Solution

1
Solution

• Homogeneous mixture in a single phase.

2
Classification of Matter
Also called solutions
Also called suspensions
3
Solvent

• Substance you have the most of. Substance that
  retains its phase. Dispersing medium.

4
Solute

• Substance you have the least of. Substance that
  dissolves.

5
Dilute Solution

• Relatively small amount of solute.

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Concentrated Solution

• Relatively large amount of solute.

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Aqueous Solution

• Water is the solvent.

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NaCl(aq)

• Solution of NaCl dissolved in water!

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Soluble

• Capable of being dissolved.

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Solubility

• Maximum amount of 1 substance that will dissolve
  in a given amount of another substance.

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Factors that influence solubility

• Temperature for all systems pressure for
  systems involving gases.

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Factors that influence the rate of dissolving.

• Temperature
• Stirring or agitation
• Surface Area of solute
• Amount of solute already present

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What kind of change is dissolving?

• Physical change

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How does a chemist represent the dissolving of a
covalently bonded substance?

• C6H12O6(s) ? C6H12O6(aq)

15
How does a chemist represent the dissolving of an
ionically bonded substance?

• NaCl(s) ? Na1 (aq) Cl-1(aq)

16
What happens to an ionic substance when it
dissolves?

• It separates into ions.

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What is the equation for the dissolving of CaBr2?

• CaBr2(s) ? Ca2(aq) 2Br-1(aq)

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Molecule-Ion Attraction

• Interaction between water molecules and ions in
  solution.

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What kind of molecule is H2O?

• Polar the O end is a bit negative the Hs are
  a bit positive.

20
Is the orange ion positive or negative how do
you know?
21
Is the orange ion positive or negative how do
you know?
22
Units of Solubility?

• Grams of solute per 100 grams of solvent

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What happens to the solubility of all gases as
the temperature increases?

• The solubility of gases ? as the temperature ?

24
What happens to the solubility of most solids as
the temperature increases?

• The solubility of most solids ? as the
  temperature ?.

25
What do you need to conduct electricity?

• Mobile charged particles!

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Electrolyte?

• A substance that dissolves in water to produce a
  solution that conducts an electric current!

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Nonelectrolyte?

• A substance that dissolves in water to produce a
  solution that does not conduct an electric
  current!

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Saturated solution

• Contains the maximum amount of dissolved solute
  at that temperature.

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Supersaturated solution

• Contains more than the maximum amount of
  dissolved solute at that temperature.

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Unsaturated solution

• Contains less than the maximum amount of
  dissolved solute at that temperature.

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Precipitation

• The opposite of dissolving. A solid comes out of
  solution.

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Dynamic Equilibrium

• Term used to describe a saturated solution.
  Precipitation dissolving are ocurring at the
  same rates. No net change.

33
How do you test a solution for saturation?

• Throw a crystal of the solute into the solution
  observe what happens.

34
What are 3 possible outcomes of the saturation
test?

• Crystal dissolves Soln was unsaturated.
• No change in crystal Soln was saturated.
• Crystal gets larger Soln was supersaturated.

35
What are 3 regions of a solubility curve?

• On the trace saturated solution.
• Above the trace supersaturated solution.
• Below the trace unsaturated solution.

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Concentration

• A number that describes how much solute compared
  to how much solution or how much solvent.

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Percent

• Part over Whole X 100

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Molarity (M)

• Molarity moles solute

Liters of solution
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No. of Grams
?by F.M.
X formula mass
No. of Moles
X 22.4 L/mol
X 6.02 X 1023

• by
• 6.02 X 1023

? by 22.4
No. of Particles
No. of Liters
Mole Map
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Parts per Million (PPM)

• PPM grams solute X 1000000

grams solution
41
How much KCl will dissolve in 300 grams of water
at 50?C? Use the graph to set up a proportion.
Problem
42 g KCl X g KCl
100 g H2O
300 g H2O
X 126 g KCl
42
88 g KNO3 in 100 g H2O at 50?C.
20 g KNO3 in 100 g H2O at 10?C.
88 g 20 g 68 g KNO3 precipitates.
50? to 10? - How much KNO3 precipitates?
43
Measuring Heat of Solution
Water is the environment!
If Temperature of H2O ?, dissolving was
exothermic. If temperature of H2O ?, dissolving
was endothermic.
source
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Factors affecting Solubility

• Temperature
• Pressure
• Nature of the Solvent Solute

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Nature?

• Ionic
• Polar Covalent
• Nonpolar Covalent
• Like Dissolves Like

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MolarityC X VolumeC MolarityD X VolumeD
MC X VC MD X VD
Dilution Problems
48
Colligative Property

• Depends on the concentration of the solute, NOT
  on the nature of the solute. Does not matter if
  ions or neutral particles are in solution.

49
What are 2 colligative properties?

• Freezing Point Depression Boiling Point
  Elevation

50
Which solution has the most dissolved particles?

• 1 mole of C6H12O6 in 1 Liter H2O
• 1 mole of NaCl in 1 Liter H2O
• 1 mole of CaBr2 in 1 Liter H2O