Solutions
Water
Water is a bent molecule and is
polar, and the molecules are held
together through hydrogen
bonding.
Properties of Water
1.
2.
3.
High Surface Tension – acts like a “thin” skin on the
surface.
Low vapor pressure & High Boiling Point – needs
a lot of energy/heat to make it evaporate or boil
High Specific Heat – takes a lot of heat to change its
temperature
WATER! It’s good for! You! I think!
Washcloth
Can you cry in space?
Suspensions
(large particles)
filtered out with filter paper, and
They can be ____________
they will _________
_____
settle
out by gravity.
scatter
These particles will also ______________
light
shined through the mixture so the beam can be seen.
vinegar and oil salad dressing
Colloids

(small particles)
filtered
They cannot be ___________
nor do
they__________
_____
settle
out , but they are still big enough
scatter
to ___________
a beam of light.
What is a solution?

A solution is a homogeneous mixture (same throughout)
A solution can be a gas, liquid or solid.
Examples:
Air = O2 in N2
Kool-aid = Sugar in water
Brass = mixture of copper in zinc
Solutions
Two Parts to a Solution:
Solvent the dissolving medium which is
1) ____________typically a liquid or the substance in greater amount
when 2 similar phases are mixed
2) _____________
- the substance that dissolves
Solute
Hello again…
Aqueous Solutions

Solutions with water as the solvent.
Kool-aid =
SUGAR in water
Does sugar “disappear” or dissolve in water?
Does salt “disappear” or dissolve in water?
The dissolving questions have to
do with polarity…
Is water polar?
Stuff that dissolves in Water
1.
Polar Molecules – sugar is a polar molecule because
of the many polar –OH groups.
1.
Ionic Substances – salt is an ionic substance.

Ionic substances: cation + anion
Stuff that doesn’t dissolve in Water
3. Nonpolar Molecules – petroleum is nonpolar because
of all the nonpolar C-H bonds in the molecule. The
petroleum instead floats on water.
“Like dissolves like”

This phrase means that polar solvents dissolve
__________
polar solutes and nonpolar solvents dissolve
___________
nonpolar solutes.
Polar dissolves Polar
Nonpolar dissolves Nonpolar
You try “Like dissolves Like”


Would rubbing alcohol (polar) dissolve in nonpolar
oil?
Would nonpolar iodine (I2) dissolve in oil?
Solutions & Electricity
 __________________Electrolyte
a solution that conducts electricity.
Nonelectrolyte
 __________________a solution that does not conduct electricity.
What Determines if a Solution will Conduct Electricity?
charged ______________
particles
 A solution will conduct if there are ____________
ions
(or _________),
in the solution.
Most typical electrolytes: IONIC SOLUTIONS
 Example: Salt (NaCl)
Some solution vocab…
Miscible
• _______________
: two liquids that can dissolve in
each other
alcohol in water
Example: ____________
• _________________
: the liquids don’t mix
Immiscible
Oil and water
Example: _____
Exit Slip
1. If something dissolves in water, would it be a polar
or nonpolar substance?
2.
What would make a better electrolyte: Li3N or SF6?
3.
My name is monkey…. What is my favorite
smoothie?
Answers to Solutions Practice
f, e, a, b, c, d
2.
Solvent = Water; Solute = Coffee Beans
3.
Heterogeneous – looks different throughout; Homogeneous –
looks the same throughout (pg 39)
4. Polar dissolves polar; nonpolar dissolves nonpolar. Chemically like
substances dissolve each other
5. Grease stain must be nonpolar because it does not dissolve in water
and water is a polar substance; water just spreads the oil (in real life
 soap would be better and safer  soap has the ability to dissolve
both polar and nonpolar)
6. Miscible  choc syrup is mixable with milk
7. E, N, N, E, E
8. Gasoline – maybe unconventional, but can dissolve the oil (it’s why
it’s hard to wash oil off with water)
9. Unsaturated (it’s in the last section of your notes)
1.
Solubility

solute can dissolve
Solubility tells us how much _________
in a certain amount of _____________
at a particular
solvent
temperature and pressure to make a
saturated
“__________________”
solution.


_________________
Saturated solutions: a solution that contains as
much solute as will dissolve at that temperature
________________
Unsaturated solutions: a solution in which more
solute can dissolve than is already dissolved at that temp
Factors that
Affect Solubility:
Temperature
(abnormal behavior)
Increase temperature,
increase solubility.
On the solubility curve, the
lines indicate the concentration
saturated solution.
of a ____________
Values on the graph
_____________
below
a curve
represent unsaturated
solutions.
Example on Reading the Graph:
-Find the curve for KClO3
At 30°C approximately 10 g of
KClO3 will dissolve in 100g of
water. If the temperature is
increased to 80°C,
approximately ______
40 g of the
substance will dissolve in 100g
(or 100mL) of water.
1. What mass of KNO3 will
dissolve in 100 mL of water
at 70°C? ________.
2. What is the solubility of KCl
at 10°C? ______ g per 100 g
H2 O
3. a solution that contains 70g of
NaNO3 at 30°C (in 100 mL H2O)
Factors that Affect Solubility:
-------------------------------------------------
 Question:
What are 3 things you can do to get a solid to dissolve
more rapidly in a liquid?
1) Heat up the solution.
2) Stir the solution.
3) Crush the solid.
Solubility Curves Answers
1)
2)
3)
4)
5)
a. ~44 g
b. 40 g
c. 70 g
d. NaCl
(all answers g per 100 g H2O) a. 34 g b. ~14 g c. 5 g
Unsaturated
1. sat, - 2. sat, 3. unsat, 60 g 4. unsat, 35g
KClO3
Since we’re working with graphs – an approximation
for numbers. Be in the ballpark!!
Exit Slip
1.
2.
How many more grams
would it take to saturate a
solution a solution that
contains 65 grams of NaNO3
at 50 degrees Celsius? (how
much more solute can
dissolve?)
If you had to name a penguin
for a short story, what would
you name the penguin?
Answers to Solutions Practice 2
1) Hydrogen Bonding
3) B
4) C
5) A, B
2) A lot
6) C
7) C
8) B
9) A
10) A 10.5) A, B, C
11) Unsaturated
12) A. Unsaturated b. Around 34 degrees C (the saturation point
for NaNO3 of 100 grams is at 35 degrees  so above the
saturation line is when the solid cannot dissolve anymore in the
solute, 100 grams is above the solute line around 34).
14) a. No
b. Unsat
c. Copper Sulfate
Exit Slip
1.
2.
3.
Why can a mosquito can stand on water (think about
properties of water)
What type of mixture (suspension/colloid/solution)
would clouds be considered?
If you found out you could fly, what would be the first
thing you would do?
Exit Slip
1.
Explain why a mosquito can stand on water (think
about properties of water)
2.
If you found out you could fly, what would be the first
thing you would do?
Molarity & Concentrations
It’s a hot day.You took a sip of your lemonade.
And it tasted wayyyyyy too sweet. What can
you do to make your lemonade taste better?
Measuring the Concentration of a Solution
Concentration how much solute is dissolved in a certain
 ___________________:
amount of solvent at some given temperature and pressure.
Qualitative Vocabulary
Dilute
 _______________
: contains a small amount of solute
Concentrated : contains a large amount of solute
 _______________
concentrated
dilute
Molarity

Expression of concentration of a solution.
moles of solute
Molarity (M) =
liters of solution
mol
L
1 mol of solute per liter of solution is written as 1.0
(that is one molar)
moles
Molarity X
Liters
M
Making a Solution of a Required Concentration
# of moles
÷
# of liters
= Molarity
Example
What is the molarity of 2.0 moles of NaCl in 4L of
water?
1000 mL = 1 L
Example
What is the molar concentration of an aqueous NaCl
solution when 25.0 grams are dissolved in water to make
500 mL of solution?
Making Dilutions
Dilution: Making a solution _______
less concentrated by ________
adding
more ___________
.
solvent
Why dilutions??!!
“To save time and space in a lab, solutions are
purchased in concentrated form (stock solutions).
So, water (or another solvent) is added to achieve
the molarity of a particular solution”
Important: When diluting acids:
“Do like you otta, add acid to watta” (add acid to
base)
Equation for Dilutions
M1V1=M2V2
M1 -- the initial concentration of the solution.
V1 -- the initial volume of the original solution that is going to be diluted with water.
M2 -- the final concentration of the solution after it’s diluted with water.
V2 -- the total volume of the final solution after it has been diluted with water.
Making Dilutions
M1xV1=M2xV2
Practice Problem:
1) The science department buys HCl in large bottles that have a
concentration of 12 Molar. The science teacher then dilutes the acid
for labs. How would the teacher make 2.0 liters of a 2.5 M HCl
solution from this “stock” solution?
( 12 M ) ( V1 ) = ( 2.5 M ) ( 2.0 L )
V1 = 0.417 L
Take 0.417 L of the 12 M solution and add enough
water to make a final volume of 2.0 liters.
Making Dilutions
M1xV1=M2xV2
2) What is the final concentration of a sugar solution if water is added
to dilute 500 mL of a 2.5 M sugar solution to make a 800 mL
solution?
( 2.5 M ) ( 500 mL) = (
M2 ) ( 800 mL)
M2 = 1.56 M