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Chemistry OFA > solutions > Flashcards

solutions Flashcards

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1
Q

solution

A

a type of homogenous mixture composed of 2 or more substances

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2
Q

solubility of a substance

A

the amount of substance that will dissolve in a given amount of solvent

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3
Q

what does solubility quantify?

A

the dynamic equilibrium state is achieved when the rate of dissolution equals the rate of precipitation

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4
Q

why does a solution form?

A

because of entropy

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5
Q

entropy

A

the pervasive tendency for energy to spread out, or disperse whenever it is not restrained from doing so: reason why ideal gases mix

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6
Q

what are the different forces that can favor/ prevent the process

A

dispersion
dipole-dipole
hydrogen bond
ion dipole

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7
Q

what are the interactions within a solution

A

solvent-solute interactions
solvent-solvent interactions
solute-solute interactions

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8
Q

solution forms

A

solvent-solute interactions> solvent-solvent and solute-solute interactions

solvent-solute interactions = solvent-solvent and solute-solute interactions

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9
Q

the solution may/may not form depending on the relative disparity

A

solvent-solute interactions < solvent-solvent and solute-solute interactions

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10
Q

what do we use to dissolve something nonpolar?

A

soap molecules are used. the nonpolar chain of the soap molecule will surround the dirt and we get a sphere of soap molecules surrounding the dirt molecules.

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11
Q

how do we separate compounds that are polar from nonpolar?

A

we utilize their different solubility in different solvents

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12
Q

factors that affect solubility

A
  1. pressure (only for gasses)
  2. temperature
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13
Q

henry’s law

A

the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid at a defined temp

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14
Q

henry’s law equation

A

Sgas = kH Pgas

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15
Q

henry’s law and scuba diving

A

we have a higher pressure so there is higher solubility of air into our blood. when we go up is released very quickly bc of the pressure drop. when it is released very quickly it can form bubbles and can cause arterial gas embolism-> can be lethal

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16
Q

is the dissolution of most gases exothermic or endothermic?

A

exothermic

17
Q

is the dissolution of solids in liquids exothermic or endothermic?

A

endothermic

18
Q

equation for molarity

A

molarity= amount solute/ volume solution (the total solution)

19
Q

equation for mole fraction

A

amount solute (mol)/ mass solvent (kg)

20
Q

the equation for parts by mass

A

mass solute/ mass solution x multiplication factor

21
Q

ppm multiplication factor

A

10^6

22
Q

percentage per mass factor

A

100

23
Q

parts per billion factor

A

10^9

24
Q

the equation for the parts by volume

A

volume solute/ volume solution x multiplication factor

25
Q

what is the conc used in medicine

A

mg/dL

26
Q

concentration of dilution

A

m1v1 = m2v2

v2= initial + added

27
Q

colligative properties

A

do not depend on the nature of the solvent or solute, depend only on the relative concentration of the two

28
Q

osmosis

A

the flow of water from a solution of lower solute conc to one of a higher solute conc across a partially permeable membrane

29
Q

osmotic pressure

A

pressure required to stop the osmotic flow

30
Q

what happens when RBCs are placed in isosmotic solution

A

normal shape

31
Q

what happens when RBCs are placed in hyperosmotic solution

A

they lose water and shrivel

32
Q

what happens when RBCs are placed in hypoosmotic solution

A

they swell up and may burst as water flows into the cell

33
Q

reverse osmosis

A

pushes water from the higher solute conc to the lower solute conc.: place a pressure greater than the osmotic pressure

34
Q

reverse osmosis as a water purification process

A

it uses a partially permeable membrane to remove ions, unwanted molecules, and larger particles from drinking water

Chemistry OFA (7 decks)

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