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Bioscience > Fluids (Solution/Solubility) CH 5 &8 > Flashcards

Fluids (Solution/Solubility) CH 5 &8 Flashcards

1
Q

What is a fluid

A

Any material that has the ability to flow

Both liquid and gases are considered fluids

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2
Q

Hydrostatics

A

is the study of fluids that are NOT MOVING

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3
Q

Hydrodynamics

A

is the study of fluids that ARE MOVING

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4
Q

For hydrostatic fluids, what two properties are important to consider

A

density (p) and pressure (P)

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5
Q

If density is known, what is the formula to calculate for pressure

A

P = pgh

p=density
g=gravity
h=height

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6
Q

Density of water

A

1g/m^3 or 1g/cm^3
1000kg/m^3 or 1000kg/cm^3
8.33 lb/gal

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7
Q

1Pa =

A
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8
Q

Formula for hydrostatic pressure

A

p= density
g= gravity
h= height

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9
Q

Formula for pressure variation (pressure that accounts for top and bottom)

A

P2 = bottom
P1= top

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10
Q

Is pressure affected by container shape?

A

No, pressure is independent of container shape.

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11
Q

Pascal’s Principle states

A

If you apply external pressure to a confined fluid, that pressure is transmitted unchanged to every point within the fluid

Ex: if we increase P1 (top) by 5psi, the P2 (bottom) will be the original pressure plus 5psi

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12
Q

Buoyant Force states

A

all fluids exert a buoyant force on objects immersed in them

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13
Q

Normal Forces

A

Describes forces that are perpendicular to a surface

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14
Q

What is the Buoyant Force Formula

A

note: (pgV) represents weight (which is a force) of displaced fluid

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15
Q

Archimedes’ Principle states

A

An object immersed either totally or partially in a fluid feels a buoyant force equal to the weight of fluid displaced

Formula
Wapparent = Wtrue - Fb

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16
Q

If Density of object > Density of fluid, what will happen?

A

Object will sink

Fb < Wtrue

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17
Q

If Density of object < Density of fluid, what will happen?

A

Object will float

Fb > Wtrue

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18
Q

If Density of object = Density of fluid, what will happen?

A

Object will remain stationary in the fluid

Fb = Wtrue

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19
Q

Hydrometer is

A

a very simple device used to measure the specific gravity of liquids such as urine or milk

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20
Q

What are the 2 types of hydrodynamic flows

A

Laminar Flow
Turbulent Flow

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21
Q

Laminar flow is

A

unchanging flow pattern

smooth and orderly

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22
Q

Turbulent Flow is

A

continuously varying pattern flow

chaotic and abrupt

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23
Q

Flow rate is

A

the volume of fluid passing a particular point per unit of time

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24
Q

What is the SI unit of flow rate

A

m^3/s

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25
Q

What happens to the speed of water when diameter is made smaller?

A

It increases tremendously

decrease diameter = increase speed

assuming no leaks, volume and density will remain unchanged

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26
Q

Incomprehensible Fluids are

A

fluids whose volume or density do not change with pressure

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27
Q

What is the formula to calculate incomprehensible fluid flow rate?

aka The Continuity Equation

A

A1v1=A2v2

A= area
v= speed of incomprehensible fluid (flow rate)

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28
Q

Circular cross-sectional flow rate

A

Flow rate = Av=TTr^2v

A = TTr^2
v=speed of fluid (flow rate)

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29
Q

The Bernoulli Effect states

A

as the speed of a fluid increases, the pressure exerted by the fluid decreases

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30
Q

What is the Bernoulli Formula

A

pgh1 and pga 2 cancel out

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31
Q

Force equals

A

Pressure x Area

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32
Q

What is a Venturi tube flowmeter

A

Device used to measure fluid speed in pipes

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33
Q

What is the U-tube and what does it do?

A

U-tube is a manometer and we can use it to measure the differences in pressures (P1-P2)

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34
Q

What is the Venturi Tube Flowmeter Equation

A
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35
Q

What is the difference between ideal fluids and real fluids

A

Ideal fluids are those in which there is no loss of energy due to friction, no interactions between molecules, no interactions between molecules and pipe, tubing, or container.

Real fluids are what we deal with every day

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36
Q

What is viscosity

A

the measure of a fluid’s resistance to flow

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37
Q

What determines the speed of fluid through a pipe?

A

The closer a molecule to the wall, the slower it will move

Those closest to the center of the pipe will move the fastest

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38
Q

what must be introduced in order for real fluids to maintain flow?

A

A force

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39
Q

What is the equation for viscosity?

A
40
Q

what is Poiseuille’s Equation?

A
41
Q

Reynold’s Number is

A

A dimensionless qty that is used to characterize flow

If Nr < 2k = Laminar flow
If Nr > 3k = Turbulent flow
if between 2-3k= unstable

42
Q

Reynold’s Number if formulated as

A

d= diameter of pipe
p=density
v=speed
n=viscosity

43
Q

what is a solution?

A

a homogenous mixture of one or more solutes UNIFORMLY dispersed at the molecular or ionic level in a given solvent

44
Q

What is homogenous mixture

A

it is not possible to discern phase boundaries between the components of the mixture

45
Q

What is phase boundary

A

a boundary that separates/demarcates the regions of mixture where chemical or physical properties of the mixture change (ex vomit)

46
Q

What is a solute

A

the material that gets dissolved (present in smaller quantities)

47
Q

what is a solvent

A

the material that does the dissolving

48
Q

Are all solutions liquids?

A

No, they can be liquid, gas or solid

49
Q

What is molarity (M)?

A

molarity (molar concentration) is defined as the moles of a solute per liter of solution (Mass/Volume).

It is the most common concentration unit in chemistry

It is TEMPERATURE DEPENDENT

as temp goes up, volume goes up and molarity will decrease

50
Q

What is Molality (m)?

A

Molality (molal concentration) expresses the concentration in terms of moles of solute per kg of solvent (mass/mass)

Mass is NOT temperature dependent, therefore molality is independent of this factor

Molality finds application in physical chemistry, often necessary to consider the quantities of solute and solvent separately, rather than as a mixture.

51
Q

Are molarity and molality equal?

A

NEVER, but the differences become smaller as solutions become more dilute

52
Q

What do you need to know in order to convert between molality and molarity?

A

Density of the solution

53
Q

What is percent by weight to volume (%w/v)?

A

Defined as grams of solute per 100 mL of solution

54
Q

What is percent by weight to weight (%w/w)?

A

Defined as grams of solute per 100g of solution

55
Q

what is percent by volume to volume (%v/v)

A

never used because volumes are not additives

56
Q

What is an equivalent (Eq) analogous to?

A

a mole (mol)

1 Eq = 1 mol

57
Q

What is Normality analogous to?

A

Molarity (M)

58
Q

When expressing the Eq of electrolyte cations, the number of Eq in a mol is equal to ?

A

The charge on the cation

Ex: Ca2+ has 2 cations, so 2Eq/mol

59
Q

How do we solve for Normality (N) expressed in Eq/L ?

A

Remember Eq/L can go to mol/L because 1Eq=1mol and we use the number on the cation charge as the Eq/mol converting factor

ex: 0.40 Eq/L Ca2+ (2Eq/mol) so…
0.40Eq/L x mol/2Eq = 0.020 mol/L

60
Q

Parts per million (PPM) is used when?

A

to express the concentration of extremely dilute solutions.

It is analogous to a percent except e are comparing the amount of g solute to a MILLION g of solution rather than 100g

61
Q

1 mL = g?

A

1.06g = 1mL

62
Q

1PPM = ? mg/L

A

1 mg/mL

63
Q

What is solubility?

A

the amount of solute that will dissolve in a. given solvent at a given temperature

64
Q

Define a saturated solution

A

solution that contains the max amount of solute it can absorb

65
Q

Define supersturated

A

solution that contains more solute than allowed; unstable, will leak out of solution and either crystalize as a solid, separate as a liquid, or bubble out as a gas

66
Q

What is the rule of thumb?

A

“Like dissolves Like”

polar solutes are more soluble in polar solvents

non polar solutes are more soluble in non polar solvents

67
Q

Most polar species are ?

A

ionic compounds, followed by those that can form hydrogen bonds such as water and ethanol

68
Q

What is energy change?

A

When a solute dissolves in a solvent, an associated energy change occurs, resulting in a change in temperature.

Energy change = Heat of the solution or Enthalpy of Solution

69
Q

Define Enthalpy (H)

A

The energy change that accompanies dissolving exactly 1 mol of solute in a given solvent

Enthalpy is a state function

Enthalpy (H) = Energy (Q) as long as the pressure remains constatnt

70
Q

If a solution process is endothermic, what happens to the energy of the system?

A

Energy is going INTO they system from the surroundings, so energy will INCREASE in the system; it will increase enthalpy (H)

71
Q

If a solution process is exothermic, what happens to the energy of the system?

A

Energy is going OUT of the system onto the surrounding, so there is an energy loss. System cools, Enthalpy (H) will DECREASE

72
Q

What is Coulomb’s law?

A

Opposite charges attract

73
Q

What is solvation?

A

involves opposite charges coming toward each other through EXOTHERMIC process. Very messy process

74
Q

What is lattice energy?

A

Energy required to separate 1 mol of an ionic compound into its constituent ions (cation/anion) in the gas phase

75
Q

What determines if the heat of the solution is an endothermic or exothermic process

A

Depends on the relative magnitudes of the lattice energy and heat of solution (H)

If energy released by solvation < energy required to tear ions apart, then H = ENDOTHERMIC

If energy related by solvation > energy required to tear ions apart, then H = EXOTHERMIC

76
Q

How does pressure affect solubility of a gas solute in a liquid solvent?

A

as pressure increases, solubility increases

77
Q

How does pressure affect solubility of a solid or liquid?

A

Pressure has very little effect on solubility of solids and liquid solutes since they are NOT COMPRESSIBLE

78
Q

What does Henry’s Law state?

A

if the pressure of a gas over liquid increases, then the amount of gas dissolved (solubility) in the liquid will increase proportionally

79
Q

What is Henry’s constant Kh?

A

42mg/L/atm
or
0.042g/L/atm

80
Q

How does the temperature affect solubility of solid and liquid solutes in liquid solvents?

A

as temp increases, solubility increases

81
Q

How does the temperature affect solubility of gas solutes in liquid solutes?

A

as temp increases, solubility decreases

82
Q

What are colligative properties

A

properties of solutions that DEPEND on the NUMBER of solute particles and NOT the IDENTITY of the solute particles

83
Q

What are the 4 commonly cited colligative properties?

A

As concentration of solute increases:

1) Vapor pressure decreases
2) Boiling point increases
3) Freezing point decreases
4) Osmotic pressure increases (most dramatic!)

84
Q

What results will vapor pressure have when the concentration of a solute increases

A

colligative property

the VP will decrease, which means more heat (Q) is needed to increase the VP to ambient pressure

85
Q

What does Raoult’s Law state?

A

The vapor pressure of a volatile component of a solution (P) is qual to the vapor pressure of the pure substance (Pdegree) times the mole fraction (X) of that substance

86
Q

Dalton’s law of partial pressure states

A

Total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual component gases

87
Q

Define boiling point

A

The temperature at which the vapor pressure of the material is equal to the ambient pressure

88
Q

Change in the boiling point temperature is equal to what?

A

change in boiling point is directly proportional to the molar concentration of the solute particles

89
Q

What is the Ebullioscopic constant (Kbp) of water?

A

0.512 (degrees C)/molal (m)

90
Q

What is the freezing point

A

Freezing point (or melting point) of a sample is the temperature at which the liquid phase of the material is in equilibrium with the solid phase

91
Q

What is the cryoscopic constant (Kfp) of water

A

1.86 (degrees C)/molal (m)

92
Q

Describe the levels of tonicity (isotonic, hypertonic, hypotonic)

A
93
Q

What is osmotic pressure (TT)?

A

The drive for the concentration of water to equalize.

Where,
TT=MRT

TT=Osmotic Pressure
M=Molarity
R= Ideal gas constant
T= Absolute temperature

94
Q

What is the ideal gas constant (R)?

A

0.08206 (Lxatm)/(mol/K)

95
Q

What are colloids?

A

Consist of one phase uniformity dispersed in a second phase

Not true solutions

particles are larger! (x100-1000s)

Cannot be filtered and do not settle out of solution

Have Tyndall effect

96
Q

What is the Tyndall effect?

A

When shine a light, particles are large enough to scatter

97
Q

Types of colloids

A

Blood, protiens, starch (hetastarch), milk

Bioscience (5 decks)

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