states of matter lesson 4.9 chemistry 2...
TRANSCRIPT
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States of Matter
Lesson 4.9
CHEMISTRY 2
HONORS
Jeff Venables
Northwestern High School
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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.
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• Eventually the pressure difference between the arms
stops osmosis.
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• Osmotic pressure, , is the pressure required to stop
osmosis:
• Isotonic solutions: two solutions with the same
separated by a semipermeable membrane.
iMRT
RTV
ni
inRTV
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• Hypotonic solutions: a solution of lower than a
hypertonic solution.
• Osmosis is spontaneous.
• Red blood cells are surrounded by semipermeable
membranes.
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• 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.
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Osmosis
Colligative Properties
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• Hemolysis:
– red blood cells placed in a hypotonic solution;
– there is a higher solute concentration in the cell;
– osmosis occurs and water moves into the cell.
– The cell bursts.
• To prevent crenation or hemolysis, IV (intravenous)
solutions must be isotonic.
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– Cucumber placed in NaCl solution loses water to shrivel up and
become a pickle.
– Limp carrot placed in water becomes firm because water enters
via osmosis.
– Salty food causes retention of water and swelling of tissues
(edema).
– Water moves into plants through osmosis.
– Salt added to meat or sugar to fruit prevents bacterial infection
(a bacterium placed on the salt will lose water through osmosis
and die).
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• Active transport is the movement of nutrients and waste
material through a biological system.
• Active transport is not spontaneous.
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Example
What is the osmotic pressure of a solution of 7.95 g of
NaCl in 50.0 mL of an aqueous solution at 75˚C?
155 atm
118,000 mm Hg
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One major application of vapor pressure lowering and
colligative properties is in molar mass problems
1. An aqueous solution contains 1.00 g/L of a detergent.
The osmotic pressure of this solution at 25˚C is 17.8 torr.
What is the molar mass of the detergent?
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2. 1.008 g of a compound was dissolved in
11.38 mL of benzene (d=0.879 g/mL) and
the solution froze at 4.37˚C. What is the
molar mass of the compound?
Tf(benzene) = 5.48˚C
Kf(benzene) = 5.12˚C/molal
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• Typical hydrophilic groups are polar (containing C-O, O-
H, N-H bonds) or charged.
• Hydrophobic colloids need to be stabilized in water.
• Adsorption: when something sticks to a surface we say
that it is adsorbed.
• If ions are adsorbed onto the surface of a colloid, the
colloids appears hydrophilic and is stabilized in water.
• Consider a small drop of oil in water.
• Add to the water sodium stearate.
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• Sodium stearate has a long hydrophobic tail
(CH3(CH2)16-) and a small hydrophobic head (-CO2-Na+).
• The hydrophobic tail can be absorbed into the oil drop,
leaving the hydrophilic head on the surface.
• The hydrophilic heads then interact with the water and
the oil drop is stabilized in water.
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Colloids
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• Most dirt stains on people and clothing are oil-based.
Soaps are molecules with long hydrophobic tails and
hydrophilic heads that remove dirt by stabilizing the
colloid in water.
• Bile excretes substances like sodium stereate that forms
an emulsion with fats in our small intestine.
• Emulsifying agents help form an emulsion.