Solutions are:

1

• Solutions are
• Homogeneous
• Usually clear (liquids)
• Can vary in concentration
• Can not separate by filtration
• Will not separate by standing
• Made up of at least two different substances
• Can separate using a physical change

2
Solutions samples containing dissolved
substances that can be solid, liquid or
gas. Solvent the dissolving medium. The thing
that the stuff dissolves in. Solute the
dissolving particles. The thing that
dissolves. Aqueous solution a solution that
has water as the solvent. An aqueous salt
solution water is the solvent, salt is the
solute
3

• Factors affecting solvation (how fast things
  dissolve)
• Increasing the heat or temperature
• Stirring or agitation
• Increasing the surface area of the particles or
  making the particles smaller

4

• One way to describe compounds
• Polar (ionic) made up of ions made up of
  metals and nonmetals positive and negative ions
• Nonpolar (covalent) made up of nonmetals, no
  charged particles
• Likes Dissolve Likes
• Polar solutes dissolve in polar solvents
• Nonpolar solutes dissolve in Nonpolar solvents

5
Miscible two liquids are miscible if they will
dissolve in each other Immiscible two liquids
are immiscible if two liquids will not dissolve
in each other. Polar/polar and non
polar/nonpolar solutions are miscible.
Polar/nonpolar solutions are immiscible. Oil/wate
r immiscible Water/ food coloring - miscible
6
Solubility the amount of substance that can
dissolve in a given amount of solvent at a given
temperature. Saturated Solution contains the
maximum amount of solute for a given temperature
and a given amount of solvent. Unsaturated
Solution contains less than the maximum amount
of solute. Supersaturated Solution contains
more solute than it can theoretically hold at a
given temperature. It is an unstable solution,
and will very easily turn into a solid.
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In general, the solubility of solids in liquids
increases as the temperature of the solution
increases. The solubility of gases in liquids
decreases as the temperature of the solution
increases. That explains the shape of the
solubility graph most lines curve up. The lines
that curve down are gases.
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Concentration of a Solution How much solute is
dissolved in a given quantity of solvent. The
most common unit of concentration in chemistry is
MOLARITY. Molarity (mole of solute/liters of
solution) M mol/liters A 4.00 M solution
contains 4.00 moles of solute for every liter of
solution (2.00 moles for every 0.500 liters, 8.00
moles for every 2.00 liters, )
9

• How many moles of NaCl are needed to make 150. ml
  of 1.25 M solution?
• Change from ml ? liters
• M x L moles
• (1.25 M) x (0.150 L) 0.188 mol NaCl

10
Moles Molarity Liters
11

1. What volume of solution is needed to turn 17.3
   grams of NaNO3 into a 1.35 M NaNO3 solution?
2. How many grams of NaCl are needed to make 145 ml
   of 0.750 M NaCl?
3. What is the molarity of 243 grams of LiNO3
   dissolved to make 1458 ml of solution?
4. What is the molarity of a solution when 13.5
   grams of NaCl is dissolved to make 125 ml of
   solution?

12

• 17.3 g NaNO3 1 mol NaNO3 0.2035 mol NaNO3
• 85.0 g NaNO3
• (0.2035 mol NaNO3/1.35 M NaNO3) 0.151 l
  solution
• 0.145 l soln x 0.750 M NaCl 0.10875 mol NaCl
• 0.10875 mol NaCl 58.5 g NaCl 6.36 g NaCl
• 1 mol NaCl
• 3. 243 g LiNO3 1 mol LiNO3 3.526 mol LiNO3
• 68.9 g LiNO3
• (3.526 mol LiNO3/1.458 l soln) 2.42 M LiNO3
• 4. 13.5 g NaCl 1 mol NaCl 0.23076 mol NaCl
• 58.5 g NaCl
• (0.23076 mol NaCl/0.125 l soln) 1.85 M NaCl

13
When diluting a solution, the amount of solute
remains constant, only the volume of the solution
is changed. A stock solution is an essentially
unlimited amount of a solution at a given
concentration. M1V1 M2V2 M1 concentration of
solution (initial) M2 concentration of solution
(final) V1 volume of solution (initial) V2
volume of solution (final)
14
It is very important when working dilution
problems to make sure all of the information is
properly labeled get the right concentration
paired with the right volume. There are three
different volumes in a dilution problem V1
starting volume V2 ending volume V2-V1 amount
of solvent added in the dilution.
15

1. What is the starting concentration of NaCl if
   14.6 ml of solution is diluted to make 263.2 ml
   of 0.137 M NaCl?
2. What is the final concentration of the solution
   if 17.5 ml of 2.61 M NaOH is diluted to make
   250.0 ml of solution?
3. How do you make 125 ml of 0.135 M HCl from 3.62 M
   HCl?

16

• M1V1 M2V2 M1(14.6) (0.137)(263.2)
• M1 (0.137 x 263.2)/14.6 2.47 M NaCl
• 2. M1V1 M2V2 (17.5)(2.61) (250.0)M2
• M2 (17.5 x 2.61)/250.0 0.183 M NaOH
• 3. M1V1 M2V2 (0.135)(125) (3.62)V
• V2 (0.135 x 125)/3.62
• 4.66 ml of 3.62 M HCl
• 125 ml 4.66 ml 120. ml of water

17

• Colligative Properties
• Properties of a solution that depend on the
  number of particles dissolved in the solvent.
• Boiling Point (BP)
• Freezing Point (FP)
• Vapor Pressure (VP)
• Osmosis

18

• As the number of particles in the solution
  increases
• The BP increases
• The FP decreases
• The VP decreases
• The solvent always flows from the solution with
  the smaller concentration towards the solution
  with the higher concentration.

19
When talking about colligative properties, it is
convenient to talk about osmolarity (osmol). The
solution with the highest osmolarity will have
the most number of particles in solution. Osmol
( ions/molc) x Molarity For ionic compounds,
count the total number of ions in a molecule. For
a covalent compound, the number of ions per
molecule will be 1.
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Osmolarity
solution concentration of ions osmol
1.75 M NaCl
0.650 M Na3PO4
2.25 M Mg(OH)2
1.50 M HC2H3O2
1.25 M C6H12O6
21
Osmolarity
solution concentration of ions osmol
1.75 M NaCl 1.75 M 2 3.50 osmol
0.650 M Na3PO4 0.650 M 4 2.60 osmol
2.25 M Mg(OH)2 2.25 M 3 6.75 osmol
1.50 M HC2H3O2 1.50 M 2 3.00 osmol
1.25 M C6H12O6 1.25 M 1 1.25 osmol