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Chapter 7: Solutions and Colloids
Suggested Problems:
4, 16, 20-28, 46, 48, 52-56, 64, 66,
72, 74, 92
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What is a Solution?• A solution is a homogeneous mixture comprised
of one or more solutes dispersed at an atomic, ionic or molecular level uniformly throughout a medium called the solvent
• Solvent: Is the most abundant substance in a solution
• Solute: Are all of the other components that comprise the solution– Notice I did not say dissolved in the solvent
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Importance of Solutions
• Most medicines are given as solutions• Most chemistry occurs in solution, rather
than in a pure state• Focus of this chapter
– Solution concentrations– Properties of solutions
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Describing Solutes• Solubility: The maximum amount of solute than
can be dissolved in a specific amount of solvent under specific conditions of temperature and pressure
• Soluble Substance: is a substance that dissolves to a significant extent in the solvent
• Insoluble Substance: A substance that does not dissolve to a significant extent in a solvent
• Immiscible: A term used to describe liquids that are insoluble in each other
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Describing Solutions
• Saturated: A solution that has the maximum amount of solute dissolved in a given amount of solvent
• Super Saturated: A solution that has a solute dissolved at a greater amount than the solubility of that solute
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Process of Solution Formation
• Ionic Solutes: Need Polar solvent • IMF’s between solute/solvent > solute/solute
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Process of Solution Formation
• Molecular Solutes: Need proper solventPolar if Polar solute Non-polar if Non-polar solute
Dissolved gases: O2, N2
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Solution Concentrations: Percent Definitions
100%solution of mL
solute grams %(w/v)
100% olumesolution v
volumesolute %(v/v)
100%masssolution
mass solute %(w/w)
100 x total
part %
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solvent mass solute mass masssolution
100% masssolution
mass solute (w/w) %
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• Beware of question wording– If solute is added to enough solvent to make a
solution of a certain volume• This volume is the volume of solution
– If problem states a volume of solute is added to a volume of solvent• Then you need to add the two volumes to get
volume of solution
solvent of volume solute of volumesolution of volume
100% solution of volume
solute of volume (v/v) %
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• Remember that percentages are best used if based out of a total of 100– This is true whether it be mass or volume
• For example a 5 % (w/v) solution– This is the same as saying:
100% solution of mL
solute of mass (w/v) %
solution mL 100
solute grams 5
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Percent Example
• What is the percent (w/v) concentration of a solution prepared by dissolving 45 grams of glucose in enough water to give 300.0 mL of solution?
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Percent Example
• Normal saline is 0.89% (w/v) NaCl in water. What volume of normal saline is required to deliver 45 grams of NaCl?
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Percent Example
• D-5-W is 5.0% (w/v) dextrose in water. How many grams of dextrose are contained in 1500.0 mL D-5-W?
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Solution Concentrations: Molarity
• Useful unit in dealing with chemicals in solution
solution L
solute molesM
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Molarity Example
• What is the molarity of a solution prepared by dissolving 58.5 grams of Cu(NO3)2 in enough water to give a total volume of 500.0 mL?
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Molarity Example
• How many moles of HCl are contained in 750.0 mL of a 2.5 M solution?
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Titration• A titration is a chemical analysis
that uses volume and molarity• In simple acid-base titrations, you
can use this equation*:
MacidVacid= MbaseVbase
• *must be a 1:1 stoichiometric reaction or else this equation does not work
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Titration Example• A 25 mL sample of vinegar (which
contains acetic acid) is titrated with 0.100 M NaOH. If 6.75 mL of NaOH are required, what is the molarity of the acetic acid in vinegar?
25 mL of vinegar
0.100 M NaOH
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Dilutions
• Many reagents and medicines are available as “stock” solutions that must be diluted prior to use
• In any dilution, you can always use this equation:
C1V1=C2V2
C = concentration V = volume
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Example
• If 8.33 mL of 12 M HCl are diluted with water to give a new volume of 1000.0 mL, what is the molarity of the resulting solution?
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Example
• How many mL of 5.0% NaCl solution are needed to prepare 5.0 Liters of normal saline?
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Electrolytes
• Strong electrolytes dissolve 100% in water to afford solutions that conduct electricity
– Soluble ionic compounds– Strong acids (HCl, H2SO4, HNO3)
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Weak Electrolytes
• Weak electrolytes dissociate less than 100% into ions when dissolved in water and produce solutions with varying ability to conduct electricity
– Weak Acids (H3PO4, HF, H2S)
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Non-Electrolytes
• When molecular compounds (covalently bonded compounds) dissolve in water, no ions are produced, so the solution does not conduct electricity
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Colligative Properties of Solutions
• Colligative properties are those properties that depend on the concentration of the solute, not the identity of the solute
• Examples:– Electrical Conductivity– Vapor Pressure– Boiling Point– Freezing Point
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Freezing Point Depression
• The freezing point of a solution goes down as the concentration of solute increase
• Should use molality
solution ofMolarity M
solventgiven afor constant K
moles ofnumber n
solution andsolvent pure ofpoint freezingin difference t
MnKt
f
f
ff
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Freezing Point Depression Example
• Calculate the freezing point of a solution comprised of 171 g of C12H22O11 dissolved in enough water to have a final volume of 1.00 L.
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Boiling Point Elevation
• The boiling point of a solution increases as the concentration of solute increases
• Should use molalitysolution ofMolarity M
solventgiven afor constant K
moles ofnumber n
solution andsolvent pure ofpoint boilingin difference t
MnKt
b
f
bb
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Boiling Point Elevation Example
• If 13.4 g of NH4Cl is dissolved in water to form a 500.0 mL solution, what is the new boiling point of this solution, assuming that water boils at 100 oC?
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Osmotic Pressure
• The osmotic pressure of a solution increases as the concentration of solute increases
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Diffusion• Diffusion is the movement of a substance
from an area of high concentration to an area of low concentration
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Osmosis• Osmosis is diffusion of water through a
semipermeable membrane• Solute particles are too big (or too polar) to
make it across the membrane• This is how water gets moved around cells
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Hydrostatic Pressure
– As the water level rises so does the hydrostatic pressure against the membrane, until a pressure is reached that causes the net movement of water to equilibrate and the volume levels of the two sides become constant
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Osmotic Pressure• Osmotic Pressure () is the hydrostatic pressure required
to stop the flow of a solvent from low concentration to high concentration
=nMRT
n = moles of particles obtained when one mole of solute dissolvesM= molarity of the solutionR = is the ideal gas constantT = the temperature in KelvinnM = Osmolarity, a term used in biology and medicine
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Tonicity
• Isotonic solutions have equal concentrations of solute particles
• A hypertonic solution has a greater concentration of solute
• A hypotonic solution is a lower concentration of solute
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Example
Na+
H2OH2O
Cl-
Hypertonic solutionLess water
Na+
H2OH2O
Cl-
Hypotonic solutionMore water
Direction of osmosis
SPMWhich direction will the water diffuse?
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Question• What will happen to a red blood cell when
it is placed into pure water? Cells are isotonic with normal saline (0.89% NaCl). Hint: think about the flow of H2O.
• Hemolysis
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Question
• What will happen to a red blood cell when it is placed into 10% aqueous sodium chloride? Cells are isotonic with normal saline (0.89% NaCl)