Chapter 4_3&4

8/10/2019 Chapter 4_3&4

1/93

Prentice Hall 2003 Chapter 13

Chapter 4_3

Physical Transformation of

Pure Substances

David P. White

8/10/2019 Chapter 4_3&4

2/93


Viscosity

Viscosity is the resistance of a liquid to flow.

A liquid flows by sliding molecules over each other.

The stronger the intermolecular forces, the higher the

viscosity.

Example: glycerol C3H8O3(1.49 Ns/m2) and water

(1.01x10-3Ns/m2)

Some Properties of Liquids

8/10/2019 Chapter 4_3&4

3/93

Surface Tension

Surface Tension

Bulk molecules (thosein the liquid) are

equally attracted to

their neighbors.

8/10/2019 Chapter 4_3&4

4/93


Surface Tension

Surface molecules are attracted downwards and sideways by other

molecules but not upwards away from the surface.

Therefore, the surface to tighten like an elastic film Surface tension is the amount of energy required to stretch or

increase the surface area of a liquid.

Liquids with strong intermolecular forces have higher surface

tension Cohesive forcesbind molecules to each other.

Adhesive forcesbind molecules to a surface.


8/10/2019 Chapter 4_3&4

5/93


Surface Tension

Meniscusis the shape of the liquid surface.

If adhesive forces are greater than cohesive forces, the liquid

surface is attracted to its container more than the bulkmolecules. Therefore, the meniscus is U-shaped (e.g. water in

glass).

If cohesive forces are greater than adhesive forces, the meniscus

is curved downwards. (e.g mercury) Capil lary Action: When a narrow glass tube is placed in

water, the meniscus pulls the water up the tube.


8/10/2019 Chapter 4_3&4

6/93


Transformation from one phase to another,

Occur when energy (usually heat) is added or removed from a

substance Sublimation: solid gas. Hsub> 0 (endothermic).

Vaporization: liquid gas. Hvap> 0 (endothermic).

Melting orfusion: solid liquid. Hfus> 0 (endothermic).

Deposition: gas solid. Hdep< 0 (exothermic).

Condensation: gas liquid. Hcon< 0 (exothermic).

Freezing: liquid solid. Hfre< 0 (exothermic).

Phase Changes

8/10/2019 Chapter 4_3&4

7/93

Phase Changes

8/10/2019 Chapter 4_3&4

8/93

Liquid-vapor equilibrium

Collision rate higher in liquid phase.

Molecules in liquid phase have sufficient energy to escapefrom the surface a phase change occurs

evaporation/vaporization.

Evaporation depends on temperature: higher T, greater kinetic

E, hence more molecules leave the liquid.


Phase Changes

8/10/2019 Chapter 4_3&4

9/93


Explaining Vapor Pressure on the

Molecular Level

Some of the molecules on the surface of a liquid have

enough energy to escape the attraction of the bulk liquid.

These molecules move into the gas phase.

As the number of molecules in the gas phase increases,

some of the gas phase molecules strike the surface and

return to the liquid. After some time the pressure of the gas will be constant

at the vapor pressure.

Vapor Pressure

8/10/2019 Chapter 4_3&4

10/93



Molecular Level

Vapor Pressure

8/10/2019 Chapter 4_3&4

11/93



Molecular Level

Dynamic Equilibrium: the point when as many molecules

escape the surface as strike the surface.

Vapor pressure is the pressure exerted when the liquidand vapor are in dynamic equilibrium.

Volatility, Vapor Pressure, and Temperature

If equilibrium is never established then the liquidevaporates.

Volatile substances evaporate rapidly.

Vapor Pressure

8/10/2019 Chapter 4_3&4

12/93


Vapor Pressure and Boiling Point

Liquids boil when the external pressure equals the vapor

pressure.

Vapor pressure of a liquid increases with increasingtemperature

Vapor Pressure

8/10/2019 Chapter 4_3&4

13/93

Molar heat of vaporization and boiling point

A measure of strength of intermolecular forces in a liquid is the

molar heat of vaporization Energy required to vaporize 1 mole of a liquid

Strong intermolecular forces in liquid, high molar heat of

vaporization, low vapor pressure

Vapor pressure of a liquid increases with increasing temperature Relationship between vapor pressure of a liquid and the absolute

temperature is given by the Clausius-Clapeyron equation


Phase Changes

8/10/2019 Chapter 4_3&4

14/93

Clausius-Clapeyron equation

Can determine heat of vaporization by slope.


Phase Changes

8/10/2019 Chapter 4_3&4

15/93

If we know the values of Hvap and P of a liquid at one

T, can use Clausius-Clapeyron equation to calculate the

vapor pressure of liquid at different T


Phase Changes

8/10/2019 Chapter 4_3&4

16/93

Example 1

Diethyl ether is a volatile, highly flammable organic

liquid that is used mainly as a solvent. The vapor

pressure of diethyl ether is 401 mmHg at 18o

C. Calculateits vapor pressure at 32oC. Hvap = 26.0 kJ/mol


8/10/2019 Chapter 4_3&4

17/93

Boling point

At boiling point, bubbles form within liquid

When bubble forms the liquid originally occupying that space ispushed aside and level of liquid in container is forced to rise.

The P exerted on the bubble is largely atmospheric pressure.

The P inside bubble is due solely to the vapor pressure of liquid.

when vapor pressure = external pressure, bubble rise to surface ofliquid and burst.

If vapor pressure in bubble lower than external pressure bubble

collapse before it could rise


Phase Changes

8/10/2019 Chapter 4_3&4

18/93

We can conclude that boiling point of liquid depends on

external pressure.

Bcoz boiling point defined in terms of vapor pressure ofliquid, we expect boiling point to be related to the molar

heat of vaporization.

Higher heat of vaporization, higher boiling point

Both determined by strength of intermolecular forces

Ar and methane (weak dispersion forces) low bp and Hvap

Ethanol and water (H-bonding) high bp and HvapPrentice Hall 2003 Chapter 13

Phase Changes

8/10/2019 Chapter 4_3&4

19/93

Molar heat of fusion- energy required to melt 1 mole of a

solid

Molar heat of sublimation- energy required to sublime 1mole of a solid

Hsub= Hfus+ Hvap


Phase Changes

8/10/2019 Chapter 4_3&4

20/93


8/10/2019 Chapter 4_3&4

21/93

Example 2

Calculate the amount of energy needed to heat 346 g of

liquid water from 0oC to 182oC. Assume that the

specific heat of water is 4.184 J/go

C over the entireliquid range and that the specific heat of steam is 1.99 J/goC.


8/10/2019 Chapter 4_3&4

22/93


Phase diagram: plot of pressure vs. Temperature

summarizing all equilibria between phases.

Given a temperature and pressure, phase diagrams tell uswhich phase will exist.

Any temperature and pressure combination not on a

curve represents a single phase.

Phase Diagrams

8/10/2019 Chapter 4_3&4

23/93


Features of a phase diagram:

Triple point: temperature and pressure at which all three phases

are in equilibrium. Vapor-pressure curve: generally as pressure increases,

temperature increases.

Critical point: critical temperature and pressure for the gas.

Melting point curve: as pressure increases, the solid phase isfavored if the solid is more dense than the liquid.

Normal melting point: melting point at 1 atm.

Phase Diagrams

8/10/2019 Chapter 4_3&4

24/93


Critical Temperature and Pressure

Every substance has a:

Critical temperature, Tc:

Above it gas phase cannot be made to liquefy nomatter how great the applied pressure

Highest T at which a substance can exist as a liquid

Above Tc, there is no fundamental distinction betweenliquid and gas

Critical pressure, Pc: minimum pressure required for

liquefaction at Tc

Phase Diagrams

8/10/2019 Chapter 4_3&4

25/93


Phase Diagrams

8/10/2019 Chapter 4_3&4

26/93


The Phase Diagrams of H2O and CO2

Phase Diagrams

8/10/2019 Chapter 4_3&4

27/93



Water:

The melting point curve slopes to the left because ice is less

dense than water. Triple point occurs at 0.0098C and 4.58 mmHg.

Normal melting (freezing) point is 0C.

Normal boiling point is 100C.

Critical point is 374C and 218 atm.

Phase Diagrams

8/10/2019 Chapter 4_3&4

28/93



Carbon Dioxide:

Triple point occurs at -56.4C and 5.11 atm.

Normal sublimation point is -78.5C. (At 1 atm CO2sublimesit does not melt.)

Critical point occurs at 31.1C and 73 atm.

Phase Diagrams

8/10/2019 Chapter 4_3&4

29/93


Chapter 4_4Properties of Solutions

David P. White

8/10/2019 Chapter 4_3&4

30/93


A solution is a homogeneous mixture of solute (present in

smallest amount) and solvent (present in largest amount).

Solutes and solvent are components of the solution.

In the process of making solutions with condensed

phases, intermolecular forces become rearranged.

The Solution Process

8/10/2019 Chapter 4_3&4

31/93

8/10/2019 Chapter 4_3&4

32/93



8/10/2019 Chapter 4_3&4

33/93


Energy Changes and Solution

Formation

There are three energy steps in forming a solution:

separation of solute molecules (H1),

separation of solvent molecules (H2), formation of solute-solvent interactions (H3).

We define the enthalpy change in the solution process as

Hsoln= H1+ H2+ H3. Hsolncan either be positive or negative depending on the

intermolecular forces.


8/10/2019 Chapter 4_3&4

34/93



Formation

Breaking attractive intermolecular forces is always

endothermic.

Forming attractive intermolecular forces is alwaysexothermic.


8/10/2019 Chapter 4_3&4

35/93



Formation

To determine whether Hsolnis positive or negative, we

consider the strengths of all solute-solute and solute-

solvent interactions: H1and H2are both positive.

H3is always negative.

It is possible to have either H3> (H1+ H2) or H3< (H1+

H2).


8/10/2019 Chapter 4_3&4

36/93

8/10/2019 Chapter 4_3&4

37/93



Formation

Examples:

NaOH added to water has Hsoln= -44.48 kJ/mol.

NH4NO3added to water has Hsoln= + 26.4 kJ/mol.

Rule: polar solvents dissolve polar solutes. Non-polar

solvents dissolve non-polar solutes

If Hsolnis too endothermic a solution will not form.

NaCl in gasoline: the ion-dipole forces are weak because

gasoline is non-polar. Therefore, the ion-dipole forces do not

compensate for the separation of ions.


8/10/2019 Chapter 4_3&4

38/93



Formation

Water in octane: water has strong H-bonds. There are no

attractive forces between water and octane to compensate for

the H-bonds.


8/10/2019 Chapter 4_3&4

39/93

Why solute dissolves in a solvent if attraction for its own

molecules are stronger than the solute-solvent attraction

Solution process governed by energy(exothermic/endothermic) and entropy (tendency

towards disorder)

In pure state, the solvent and solute possess a fair degree

of order (regular arrangement of molecules/ions/atoms)

Order is destroyed when the solute dissolves in the

solvent



8/10/2019 Chapter 4_3&4

40/93


Solution Formation, Spontaneity, and

Disorder

A spontaneous process occurs without outside

intervention.

When free energy of the system decreases (e.g. droppinga book and allowing it to fall to a lower potential energy),

the process is spontaneous.


8/10/2019 Chapter 4_3&4

41/93



Disorder

If the process leads to a greater state of disorder, then the

process is spontaneous.

Example: a mixture of CCl4and C6H14is less orderedthan the two separate liquids. Therefore, they

spontaneously mix even though Hsolnis very close to

zero.

There are solutions that form by physical processes and

those by chemical processes.


8/10/2019 Chapter 4_3&4

42/93



Disorder


8/10/2019 Chapter 4_3&4

43/93


Solution Formation and Chemical

Reactions

Example: a mixture of CCl4and C6H14is less ordered

Consider:

Ni(s) + 2HCl(aq) NiCl2(aq) + H2(g).

Note the chemical form of the substance being dissolved

has changed (Ni NiCl2).

When all the water is removed from the solution, no Ni isfound only NiCl26H2O. Therefore, Ni dissolution in

HCl is a chemical process.


8/10/2019 Chapter 4_3&4

44/93


Solution Formation and Chemical

Reactions

Example:

NaCl(s) + H2O (l) Na+(aq) + Cl-(aq).

When the water is removed from the solution, NaCl isfound. Therefore, NaCl dissolution is a physical

process.


S t t d S l ti d

8/10/2019 Chapter 4_3&4

45/93


Solutions can be characterized:

Saturated solution: contains maximum amount of a solute that

will dissolve in a given solvent at a specific temperature Unsaturated solution: contains less solute than it has the

capacity to dissolve

Supersaturated solution: a solution formed when more solute is

dissolved than in a saturated solution. Not stable and solute willcome out from supersaturated solution as crystals

Crystallization: process in which dissolved solute comes out of

solution and forms crystals.

Saturated Solutions and

Solubility

8/10/2019 Chapter 4_3&4

46/93


F t Aff ti

8/10/2019 Chapter 4_3&4

47/93


Solute-Solvent Interaction

Solubility is a measure of how much solute will dissolve in a

solvent at a specific temperature.

like dissolve like helpful in predicting solubility of substance in agiven solvent

Miscible liquids: mix in any proportions.

Immiscible liquids: do not mix.

Polar liquids tend to dissolve in polar solvents. Intermolecular forces are important: water and ethanol are miscible

because the broken hydrogen bonds in both pure liquids are re-

established in the mixture.

Factors Affecting

Solubility

F t Aff ti

8/10/2019 Chapter 4_3&4

48/93



The number of carbon atoms in a chain affect solubility:

the more C atoms the less soluble in water.

The number of -OH groups within a molecule increasessolubility in water.

The more polar bonds in the molecule, the better it

dissolves in a polar solvent.

The less polar the molecule the less it dissolves in a polar

solvent and the better is dissolves in a non-polar solvent.

Factors Affecting

Solubility

F t Aff ti

8/10/2019 Chapter 4_3&4

49/93



Factors Affecting

Solubility

Factors Affecting

8/10/2019 Chapter 4_3&4

50/93



Factors Affecting

Solubility

8/10/2019 Chapter 4_3&4

51/93

Example 3

Predict the relative solubilities in the following cases

Bromine (Br2) in benzene (= 0 D) and in water (= 1.87 D)

KCl in carbon tetrachloride (= 0 D) and in liquid ammonia(= 1.46 D)

Formaldehyde (H2C=O) in carbon disulfide (= 0 D) and in

water


Factors Affecting

8/10/2019 Chapter 4_3&4

52/93



Network solids do not dissolve because the strong

intermolecular forces in the solid are not re-established in

any solution. Example: SiO2

Factors Affecting

Solubility

Factors Affecting

8/10/2019 Chapter 4_3&4

53/93


Pressure Effects

Solubility of a gas in a liquid is a function of the pressure

of the gas.

The higher the pressure, the more molecules of gas areclose to the solvent and the greater the chance of a gas

molecule striking the surface and entering the solution.

Therefore, the higher the pressure, the greater the solubility.

The lower the pressure, the fewer molecules of gas are close to

the solvent and the lower the solubility.

Factors Affecting

Solubility

Factors Affecting

8/10/2019 Chapter 4_3&4

54/93


Pressure Effects

Factors Affecting

Solubility

F t Aff ti

8/10/2019 Chapter 4_3&4

55/93

Henrys law states that the solubility of a gas in a liquid

is proportional to the pressure of the gas over the

solution

Where c is the molar concentration (mol/L) of dissolved

gas, k is a constant with the units mol/L .atm, andPis

the pressure of the gas over the solution at equilibrium


Factors Affecting

Solubility

kPc

Factors Affecting

8/10/2019 Chapter 4_3&4

56/93


Pressure Effects

Carbonated beverages are bottled with a partial pressure

of CO2> 1 atm.

As the bottle is opened, the partial pressure of CO2decreases and the solubility of CO2decreases.

Therefore, bubbles of CO2escape from solution.

Factors Affecting

Solubility
http://d/Media_Portfolio/HenrysLaw/HenrysLawMovie.html

8/10/2019 Chapter 4_3&4

57/93

Example 4

The solubility of nitrogen gas at 25oC and 1 atm is

6.8x10-4mol/L. What is the concentration in molarity of

nitrogen dissolved in water under atmospheric

conditions? The partial pressure of nitrogen gas in the

atmosphere is 0.78 atm


Factors Affecting

8/10/2019 Chapter 4_3&4

58/93


Temperature Effects

Experience tells us that sugar dissolves better in warm

water than cold.

As temperature increases, solubility of solids generallyincreases.

Sometimes, solubility decreases as temperature increases

(e.g. Ce2

(SO4

)3

).

Factors Affecting

Solubility

8/10/2019 Chapter 4_3&4

59/93

F t Aff ti

8/10/2019 Chapter 4_3&4

60/93

Fractional crystallization: separation of a mixture of substances

into pure components on the basis of their different solubilities

Example: 90 g of KNO3is contaminated with 10g of NaCl.

To purify KNO3, dissolve mixture in 100ml of water at 60oC then

cool to 0oC.

Solubility KNO3and NaCl are 12.1g/100g H2O and 34.2g/100g

H2O

Therefore, 78 g of KNO3will crystallize out of the solution


Factors Affecting

Solubility

Factors Affecting

8/10/2019 Chapter 4_3&4

61/93


Temperature Effects

Experience tells us that carbonated beverages go flat as

they get warm.

Therefore, gases get less soluble as temperatureincreases.

Thermal pollution: if lakes get too warm, CO2and O2

become less soluble and are not available for plants or

animals.

Factors Affecting

Solubility

8/10/2019 Chapter 4_3&4

62/93

Ways of Expressing

8/10/2019 Chapter 4_3&4

63/93


Mass Percentage, ppm, and ppb

All methods involve quantifying amount of solute per

amount of solvent (or solution).

Generally amounts or measures are masses, moles orliters.

Qualitatively solutions are dilute or concentrated.

Definitions:

Ways of Expressing

Concentration

100solutionofmasstotal

solutionincomponentofmasscomponentof%mass

Ways of Expressing

8/10/2019 Chapter 4_3&4

64/93



Parts per million (ppm) can be expressed as 1 mg ofsolute per kilogram of solution.

If the density of the solution is 1g/mL, then 1 ppm = 1 mg

solute per liter of solution.

Parts per billion (ppb) are 1 g of solute per kilogram of

solution.

Ways of Expressing

Concentration


solutionincomponentofmasscomponentofppm

Ways of Expressing

8/10/2019 Chapter 4_3&4

65/93



Mole Fraction, Molarity, and Molality

Recall mass can be converted to moles using the molar

mass.

Ways of Expressing

Concentration


solutionincomponentofmasscomponentofppb

solutionofmolestotal

solutionincomponentofmolescomponentoffractionMole

solutionofliters

solutemolesMolarity

Ways of Expressing

8/10/2019 Chapter 4_3&4

66/93


Mole Fraction, Molarity, and Molality

We define

Converting between molarity (M) and molality (m)

requires density.

Ways of Expressing

Concentration

solventofkg

solutemolesMolality, m

8/10/2019 Chapter 4_3&4

67/93

8/10/2019 Chapter 4_3&4

68/93

Example 5

The density of a 2.45M aqueous solution of methanol

(CH3OH) is 0.976 g/ml. What is the molality of the

solution? Molar mass of methanol is 32.04g/mol


Ways of Expressing

8/10/2019 Chapter 4_3&4

69/93

The choice of concentration unit is based on the purpose

of the experiment

Advantage of molarity is easier to measure the volume ofsolution than to weigh the solvent. Thus molrity is

usually preferred.

However, molality is independent of temperature.

Volume of solution increases with increasing T so that asolution that is 1.0M at 25oC may become 0.97M at 45oC

Can affect accuracy of experiment


Ways of Expressing

Concentration

C lli ti P ti

8/10/2019 Chapter 4_3&4

70/93


Colligative properties are properties that depend only on

the number of solute particles in solution and not on the

nature of the solute particles. depend on number of solute particles present.

Vapor-pressure lowering, boiling point elevation, freezing

point depression and osmotic pressure

Colligative Properties

8/10/2019 Chapter 4_3&4

71/93

Lowering Vapor Pressure

If a solute is nonvolatile the vapour pressure of its solution is

always less than that of the pure solvent.

Thus the relationship between solution and solvent vapor pressure

depends on the concentration of the solute in the solution

Non-volatile solvents reduce the ability of the surface solvent

molecules to escape the liquid.

Therefore, vapor pressure is lowered.

The amount of vapor pressure lowering depends on the amount of

solute.



C lli ti P ti

8/10/2019 Chapter 4_3&4

72/93




C lli ti P ti

8/10/2019 Chapter 4_3&4

73/93



Raoults Law: vapor pressure of a solvent over a solution,

PAis given by the vapor pressure of the pure solvent, Po

A,

times the mole fraction of the solvent in the solution, XA

In a solution containing only one solute, X1= 1-X2, where

X2 is the mole fraction of the solute.


AAA PP

ABAAA PPPP ?

C lli ti P ti

8/10/2019 Chapter 4_3&4

74/93



Ideal solution: one that obeys Raoults law.

Raoults law breaks down when the solvent-solvent and

solute-solute intermolecular forces are greater thansolute-solvent intermolecular forces.

If both components of a solution are volatile(measureable

vapor pressure) the vapor pressure of the solution is the

sum of the individual partial pressures

PT= PA+ PB


8/10/2019 Chapter 4_3&4

75/93

Example 6

Calculate the vapor pressure of a solution made by

dissolving 218 g of glucose (molar mass = 180.2 g/mol)

in 460ml of water at 30oC. What is the vapor pressure

lowering? The vapor pressure of pure water at 30oC is

31.82 mmHg.Assume the density of the solution is

1.00g/ml


8/10/2019 Chapter 4_3&4

76/93

Boiling-Point Elevation

Boiling point is the T at which its vapor pressure equals

the external atmospheric pressure Non-volatile solute lowers the vapor pressure. Therefore,

boiling point of the solution must be affected.



8/10/2019 Chapter 4_3&4

77/93


8/10/2019 Chapter 4_3&4

78/93


Boiling-Point Elevation

At 1 atm (normal boiling point of pure liquid) there is a

lower vapor pressure of the solution. Therefore, a higher

temperature is required to teach a vapor pressure of 1 atmfor the solution (Tb).

Molal boiling-point-elevation constant,Kb, (oC/m)

expresses how much Tbchanges with molality, m:


mKT bb


8/10/2019 Chapter 4_3&4

79/93


Freezing Point Depression

When a solution freezes, almost pure solvent is formed

first.

Therefore, the sublimation curve for the pure solvent is thesame as for the solution.

Therefore, the triple point occurs at a lower temperature

because of the lower vapor pressure for the solution.



8/10/2019 Chapter 4_3&4

80/93



The melting-point (freezing-point) curve is a vertical line

from the triple point.

The solution freezes at a lower temperature (Tf) than thepure solvent.

Decrease in freezing point (Tf) is directly proportional

to molality (Kfis the molal freezing-point-depression

constant):


mKT ff

8/10/2019 Chapter 4_3&4

81/93

Freezing involves transition from disordered to ordered

state

Therefore energy must be removed from system Solution has greater disorder than pure solvent, more

energy needs to be removed from it to create order than

pure solvent

Therefore the solution has a lower freezing point than itssolvent



8/10/2019 Chapter 4_3&4

82/93

Example 7

Ethylene glycol is a common automobile antifreeze. It is

water soluble and fairly nonvolatile (b.p 197 oC). Calculate

the freezing point of a solution containing 651 g of this

substance in 2505 g of water. Would you keep this

substance in your car radiator during the summer? The

molar mass of ethylene glycol is 62.01 g/mol.

Kf = 1.86o

C/m and Kb = 0.52o

C/m



8/10/2019 Chapter 4_3&4

83/93




8/10/2019 Chapter 4_3&4

84/93


8/10/2019 Chapter 4_3&4

85/93


Osmosis

Semipermeable membrane: permits passage of some

components of a solution. Example: cell membranes and

cellophane. Osmosis: the movement of a solvent from low solute

concentration to high solute concentration.

There is movement in both directions across a

semipermeable membrane.

As solvent moves across the membrane, the fluid levels

in the arms becomes uneven.



8/10/2019 Chapter 4_3&4

86/93


Osmosis

Eventually thepressure difference between the arms

stops osmosis.



8/10/2019 Chapter 4_3&4

87/93


Osmosis

Osmotic pressure, , is the pressure required to stop

osmosis:

Isotonic solutions: two solutions with the same

separated by a semipermeable membrane.


MRT

RTV

n

nRTV


8/10/2019 Chapter 4_3&4

88/93


Osmosis

Hypotonic solutions: a solution of lower than a

hypertonic solution.

Osmosis is spontaneous. Red blood cells are surrounded by semipermeable

membranes.



8/10/2019 Chapter 4_3&4

89/93


Osmosis

Crenation:

red blood cells placed in hypertonic solution (relative to

intracellular solution);

there is a lower solute concentration in the cell than the

surrounding tissue;

osmosis occurs and water passes through the membrane out of

the cell. The cell shrivels up.



8/10/2019 Chapter 4_3&4

90/93


Osmosis


8/10/2019 Chapter 4_3&4

91/93

8/10/2019 Chapter 4_3&4

92/93


8/10/2019 Chapter 4_3&4

93/93

Osmosis

Active transport is the movement of nutrients and waste

material through a biological system.

Active transport is not spontaneous.


Documents

Chapter 4_3&4