TOPIC 7 – Properties of Solutions
Topic Overview
Why are solutions one of the most important concepts in Chemistry?
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TERM
DEFINITION
DIAGRAM
Mixture
Solution
1
alloy
solute
solvent
soluble
insoluble
2
List (and memorize) five characteristics of a solutions:
1.
2.
3.
4.
5.
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Why can solutions NOT be separated by filtration?
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How CAN solutions be separated? _______________________________
Describe distlllation (p.72)
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Describe what is meant by “like dissolves like”:
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How does temperature affect solubility of solids in water? __________________________________________________
How does temperature affect solubility of gases in liquids? _________________________________________________
How does pressure affect solubility of solids and liquids? ___________________________________________________
How does pressure affect solubility of gases in liquids? _____________________________________________________
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TOPIC 7 – Properties of Solutions
Solubility Graphs
Solubility Curves are located in Reference Table
_________!
Each curve shows how many _____ of a substance will dissolve in _______________ of water at a given _____________.
The curves with positive slopes represent ____________ being dissolved in water.
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The positive slope means that as temperature _____________________, solubility _______________________.
An exception to this rule is _____________________.
The curves with negative slopes represent ______________ being dissolved in water.
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The negative slope means that as temperature _____________________, solubility
_________________________.
The three gases on these solubility curves are __________, ___________, and __________.
TERM
DEFINITION
DIAGRAM
Saturated
4
Unsaturated
Supersaturated
Dilute
Concentrated
5
On EACH solubility curve below,
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A is ___________________________________
B is ___________________________________
C and D are _______________________________
C
A
B
B
C
B
D
A
C
D
B
D
D
A
Solubility Guidelines are located in Reference Table
C
A
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What is this table useful for? _________________________________________________________________________
When will a reaction take place? ______________________________________________________________________
If you are in a lab and need to determine whether a solution is unsaturated, saturated, or supersaturated, you can add
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If the solution is unsaturated, then ______________________________________________________________
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If the solution is saturated, then ________________________________________________________________
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If the solution is supersaturated, then ___________________________________________________________
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TOPIC 7 – Properties of Solutions
Concentration of Solutions
When are the terms “dilute” and “concentrated” not adequate to describe solutions?
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Ways to Express and Calculate Concentration and When Each is Useful
Remember: Equations are on Reference Table _______
MOLARITY (M)
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Solutions in a lab are labeled with MOLARITY.
molarity = _____________________
Ex.) Mr. Bitar needs to prepare a 0.5M solution of hydrochloric acid for a lab. He needs to have 2.0 liters of solution.
How many moles of HCl does he need?
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PERCENT MASS

Consumer products often are labeled with their active ingredients as percent mass.
percent mass = _________________________
Ex.) Miracle Grow fertilizer lists nitrogen as 15%. How many grams of nitrogen are in a 5lb (2260g) bag?
The same fertilizer lists phosphate (P2O5) as 30%. How many grams of phosphate are in this bag?
PERCENT VOLUME

Consumer products that are liquid often are labeled with their active ingredients as percent volume.
percent by volume = ____________________________
Ex.) Rubbing Alcohol is 70% isopropyl alcohol (C3H7OH). The bottle is 16oz (473.18mL). What volume of that is
isopropyl alcohol?
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PARTS PER MILLION (ppm)
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Parts per million is used for extremely ___________________ solutions.
Often, parts per million is used for __________________________ in air or water.
ppm = ____________________________ X
Ex.) In Erie County, NY, the concentration of fluoride in the drinking water is 2.2mg/L. Convert this to ppm.
Hint: First, convert mg to g. Then convert L to grams. 1 mL of water is 1 g.
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TOPIC 7 – Properties of Solutions
Colligative Properties
The freezing and boiling points of water change when nonvolatile ______________________ are added.
Why is salt applied to roads and sidewalks when there is snow and ice?
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The amount of lowering of freezing point depends on the ___________________ of dissolved _____________________.
One mole of any particle will lower the freezing point of 1000g (1L) of water by ____________ degrees Celsius.
Molecular vs Ionic
Why does one mole of NaCl depress the freezing point of water twice as much as one mole of C12H22O11?
Use the terms molecular, ionic, ions, separates, in your answer.
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How much will one mole of dissolved particles raise the boiling point of 100g (1L) of water? ___________
What happens to the temperature of boiling water when we add table salt (NaCl)?
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Vapor Pressure
Which type of molecules are held together by dipole-dipole forces? ___________________________
Which type of molecules are held together by hydrogen bonds? _____________________________________________
Which force is stronger? ________________________
What is a vapor? ____________________________________________________________________________________
Give two examples. _______________________________________________________________________________
When the temperature of a liquid increases, their energy ____________________________.
How is this related to vapor pressure? __________________________________________________________________
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Vapor pressure of four common liquids is illustrated on Reference Table _______.
Which liquid has the highest vapor pressure? __________________________________
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This means that it has the ___________________ intermolecular forces.
Which liquid has the lowest vapor pressure? ___________________________________
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This means that it has the _______________________ intermolecular forces.
Boiling Point
As the temperature of a liquid rises, its vapor pressure ______________________.
What happens to a liquid when its vapor pressure rises enough to equal the atmospheric pressure?
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List four equivalent measures of normal atmospheric pressure
______________, ______________, ________________, _________________
Define “heat of vaporization”: _________________________________________________________________________
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Look at Reference Table ______. What is the heat of vaporization of water? ________
What happens to the boiling point of water when the atmospheric pressure is lower than normal? ________________
What happens to the boiling point of water when the atmospheric pressure is higher than normal? ________________
What is the normal boiling point of water? _____________
What is the boiling point of water today? ___________
What does that tell you about the air pressure today? ____________________________
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