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CHM020 -Ana. Chem > Chapter G: Solutions > Flashcards

Chapter G: Solutions Flashcards

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1
Q
  • may be a liquid, gas, or solid.
  • are spread evenly throughout the solution
  • mix with solvents so the solute and solvent have the same physical state.
  • cannot be separated by filtration, but they can be separated by evaporation.
  • are not visible, but they can give a color to the solution
A

Solutes

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2
Q

Solutes cannot be separated by ____, but they can separated by ____.

A
  • Filtration
  • Evaporation
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3
Q
  • is one of the most common solvents in nature.
  • is a polar molecule due to polar O–H bonds.
  • molecules form hydrogen bonds important in many biological compounds.
A

Water

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4
Q

How does solutions form?

A

When solute-solvent interactions are lare enough to overcome solute-solute and solvent-solvent interactions

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5
Q

Solute: Polar

A

Solvent: polar

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6
Q

Solute: non polar

A

Solvent: nonpolar

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7
Q

play an important role in maintaining the proper function of the cells and organs.

A

Electrolytes

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8
Q

Examples of Electrolytes

A

Sodium, Potassium, Chloride, Bicarbonate

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9
Q

dissociate 100% in water, producing positive and negative ions

A

Strong electrolytes

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10
Q

form solutions that conduct an electric current strong enough to light a bulb.

A

Strong electrolytes

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11
Q

dissociates only slightly in water.

A

Weak electrolyte

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12
Q

forms a solution with a few ions and mostly undissociated molecules

A

Weak electrolyte

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13
Q
  • dissolve as molecules in water.
  • do not produce ions in water.
  • do not conduct an
    electric current
A

Nonelectrolytes

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14
Q

Examples of Strong electrolyte

A

Ionic compounds such as;
- NaCl, KBr, MgCl2, Nano3-
Bases such as:
- NaOh, KOH
Acids such as:
- HCl, HBr, HI, HNO3, HClO4 H2SO4

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15
Q

Examples of Weak electrolyte

A

HF, H2O, NH3, acetic acid

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16
Q

Examples of Nonelectrolytes

A

Carbon compounds such as Methanol, Ethanol, Sucrose, Urea

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17
Q

NaCl

A

Strong electrolyte

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18
Q

KBr

A

Strong electrolyte

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19
Q

MgCl2

A

Strong electrolyte

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20
Q

NaNO3

A

Strong electrolyte

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21
Q

NaOH

A

Strong electrolyte

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22
Q

KOH

A

Strong electrolyte

23
Q

HCl

A

Strong electrolyte

24
Q

HBr

A

Strong electrolyte

25
Q

HI

A

Strong electrolyte

26
Q

HNO3

A

Strong electrolyte

27
Q

HClO4

A

Strong electrolyte

28
Q

H2SO4

A

Strong electrolyte

29
Q

HF

A

Weak Electrolyte

30
Q

H2O

A

Weak Electrolyte

31
Q

NH3

A

Weak Electrolyte

32
Q

HC2H3O2(Acetic acid)

A

Weak Electrolyte

33
Q

CH3OH (methanol

A

Nonelectrolyte

34
Q

C2H5OH(ethanol)

A

Nonelectrolyte

35
Q

C12H22O11(Sucrose)

A

Nonelectrolyte

36
Q

CH4N2O (urea)

A

Nonelectrolyte

37
Q

Types of particles in solution: Strong electrolyte

A

Ions Only

38
Q

Types of Particles in solution: weak electrolyte

A

Mostly molecules and a few ideas

39
Q

Types of particles in Solution: nonelectrolyte

A

Molecules Only

40
Q

is the amount of an electrolyte or an ion that provides 1 mole of electrical charge (+ or −)

A

Equivalent (Eq)

41
Q

1Eq = ?

A

1000 mEq

42
Q
  • contain less than the maximum amount of solute.
  • can dissolve more solute.
A

Unsaturated solutions

43
Q
  • contain the maximum amount of solute that can dissolve.
  • have undissolved solute at the bottom of the container.
A

Saturated Solutions

44
Q

Effect of temperature on solubility

A
  • Solubility of solids increase as temperature increase
  • Solubility of gases decreases as temperature increase
45
Q

states that
* the solubility of a gas in a liquid is directly related to the pressure of that gas above the liquid.
* at higher pressures, more gas molecules dissolve in the liquid.

A

Henry’s Law

46
Q

Henry’s Law:
* the solubility of a gas in a liquid is directly ____ to the ____ of that gas above the ____.

A
  • related
  • pressure
  • liquid
47
Q

Henry’s Law:

  • at ____ ____, more gas molecules dissolve in the _____.
A
  • higher pressures
  • liquid
48
Q

Soluble ionic compounds

A

Sulfates, (SO4^2-) are soluble unless combines with
- Ba2+,
- Pb2+,
- Ca2+,
- Sr2+,
- Hg2^2+

49
Q

an insoluble ionic compound, is used to enhance X-rays

A

Barium Sulfate (BaSO4)

50
Q

an insoluble solid that emerges from a liquid solution

A

precipitate

51
Q
  • Water is added
  • the volume of the solution increases
  • concentration decreases
A

Dilution

52
Q

Formula for concentrations and volumes are related

A

C1V1=C2V2

53
Q
  • When water is added to the concentrated solution, there is no change in number of particles.
  • The solute particles spread as the volume of the solution increases
A

Dilution of a Solution

CHM020 -Ana. Chem (4 decks)

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