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Chemistry (Midterm) > Solutions > Flashcards

Solutions Flashcards

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1
Q

elements, covalent
compounds, and ionic compounds.

A

Pure substances

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2
Q

most matter come into contact
with is a ____ of two or more pure
substances.

A

mixture

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3
Q

does not have a
uniform composition throughout the sample.

A

Heterogeneous mixture

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4
Q

has a uniform
composition throughout the sample.

A

Homogeneous mixture

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5
Q

homogeneous mixture that
contains small particles; liquid solutions are transparent.

A

solutions

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6
Q

2 components of solutions

A

solute and and solvent

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7
Q

The components cannot be separated by filtration

A

solution, colloid

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8
Q

substance present in a lesser
amount in a solution.

A

solute

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9
Q

substance present in a larger
amount in a solution.

A

solvent

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10
Q

homogeneous mixture with larger
particles, often having an opaque appearance; particles cannot be filtered and do not settle out.

A

colloid

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11
Q

heterogeneous mixture containing large particles suspended in a
liquid; particles do not dissolve, can be filtered or separated using a centrifuge.

A

suspension

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12
Q

The components cannot be separated by common filtration techniques.

A

colloid

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13
Q

The components can be separated by filtration or centrifugation

A

suspension

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14
Q

substance that conducts an
electric current in water.

A

electrolyte

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15
Q

substance that does not
conduct an electric current in water.

A

Nonelectrolyte

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16
Q

dissociates completely in
water to form ions.

A

Strong electrolyte

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17
Q

dissociates partially in
water to form some ions, leaving mostly
uncharged molecules.

A

Weak electrolyte

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18
Q

Ions that conduct an electric current; examples include NaCl, KOH, HCl, KBr

A

Strong Electrolyte

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19
Q

molecules with a few ions that conduct an electric current; examples include NH3, CH3CO2H, HF.

A

weak electrolyte

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20
Q

molecules that do not
conduct an electric current; examples include CH3OH, H2O.

A

nonelectrolyte

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21
Q

number of moles of charge
that a mole of ions contributes to a solution.

A

Equivalent (Eq)

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22
Q

equals the
charge on the ion.

A

Equivalents per mole of an ion

23
Q

amount of solute that dissolves in a given amount of solvent, usually reported in grams of solute per 100 mL of solution (g/100 mL).

A

solubility

24
Q

contains the maximum number of grams of solute that can dissolve.

A

saturated solution

25
Q

contains less than the maximum number of grams of solute that can dissolve.

A

Unsaturated solution

26
Q

Solubility principle

A

“like dissolves like”

27
Q

most ionic and polar
covalent compounds are _______ in water

A

soluble

28
Q

solvation releases more energy than required to separate particles, resulting in heat release.

A

Exothermic process

29
Q

separation of particles requires more energy than is released during solvation, resulting in heat absorption.

A

Endothermic process

30
Q

a compound is soluble if it
contains one of the following cations:

A
  • Group 1A cations: Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺
  • Ammonium, NH₄⁺
31
Q

for most ionic and molecular solids, solubility generally _ _ _ as temperature increases

A

increases

32
Q

solubility of a gas in a liquid
is proportional to the partial pressure of
the gas above the liquid.

A

Henry’s law

33
Q

tells how much solute is dissolved in a given amount of solution

A

concentration of a solution

34
Q

– number of grams of solute dissolved
in 100 mL of solution.

A

Weight/volume percent concentration
(w/v%)

35
Q

used to express the concentration of a solute when the solution contains a very small concentration of solute.

A

Parts per million (ppm)

36
Q

number of moles of solute per liter of solution.

A

Molarity (M)

37
Q

properties of a
solution that depend on the concentration of
the solute but not its identity.

A

Colligative properties

38
Q

solute that readily escapes
into the vapor phase.

A

Volatile solute

39
Q

solute that does not readily escape and has a negligible vapor pressure at a given temperature.

A

Nonvolatile solute

40
Q

membrane that
surrounds living cells.

A

Semipermeable membrane

41
Q

allow water and small molecules to pass
across, but ions and large molecules cannot

A

Semipermeable membrane

42
Q

passage of a solvent, usually water, across a semipermeable membrane from a solution of low solute concentration to a solution of higher solute concentration.

A

osmosis

43
Q

pressure that prevents the flow of additional solvent into a solution on one side of a semipermeable membrane.

A

Osmotic pressure

44
Q

two solutions with the
same osmotic pressure

A

isotonic solution

45
Q

– solution that has a lower
osmotic pressure than body fluids.

A

Hypotonic solutions

46
Q

solution that has a
higher osmotic pressure than body fluids.

A

hypertonic solution

47
Q
  • concentration of particles outside the
    cell is higher than inside the cell.
  • water diffuses out of the cell, causing it
    to shrink.
  • this process is called crenation.
A

Hypertonic solution

48
Q
  • concentration of particles outside the
    cell is lower than inside the cell.
  • water diffuses into the cell, causing it to swell and eventually burst.
  • for red blood cells, this swelling and
    rupture is called hemolysis.
A

Hypotonic solution

49
Q

process by which blood is filtered
through the kidneys in the human body.

A

dialysis

50
Q

when a person’s kidneys are incapable of removing waste products from the bood, _ _ _ is used.

A

hemodialysis

51
Q

if cooling is very slow, the solution becomes _________ with solute

A

supersaturated

52
Q

In dilution, the amount of solute is _____

A

constant

53
Q
A

Chemistry (Midterm) (2 decks)

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