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Solutions

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In fact, All ionic compounds are. polar. Jodi Grack; Wayzata High School ... Solvation occurs when the attractive forces between the solvent and solute particles is ... – PowerPoint PPT presentation

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Title: Solutions


1
Chapter 15
  • Solutions

2
  • MATTER
  • Mixtures Pure Substances
  • Homogeneous Elements
  • Heterogeneous Compounds

3
Solutions
  • Terminology
  • Solute
  • Solvent
  • Soluble
  • Insoluble -

the substance that gets dissolved
the substance that does the dissolving
able to be dissolved
cant be dissolved
Miscible/Immiscible
4
Why does something dissolve/not dissolve?
  • Rule of Thumb
  • Nonpolar Substances
  • Polar Substances

like dissolves like
i.e. polar solvents dissolve polar solutes
nonpolar nonpolar
5
Polar vs. Nonpolar
polar
Water is __________
6
polar/nonpolar?
7
Polar vs. Nonpolar
polar
Sucrose is __________
8
Polar vs. Nonpolar
polar
Sucrose is __________
9
Polar vs. Nonpolar
polar
Sucrose is __________
10
Salt is __________
polar
In fact, All ionic compounds are ________
polar
11
Methanol and other alcohols are __________
polar
12
Hydro-carbons are ______
nonpolar
13
Hydro-carbons are ______
nonpolar
14
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15
Why does something dissolve/not dissolve?
  • Rule of Thumb
  • Nonpolar Substances
  • Polar Substances

like dissolves like
i.e. polar solvents dissolve polar solutes
nonpolar nonpolar
Hydrocarbons oils, fats, grease etc.
Ionic compounds
Water, sugar, alcohol (anything w/ -OH groups)
16
Solvation
  • The solvent particles pull the solute particles
    apart and surround them.

Solvation Video
Solvation - Ionic simulation.jnlp
Solvation - molecular.notebook
Solvation occurs when the attractive forces
between the solvent and solute particles is
________ than the attractive forces holding the
solute particles together.
17
(No Transcript)
18
Dissolving Equations - Revisited
  • Write the dissolving equation for each
  • Sodium chloride
  • NaCl(s) ? Na(aq) Cl-(aq)
  • Silver sulfide
  • Ag2S(s) ? 2 Ag(aq) S2-(aq)
  • Sucrose (C12H22O11)
  • C12H22O11 (s) ? C12H22O11 (aq)

19
3 Factors affecting rate of solvation
  • Temperature
  • Increases movement of particles -gt mixes faster
  • Agitation
  • Allows particles to come into contact at a faster
    rate -gt mixes faster
  • Surface Area
  • Increases the contact area, thus allows
    particles to come into contact faster -gt mixes
    faster

20
Heats of Solution
  • Energy Absorbed
  • Energy Released

21
Solubility
  • the maximum concentration of solute that will
    dissolve in a given amt. solvent (_at_ given temp.,
    pressure)
  • Saturated
  • Unsaturated -

Contains the maximum amount of solute
Contains less than the maximum amount of solute
22
Solubility
  • the maximum amount of solute that will dissolve
    in a given amt. solvent (_at_ given temp.,
    pressure)

23
Factors Affecting Solubility
1) Nature of solute solvent
like dissolves like
24
Factors Affecting Solubility
2) Temperature
  • NaCl(s) ? Na (aq) Cl-(aq)

Increasing temperature favors the endothermic
process
Most solids dissolve ____________ solubility
______ as temp ?
Figure 11.6 Zumdahl Chemistry 7th Edition
25
Temperature Solubility
  • CO2 (g) ? CO2 (aq)

All gases dissolve ____________ solubility ______
as temp ?
Figure 11.7 Zumdahl Chemistry 7th Edition
26
Factors Affecting Solubility
Supersaturated -
A solution that contains more than the maximum
concentration of solute
http//genchem.chem.wisc.edu/demonstrations/gen_ch
em_pages/11solutionspage/crystallization_from_supe
r.htm link to supersaturated demo
27
Factors Affecting Solubility
3) Pressure Henrys Law
At a given temp, the solubility (S) of a gas is
directly proportional to the pressure (P) of the
gas above the liquid.
28
Factors Affecting Solubility
Henrys Law
Ex. If the solubility of a gas is 0.66 g/L at
10.0 atm, what is the pressure on a 1.0-L sample
that contains 1.5 g gas?
29
How would the solubility be affected by
increasing temp. for following
  • Heat NaCl (s) ? Na (aq) Cl- (aq)
  • Ce2(SO4)3 (s) ? 2 Ce3 (aq) 3 SO42-(aq)
    heat
  • H2S (g) ? H2S (aq)

30
How would the solubility be affected by
increasing pressure for following
  • Heat NaCl (s) ? Na (aq) Cl- (aq)
  • Ce2(SO4)3 (s) ? 2 Ce3 (aq) 3 SO42-(aq)
    heat
  • H2S (g) ? H2S (aq)

31
How would the solubility be affected by agitating
mixtures of each of the following
  • Heat NaCl (s) ? Na (aq) Cl- (aq)
  • Ce2(SO4)3 (s) ? 2 Ce3 (aq) 3 SO42-(aq)
    heat
  • H2S (g) ? H2S (aq)

32
Expressing Concentration
Concentration - how much solute is dissolved in a
given amount of solvent or solution possibilities
Molarity (M)
33
Expressing Concentration
1) 24.5 g NaCl is dissolved in a total volume of
2.0 L. What is the concentration (molarity) of
the NaCl solution?
34
Expressing Concentration
  • 2) You have 5.0 L of a 2.5 M soln of NaOH.
  • How many moles of NaOH are present?
  • How many grams of NaOH are present?

35
Expressing Concentration
3) You need 27.3 g of NaCl. All you have is a
0.15 M solution of NaCl. How many milliliters of
solution will you need?
36
Expressing Concentration
4) How could you prepare 250. mL of a 0.10 M
solution of copper (II) nitrate, Cu(NO3)2?
37
Dilution Problems
When diluting a concentrated solution, the key
to solving for the new concentration is that the
number of moles of solute (n) does not change.
38
Dilution Problems
1) How many milliliters of 1.00 M Cu(NO3)2
solution are needed to prepare 250. mL of a 0.100
M solution of Cu(NO3)2.
39
Dilution Problems
1) How many milliliters of 12.0 M HCl solution
are needed to prepare 10.0 L of a 0.500 M
solution of HCl?
40
Dilution Problems
2) How many milliliters of an 18.0 M H2SO4
solution are needed to prepare 3.0 L of a 0.200 M
solution?
41
Dilution Problems
3) How many milliliters of 1.50 M HCl must be
added to appropriate amount of H2O to make 25 mL
of 0.500 M HCl?
42
Dilution Problems
4) What is the concentration of a solution made
by diluting 50.0 mL of a 3.00 M solution of HCl
to 500. mL?
43
Predicting PrecipitatesRevisited
Write the total and net ionic equation for when
the following solutions are mixed. 1) potassium
chromate lead (II) nitrate
44
Predicting PrecipitatesRevisited
Write the total and net ionic equation for when
the following solutions are mixed. 2) silver
nitrate iron (III) chloride
45
Molarity 3-step Mole Method
CuCl2 (aq) 2 AgNO3 (aq) ? 2 AgCl (s)
Cu(NO3)2 (aq)
2) 125 mL of a silver nitrate solution reacts
with enough copper (II) chloride to produce 0.300
g of AgCl. What is the molarity of the initial
silver nitrate solution?
46
Molarity 3-step Mole Method
CuCl2 (aq) 2 AgNO3 (aq) ? 2 AgCl ( )
Cu(NO3)2 ( )
1) How many milliliters of 0.15 M copper (II)
chloride are needed to react with silver nitrate
to produce 50.0 g of solid silver chloride?
47
Ch. 15 Test Overview
  • 14 mult. Choice (2pt.)
  • 8 pt. free response
  • 36 total points
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