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SRNAChem&Physics > Chapter 8 > Flashcards

Chapter 8 Flashcards

1
Q

Mol /kg of solvent

A

Molality

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2
Q

moles of solute/Liter of solution

A

Molarity

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3
Q

Percentt by weight

A

allows you to measure out a volume of medicine in a syringe, and calculate the mass of the drug

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4
Q

Percent by volume

A

not on the test

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5
Q

Equivalents (Eq)

A

Analogous to mole

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6
Q

Equivalent definition

A

one Eq of a substance contains one mole of chemical reactivity

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7
Q

Ex One Eq of an acid can deliver

A

one mole of H+ ions

1 Eq/mol of H+

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8
Q

Ex calcium has

A

2 Eq /mol

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9
Q

1 mol is expressed in

A

Eq/L

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10
Q

1 mol of Ca is

A

1 mol / 2 eq

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11
Q

Parts per million

A

can be used as away to define concentration

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12
Q

PPM calculates as

A

grams of solute per one million grams of solution

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13
Q

What is the concentration of a solution in parts per million,

A

0.02/1000

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14
Q

Solubility

A

the mass of solute that will dissolve in a given amount of solvent

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15
Q

NACL is

A

very soluble in water

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16
Q

O2 is

A

not very soluble in water

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17
Q

A saturation solution contains

A

the maximum amount of solute as defined by its solubility

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18
Q

Supersaturated solution

A

contains a concentration greater than its solubility limit. The solute precipitates out

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19
Q

Example of supersaturation (2)

A
  • excessive amount of ca2 in the blood precipitate out as calcium crystals forming kidney stones
  • Sodium acetate crystals precipitate out of supersaturated solution
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20
Q

Factors affecting solubility: Increases pressure

A

Increase pressure = increase gas solubility in a liquid

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21
Q

Factors affecting solubility: Increasing Temperature

A

Increase solids & Liquids solubilities in other liquids

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22
Q

Factors affecting solubility:Increasing temperature, ______gas solubility in a liquid

A

Decrease solubility in a liquid

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23
Q

Henry’s Law

A

give relationship between pressure and solubiliy

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24
Q

S=

A 
S= K(h) P(gas)
S= Solubility
K(h) = Henry's constant
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25
Q

Henry’s law

A

if you double the pressure in the chamber with pure oxygen, the amount of oxygen dissolve in the water doubles to 84mg/L

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26
Q

Henry’s law

A

but if you have mix of gases, then you have to account for partial pressure. For examples, @ 2 atm in the chamber we have mix of 50% oxygen & 50% nitrogen

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27
Q

The henry’s law constant for oxygen in water 0.042g/L/atm at 25C. What is the solubilityis mg /L of O2 in pure water at 740 torr room air ?

A 
Fist convert torr to atm = 0.974 atm
oxygen is 21% : (0.21) (0.974) = 0.204 atm
now plug in number
S= (0.042)(0.204)= 0.0086g/L
Concert to mg/L
Final : 8.6mg/L
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28
Q

Heats of solution

A

forming solution can be endothermic (solution gets cold) exothermic ( solution gets hot) depending on the intermolecular forces and particle interaction between the solute particles themselves and the solvent particles.

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29
Q

Lattice energy

A

the attraction of solute particles for each other

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30
Q

Solvation energy

A

the attraction of solute particles and solvent molecules

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31
Q

When a solution form if lattice> solvation

A

endothermic (because it takes energy out of the solvent to break apart the lattice)

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32
Q

When a solution form if lattice < solvation

A

exothermic , because energy is released into the solvent

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33
Q

Mole fraction of a solute is equal to

A

the moles of solute in a sample divided by the total number of moles of substances in the sample

34
Q

Xi =

A

mol (I) / mol (I) + mol (solvent)

35
Q

Osmosis Capital PI =

A

MRT
M molarity
R is the idea gas constant
T (temp in Kelvin)

36
Q

Osmosis definition

Tonicity definition

A

movement of water across a semipermeable membrane from an area of greater concentration to an area of lesser concentration
- Tonicity describes the concentration of 2 solutions relative to each other.

37
Q

What osmotic pressure would an aqueous solution of 1 mol of glucose exert against pure water at 298K?

A

(1mol/L) (0.0821 L/atm/mol/k) (298)=

24.5 atm

38
Q

Osmosis and tonicity

A

net movement of H2o into and out of RBC

39
Q

What is a solution?

Ex?

A

homogeneous mix of solutes in a solvent

Ex: Salt in water

40
Q

Homogenous means there are no

A

visible phase boundaries

41
Q

MISCIBLE refers to

A

liquids that mix evenly, forming homogenous solution that do not separate

42
Q

Miscible or Immiscible–>Water and methylene

A

Immiscible

43
Q

Miscible or Immiscible–>Acetone and water

A

Miscible

44
Q

Solution vs colloid vs suspension depends on

A

Particle size.

45
Q

Particles size less than 10^-7cm

A

True Solution

46
Q

Particles size between 10^-7cm to 10^-5cm

A

Colloid Solution

47
Q

Particle size greater than 10^-5cm

A

Suspensions

48
Q

Appearance of a solution is ________ and appearance of colloid is ________

A

transparent; cloudy

49
Q

Particle size of a solution is ____________ and particle size of colloid is __________

A

Molecule size ; variable , larger than molecule

50
Q

Effect of light : Tyndall effect on solution?

A

None

51
Q

Effect of light : Tyndall effect on colloid?

A

Light dispersed in a ray

52
Q

Solutes dissolves in

A

Solvents

53
Q

Solutes and solvents, both can be

A

liquid, solids or gases

54
Q

Example of liquid solute in liquid solvent

A

Alcohol: 70% isopropanol

30% water

55
Q

Example of solid solute in liquid solvent

A

0.9% NaCl

56
Q

Example of gas solute in liquid solvent

A

CO2 in beer

57
Q

Example of solid solute in solid solvent

A

Stainless Steel alloys

58
Q

What is the definition of molarity

A

Mole of solute per liter of solution(mol/L)

59
Q

What are Colligative Properties?

A

Physical properties of a solution that are affected only by the CONCENTRATION of SOLUTE particle, NOT BY THE identity of the solute itself.

60
Q

Example of the application of colligative properties

A 
By adding salt to water you change the colligative properties of the water:
Vapor pressure Decreased
Boiling point Increased
Freezing point Decreased
Osmotic pressure increased
61
Q

Vapor pressure _________ as more solute is added

A

Decreases

62
Q

Addition of solute and vapor pressure

A

inverse proportional relationship

63
Q

Salts lowers

A

Freezing point of water

64
Q

Salt raises

A

boiling point of water

osmotic pressure of blood

65
Q

If you dissolved 1 mol of glucose in enough water to give you a total 1L of solution, you would have________and not ________

A

1 molar solution of glucose: 1 L of water

66
Q

If you started with 1L of water and then added 1 mol of glucose,

A

the final solution would be more than 1L

67
Q

Calculate the molarity of a D5W solution prepared by dissolving 1 g of C6H12O6 in enough water to give a total volume of 20ml?

A 
1g/180g = 0.0055555
Mol = 0.0055555/ 0.02L
M = 0.28
68
Q

Relationship of molarity with temperature?

why?

A

Inverse proportional relationship–> as temperature increases, molarity decreases
Volume of the solvent EXPANDS at higher temperature

69
Q

MoLAlity

A

mol of solute / kg of solvent (not liter)

70
Q

If you dissolved 1 mol of NaCl in 1 kg of water, you would have

A

1 molal solution of NaCl

71
Q

% w/v

A

Defined as gram of solute per 100ml of solution

Grams of solute / ml of solution x100%

72
Q

What is the concentration of a solution prepared by dissolving 25g of glucose in enough water to give a total volume of 500ml?

A

25/500 x 100= 5%

73
Q

How many liters of D5W are required to deliver 100g of glucose?

A

2000ml

74
Q

what is the percent by weight concentration of glucose in a solution prepared by dissolving 25g of glucose in 475 g of water?

A

25/500 x 100 =5%

75
Q

When expressing Eq of electrolyte cations in the body, the number of Eqs in a mole is equal to

A

the charge on the cation.

76
Q

Blood work says 40mEq/L , calculate mole per Liter?

A

First convert mEq to Eq

than 1mol = 2 Eq

77
Q

Parts per million (ppm)

A
  • can be use a way to define concentration
  • concentrate as gram of solute per one million g of solution
    ppm = grams of solute/grams of solution x1,000,000
78
Q

What is the concentration of a solution, in pars per million. If 0.02g of NaCL is dissolved 1000 g of solution

A

0.02g/1000g x 1000000 = 20ppm

79
Q

What is the PPM concentration of chromium in the blood if we have a level of 2.5mcg per 100ml? (blood density =1.06g/ml)

A

0.024ppm

80
Q

What osmotic pressure would an aqueous solution of 1 mol of glucose exert against pure water at 298K?

A

24.5atm

SRNAChem&Physics (13 decks)

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