but blocks the passage of solute molecules

A

semi-permeable membrane

45
Q

what is the pressure required to stop osmosis and its formula

A

osmotic pressure
= iMRT
i = vant hoff
M = molarity
R = gas constant
T = absolute temp

46
Q

2 solutions are of equal concentration

A

isotonic

47
Q

the more concentrated solution
- when it is on the outside of the cell, it causes it to crenate

A

hypertonic

48
Q

when the cell is more concentrated inside the cells, causing it to swell up and pop

A

hypotonic

CHEMISTRY-HAWAN (3 decks)

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