Note Taking Guide: Episode 1001
Name______________
Solutions
•
•
•
•
•
formed when substances ______________ in other ______________
_______________ mixtures
_______________ phase
remain _______________; particles do not _______________ out
cannot be separated by _______________
•
solvent:
 present in _______________ amount
 ____________ the ____________ to make the solution
•
solute:
 present in _______________ amount
 _______________ in the _______________
Examples of Types of Solutions
LIQUID SOLUTIONS: _______________ solvent in which a __________ ,
_______________ , or _______________ is _______________
• _______________ dissolved in _______________:
ex. ______________________________
• _______________ in _______________
ex. _______________ in water
_______________: the two liquids mix
_______________: the two liquids _______________ mix
• _______________ dissolved in a _______________:
ex. _______________ water
SOLID SOLUTIONS:
• _______________: solid mixtures of _______________
(_______________ is a mixture of _______________ and
_______________)
GAS SOLUTIONS:
• gases dissolved in _______________ other (__________ is most
common example)
CHEMISTRY: A Study of Matter
© 2004, GPB
10.1
Aqueous: _______________ is the _______________
Tincture: _______________ is the _______________
Suspension
•
•
•
•
•
a _______________ mixture
Particles in the _______________ are thousands of times
_______________ than _______________ and _______________
Particles will _______________ out upon _______________
can be separated by _______________
exhibit the _______________ _______________
--the _______________ of _______________ in all directions
Colloid
•
•
•
•
particles are _______________ in size between those of _______________
and true _______________
particles do not _______________ out upon _______________
can not be separated by _______________
exhibit the _______________ _______________
Emulsion
•
•
_______________ dispersion of _______________ in _______________
_______________ agent is necessary for maintaining _______________
(________ is an example.)
CHEMISTRY: A Study of Matter
© 2004, GPB
10.2
Electrolyte:
dissolves in water to form a _______________ that
_______________ _______________
Nonelectrolyte:
dissolves in water to form a _______________ that does
_______________ conduct _______________
Factors Affecting the Rate of Solution
1)
_______________ _______________ :
increasing the surface area of the ___________ by ____________
speeds up _______________ by increasing the number of
_______________ between the _______________ and the
_______________ surface.
2) _______________:
_______________ or _______________ helps to disperse solute
particles, _______________ the number of _______________
between the _______________ and the _______________ surface.
3)
_______________:
increases the average _______________ _______________ of the
solvent molecules so that _______________ between the solvent
molecules and the _______________ are more _______________
The Chemistry Quiz
CR1. _____ CR2. _____
1. _____
2. _____
3. _____
4. _____
CHEMISTRY: A Study of Matter
© 2004, GPB
10.3
5. _____
Worksheet: Solutions Introduction
Name______________
1. Explain why solutions are classified as mixtures instead of compounds.
2. Solutions are ________________ mixtures made up of very small particles
that are actually molecules, __________, or ________.
3. Solutions are said to be in a ______________ phase even though the
components may have been in different phases before the solution was formed.
4. Pure gold is 24 carat. 14-carat gold contains 14 parts gold and 10 parts other
metals. 14-carat gold is said to be a(n) ___________, which is a type of
_______________ solution. An example of a gaseous solution is
________________, which is made up mostly of ______________ and
nitrogen when dry. The most common solutions are ______________
solutions.
5. Define miscible:
6. Define immiscible:
7. Because of the _______________ _______________, you can see the light
beams from car headlights in a fog.
8. Multiple choice: To increase the rate of solution of a solid in water,
a. increase the pressure over the water.
b. decrease the pressure over the water.
c. crush the particles of the solid.
d. chill the water.
9. If 15 grams of iodine are dissolved in 1000 mL of alcohol, the alcohol is the
(solute, solvent) and the solution is said to be a(n) _______________.
10. A substance that dissolves other materials is a (solute, solvent). The substance
being dissolved is a (solute, solvent).
CHEMISTRY: A Study of Matter
© 2004, GPB
10.6
11. In (solutions, suspensions) the substances separate after standing a while. The
substances (can also, can not) be separated by filtration.
12. Smoke is an example of a _____________ of solid dirt and dust particles in
air. After a while, the solid particles will fall to the ground.
13. A(n) ________________’s particles are between those of a solution and a
suspension.
14. ________________ are actually colloids comprised of one liquid in another
liquid. A(n) ______________ agent keeps the particles mixed.
15. What is an aqueous solution?
16. What is the solute in a brass alloy containing 75% copper and 25% zinc?
17. How does a solution behave differently from a suspension when a beam of light
is shined through it?
18. Substances that conduct electricity when dissolved are said to be
______________, while substances that do NOT conduct electricity when
dissolved are said to be __________________.
CHEMISTRY: A Study of Matter
© 2004, GPB
10.7
Note Taking Guide: Episode 1002
Name______________
Saturated: solution containing all the _______________ _______________
possible at given conditions of _______________ and _______________.
Unsaturated: solution containing _______________ dissolved
_______________ than the _______________ amount that can be
_______________ at given conditions of _______________ and
_______________.
Supersaturated: unusual solution containing _______________ dissolved
_______________ than is normally _______________ at given conditions of
_______________ and _______________.
Solubility
A _______________ of how much _______________ can _______________ in
a given amount of _______________ at a specific _______________.
Dilute Solution:
The amount of _______________ dissolved is
_______________ in relation to the amount of _______________ present.
Concentrated Solution: The amount of _______________ dissolved is
_______________ in relation to the amount of _______________ present.
CHEMISTRY: A Study of Matter
© 2004, GPB
10.8
Factors Affecting Solubility
1)
_______________ of _______________ and _______________:
“_______________ dissolves _______________”.
2)
_______________
 generally, increasing the _______________ of the solution
_______________ the solubility of a _______________ solute
 increasing the _______________ of the solution _______________
the solubility of a _______________ solute
3)
_______________
 only affects the _______________ of a _______________
_______________
 _______________ pressure _______________ solubility
 _______________ pressure _______________ solubility
 Henry’s Law: The _______________ of a _______________ dissolved
in a given _______________ of _______________ is
_______________ proportional to the _______________ of the
_______________.
The Chemistry Quiz
CR1. _____ CR2. _____
1. _____
2. _____
3. _____
4. _____
CHEMISTRY: A Study of Matter
© 2004, GPB
10.9
5. _____
Worksheet: Solubility Graphs
Name______________
Use the provided solubility graph to answer the following questions:
For questions 1 – 4 an amount of solute is given,
and a temperature is stated. If all of the solute
could be dissolved in 100 g of water at the given
temperature, would the resulting solution be
unsaturated, saturated, or supersaturated?
1. 60 g KCl at 70 °C
_________
2. 10 g KClO3 at 60 °C
_________
3. 80 g NaNO3 at 10 °C _________
4. 70 g CaCl2 at 20 °C
_________
For questions 5 – 8 a solute and temperature are given. Tell how many grams of
each solute must be added to 100 g of water to form a saturated solution at the
given temperature.
5. Pb(NO3)2 at 10 °C
_________
7. NaCl at 20 °C
_________
6. Ce2(SO4)3 at 50 °C
_________
8. K2Cr2O7 at 50 °C
_________
For questions 9 and 10 underline the solution that is more concentrated.
9. At 10 °C: a saturated solution of KNO3 or a saturated solution of CaCl2.
10. At 50 °C: a saturated solution of KNO3 or an unsaturated solution of NaNO3
consisting of 90 g of the solute dissolved in 100 g of water.
For questions 11 – 12, show your work and circle your final answer.
11. If 115 g KNO3 are added to 100 g of water at 35 °C, how many grams do not
dissolve?
12. What mass of KCl would be needed to form a saturated solution if the KCl was
dissolved in 200 g of water at 80 °C?
CHEMISTRY: A Study of Matter
© 2004, GPB
10.12
Worksheet: More on Solubility
Name______________
1. Explain what is meant by the expression “like dissolves like”.
2. An unknown compound is observed to mix with benzene (a nonpolar solvent) but
not with water. Is the unknown compound ionic or covalent?
If the unknown compound is a liquid, will it be able to dissolve table
salt?____________ Explain:
3. What are the chemical characteristics of a good dry-cleaning solvent?
4. Explain why you are more likely to overdose on vitamin A than on vitamin C.
5. Some industrial plants use water from nearby rivers and streams as a coolant.
When the water is returned to the river or stream, the water is warmer than it
was originally. This is referred to as “thermal pollution”. Using your knowledge
of solubility, why might this thermal pollution be harmful to fish?
CHEMISTRY: A Study of Matter
© 2004, GPB
10.13
6. After a bottle of carbonated drink has been open for a while, it tastes “flat”.
Explain why.
7. For most solid solutes, the degree of solubility in a liquid solvent (increases,
decreases) with an increase in the temperature of the solvent.
8. Describe what happens to the degree of solubility of a gaseous solute in a liquid:
a) with a decrease in the temperature of the solvent.
b) with an increase in pressure ( ____________ Law).
9. The following statement is false: It is not possible to make a saturated solution
from a substance that is described as only slightly soluble. Explain why this
statement is false.
CHEMISTRY: A Study of Matter
© 2004, GPB
10.14
Note Taking Guide: Episode 1003
Name______________
Molarity (M)
•
expresses _______________ _______________
•
M=
•
_______________, _______________, ______, and _______________ all
represent the same ratio.
Ex #1.
_______________
A saline solution contains ________ g of NaCl per
________ mL of solution. What is its molarity?
M=
Ex. #2
______________________
How many moles of solute are contained in _______ L of
__________ M CaCl2?
CHEMISTRY: A Study of Matter
© 2004, GPB
10.15
Colligative Properties
• Any of the _______________ of a _______________ that change when the
_______________ of the _______________ changes.
•
•
Depend on the _______________ of _______________ dissolved in a given
_______________ of _______________
Examples of Colligative Properties:
a. Vapor _______________ Depression
-- the _______________ of the _______________
_______________ of a liquid that occurs when substances are
_______________ in the _______________.
-- Vapor Pressure: the _______________ of a _______________
in _______________ with its _______________
b. Freezing _______________ Depression
-- the _______________ of the _______________
_______________ of a liquid that occurs when
substances are _______________ in the _______________.
(ex. using _____________ in car radiators and ________ on icy
roads)
c. Boiling _______________ Elevation
-- the _______________ of the _______________
_______________ of a liquid that occurs when
substances are _______________ in the _______________.
-- boiling occurs when _______________ _______________ equals
_______________ _______________.
(ex. ______________ in a car acts as a coolant in the summer.)
•
More Examples of Colligative Properties:
_______________ ,_______________, _______________
The Chemistry Quiz
CR1. _____ CR2. _____
1. _____
2. _____
3. _____
4. _____
CHEMISTRY: A Study of Matter
© 2004, GPB
10.16
5. _____