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CHM020 - Analytical Methods for Biology > Chapter 0g: Solutions > Flashcards

Chapter 0g: Solutions Flashcards

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1
Q
  • homogeneous mixtures of two or more substances
  • form when there is sufficient attraction between the solute and solvent molecules
A

solutions

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2
Q

two components of solutions

A
  1. solvent
  2. solute
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3
Q

present in larger amount

A

solvent

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4
Q

present in smaller amount

A

solute

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5
Q

Solutes and solvents may be… ?

A
  • liquid
  • gas
  • solid
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6
Q

solutes are mixed with solvents so that they have the same __ __

A

physical state

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7
Q

solutes in a solution cannot be separated by __, but can be separated by __

A
  • filtration
  • evaporation
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8
Q
  • one of the most common solvents in nature
  • polar molecule due to polar O-H bonds
  • molecules form hydrogen bonds
A

water

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9
Q

what type of molecule is water

A

polar molecule (O-H bonds)

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10
Q

How are solutions formed

A

solute-solvent interactions are large enough to overcome solute-solute interactions and solvent-solvent interactions

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11
Q

what dissolves what

A

like dissolves like
(polar - polar)
(nonpolar - nonpolar)

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12
Q

ex. of nonpolar molecules

A
  1. iodine
  2. oil
  3. grease
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13
Q

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

A

electrolytes

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14
Q

Types of electrolytes

A
  1. strong electrolytes
  2. weak electrolytes
  3. nonelectrolytes
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15
Q
  • dissociate 100% in water
  • produce positive and negative ions
  • form solutions that conduct an electric current strong enough to light a bulb
A

strong electrolytes

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16
Q
  • dissociates only slightly in water
  • forms a solution with a few ions and mostly undissociated molecules
A

weak electrolytes

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17
Q
  • dissolve as molecules in water
  • do not produce ions in water
  • do not conduct an electric current
A

nonelectrolytes

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18
Q

Ex. of strong electrolyte formula

A

NaCl(s) –> Na+(aq) + Cl-(aq)

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19
Q

Ex. of weak electrolyte formula

A

HF(aq) <–> H+(aq) + F-(aq)

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20
Q

Ex. of nonelectrolyte formula

A

C12H22O11(s) –> C12H22O11(aq)

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21
Q

Examples of strong electrolytes

A
  • ionic compounds
  • acids such as HCl, HBr, HI, HNO3, HClO4, H2SO4
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22
Q

Examples of weak electrolytes

A
  • HF
  • H2O
  • NH3
  • HC2H3O2 (acetic acid)
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23
Q

Examples of nonelectrolytes

A

carbon compounds
- methanol (CH3OH)
- ethanol (C2H5OH)
- sucrose (C12H22O11)
- urea (CH4N2O)

24
Q

amount of an electrolyte or an ion that provides 1 mole of electrical charge

A

equivalent (Eq)

25
Q

In solution, the charge of positive and negative ions are always __

A

balanced

26
Q

electrolytes in intravenous fluids are expressed in __

A

mEq/L

27
Q

maximum amount of solute that dissolves in a specific amount of solvent

A

solubility

28
Q

how is solubility expressed

A

g of solute / 100 g water

29
Q

Two types of solution

A
  1. unsaturated solution
  2. saturated solution
30
Q
  • contain less than the maximum amount of solute
  • can dissolve more solute
A

unsaturated solutions

31
Q
  • contain the maximum amount of solute that can dissolve
  • have undissolved solute at the bottom of the container
  • contain solute that dissolves as well as solute that recrystallizes in an equilibrium process
A

saturated solutions

32
Q

saturated solution formula

A

solute + solvent –> (solute dissolves) (solute recrystallizes) <– saturated solution

33
Q

where does solubility depend

A

temperature

34
Q

solubility of solids:
temperature increases

A

more soluble

35
Q

solubility of gases:
temperature increases

A

less soluble

36
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

37
Q

when the pressure of a gas above a solution decreases, what happens to the solubility of that gas in the solution

A

also decreases

38
Q

How are ionic compounds soluble in water

A

if they contain soluble cation or anion

39
Q

Soluble in Water:
Positive ions

A
  1. Li+
  2. Na+
  3. K+
  4. Rb+
  5. Cs+
  6. NH4+
40
Q

Soluble in Water:
Negative ions

A
  1. NO3 -
  2. C2H3O2 -
  3. Cl -
  4. Br -
  5. I -
  6. SO4 2-
41
Q

Cl-, Br-, I- are insoluble when combined with…?

A
  1. Ag+
  2. Pb 2+
  3. Hg2 2+
42
Q

SO4 2- is insoluble when combined with…?

A
  1. Ba 2+
  2. Pb 2+
  3. Ca 2+
  4. Sr 2+
  5. Hg2 2+
43
Q

Ionic compounds that do not contai at least one of the soluble ions are usually __

A

insoluble

44
Q

used to enhance x-rays

A

BaSO4

45
Q

mass percent (m/m)

A

g/g

46
Q

volume percent (v/v)

A

mL/mL

47
Q

mass/volume percent (m/v)

A

g/mL

48
Q

When writing a net ionic equation, what is removed

A

spectator ions

49
Q

ions which do not participate in chemical reactions and present the same on both sides of the reactions

A

spectator ions

50
Q

a solvent, usually water, is added to a solution, which increases its volume and decreases the concentration of the solution

A

dilution

51
Q

what is added in a dilution

A

water

52
Q

what is the same in the initial and diluted solution

A

moles of solute

53
Q

equation that relate concentration and volumes

A

C1V1 = C2V2

54
Q

concentration, C, may be __ or __

A
  • percent concentration
  • molarity
55
Q

Freezing point depression of water

A

1.86°C kg/mol

56
Q

Boiling point elevation of water

A

0.515°C kg/mol

CHM020 - Analytical Methods for Biology (22 decks)

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