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Chemistry > unit 13 solutions :/ > Flashcards

unit 13 solutions :/ Flashcards

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1
Q

solution

A

homogenous mixture of two or more substances: clear and will NOT disperse light

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2
Q

solvent

A

dissolves solute

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3
Q

solute

A

dissolved by solvent

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4
Q

soluble

A

able to be dissolved

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5
Q

miscible vs immiscible

A

two LIQUIDS that can mix are miscible, if two liquids cannot they are immiscible (oil and water)

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6
Q

solvation

A

the process of dissolving a solute

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7
Q

how can you tell which is solute and which is solvent?

A

solvent is usually the bigger component, solute is smaller

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8
Q

the solubility rule

A

‘like dissolves like’
substances are soluble when IMFs and forces of attraction are similar

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9
Q

“like dissolves like” rule

A

polar dissolves polar AND ionic
nonpolar only dissolves nonpolar

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10
Q

why does like dissolves like work

A

full charges attract full charges partial charges attract partial charges
nonpolar charges attract IMFs
polar molecules prefer more polar things to fully satisfy charges

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11
Q

review LDMs and polarity

A

LDM ionic
1. draw kernel (symbol with oxidation # changed)
2. put brackets
3. put ion charges around brackets

Molecule LDM
1. add valence electrons
2. put LEAST electroneg in the middle except not hydrogen or halogens
3. -2 es for every bond connecting and put two dots around every atom until 8 around every atom
4. form multiple bonds if necessary

remember, H2S is polar goddamn it

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12
Q

electrolyte

A

a chemical compound that ionizes when dissolved OR MOLTEN and forms an electrically conductive substance
ionic compounds are electrolytes bc they dissolve/melts into loose ions with charges

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13
Q

non electrolytes

A

no mobile ions produced, just molecules (e.g. sugar)
most compounds starting with ‘C’ are nonelectrolytes (unless acid or base sometimes) and bad conductors are not usually electrolytes. covalent = non electrolyte

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14
Q

strong vs weak electrolytes

A

strong electrolytes ionize completely and have a strong current
weak electrolytes ionize partially and have a weaker current

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15
Q

is solution formation a physical or chemical change?

A

physical change (you can get back solute by evaporating solvent)

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16
Q

temperature effect on solubility (and why) (for liquids and solids)

A

increase in temp increases solubility
because particles move faster and move more particles around

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17
Q

temperature effect on solubility (and why) (for gases)

A

temp increase causes solubility decrease for gases because thermal and kinetic energy overcome attractive forces (LDFs)

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18
Q

pressure effect on solids

A

no pressure effect on solubility of solids

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19
Q

pressure effect on gases

A

direct relationship: as pressure increases solubility increases

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20
Q

particle size and solubility

A

smaller particle size increase solubility because can dissolve all at once all exposed

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21
Q

agitation

A

increase solubility bc mixing

22
Q

solution equilibrium

A

another name for a saturated solution: rate of dissolving is equal to the rate of deposition

23
Q

concentration

A

measurement of the amount of solute in a volume of solvent

24
Q

concentrated solution

A

one mole or more of solute

25
Q

diluted solution

A

less than one mole of solute

26
Q

molarity

A

how we express concentration

27
Q

molarity equation: M

A

moles of solution/liters of solution

28
Q

how to make the solution the desired molarity

A
  1. amount of solute needed weighed out on a balance
  2. portion of the solvent is added to the volumetric flask
  3. mixture swirled until solute is dissolved
  4. more solvent added until it reaches the mark on the flask
29
Q

dilution

A

adding water to an existing solution

30
Q

stock solution

A

concentrated solution needed to be diluted

31
Q

working solution

A

solution we end up with after diluting

32
Q

can you add acid to water or water into acid?

A

NEVER add water into acid ALWAYS acid into water

33
Q

what is #M vs m vs ‘m’ in italics

A

M is molar, m is moles, and m in italics is molality

34
Q

ppm formula

A

mass of solute/mass of solution x 10^6

35
Q

percent composition

A

mass of part/mass of whole x 100

36
Q

percent volume

A

volume of solute/volume of solution x 100

37
Q

molality

A

concentration unit, but NOT temp dependent like molarity (bc liters is volume and volume is temp dependent)

38
Q

molality equation

A

moles solute/kg solution

39
Q

mole fraction calcs

A

nx = moles part/moles total

40
Q

dissociation equation

A

shows the ions that an ionic compound will dissolve into
-always H2O on arrow because dissolved in water
-take number on bottom and separate each element and put it in front and then total numbers up (assuming compound is ionic)

41
Q

van’t hoff number

A

an integer that equals
the TOTAL number of
particles into which the
solute dissociates when
it is dissolved in solution
-answer to the dissociation equation
-represented by i

42
Q

ion concentration/total molar concentration of molar compound

A

takes M and do dissociation equation but with moles in answer, just multiply all numbers by the number in front of M

43
Q

colligative properties

A

physical properties that WILL CHANGE when solute is present
-change is based on how many particles are added

44
Q

boiling point colligative property

A

boiling point increases because dissolved particles will interfere with boiling process

45
Q

freezing point colligative property

A

freezing point is lowered with solute because solute particles will interfere with lattice formation

46
Q

vapor pressure colligative property

A

solute lowers vapor pressure because the it obstructs the exit pathway for molecules

47
Q

colligative calculations

A

seek to calculate new boiling and freezing point after solute added

48
Q

colligative calculations formulas

A

DT = Kb m i
DT = Kf m i
DT = change in temp
Kb = molal constant boiling: 0.52 deg C/m
Kf = molal constant freezing: 1.86 deg C/m
m (italics) = molality
i = van’t hoff number

49
Q

Kb (molal constant boiling)

A

0.52 degrees C / molal

50
Q

Kf (molal constant freezing)

A

1.86 degrees C / molal

51
Q

temperature effect on solubility and why (for gases)

A

Chemistry (18 decks)

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