Chapter 13 Notesheets
Name ___________________________
Solutions
Period_______Date _______________
13.1: The Nature of Solutions
1. Solution: A ____________________ mixture of 2 or more substances in a ________________
physical state (visibly the same throughout.)
A. Properties of Solutions:
1. ______________ particles
2. particles are _______________ distributed
3. particles won’t _________________ when allowed to stand
4. every substance has it’s own __________________
B. Vocabulary:
Solute: substance that is __________________(usually  50% of solution)
Solvent: substance that does the __________________ (usually  50% of the solution)
Soluble means something _____ be dissolved in a solvent. Ex)
Insoluble means something _________ be dissolved in a solvent. Ex)
C.Types of Solutions:
1. Solid Solutions (solid solute)
Alloys: ______________ solution that contains two or more ________________.
Ex)
Advantages of alloys over pure metals:
2. Gaseous Solutions: (gaseous solute) The properties of gaseous solutions depend on
the properties of its _______________________. Ex)
3. Liquid Solutions: (liquid solute)
Miscible liquids: Two liquids that are _________to mix together in any proportion.
Ex)
Immiscible liquids: Two liquids that are ______________ to mix together in any
proportion. Ex)
Aqueous Solutions: Solutions with _____________ as the solvent. Because water
can dissolve so many things, it is called the _______________________________.
Tincture: Solutions with __________________ as the solvent.
Ex)
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Electrolyte: __________ compounds dissolve in water to form ions that
can ________________ an _______________ current. Ex)
Nonelectrolyte: __________________ compounds dissolve in water to form
molecules that ________________conduct an _____________ current. Ex)
D. Separating Solutions: Done through a change of state - _________________________ or
______________________________.
13.2: Concentrations of Solutions
A. Terms Used for Concentration: The amount of _____________ in a given amount of
solvent or solution.
1. Concentrated: When a solution has a _____________ amount of solute compared
to solvent.
2. Dilute: When a solution has a _____________ amount of solute compared
to solvent.
3. Saturated: A solution is saturated if it contains as much ______________ as can
possibly be dissolved under existing conditions of _____________________ and
_____________________.
4. Unsaturated: Has __________ than the maximum amount that can be dissolved.
5. Supersaturated: Has _________ than the maximum amount that can be
dissolved.
The Formation of Solutions:
B. How a Solution forms:
1. Process of dissolving takes place at the _______________ of the solute.
2. The interaction between the solute and solvent to allow ions to separate is called
_________________________. This interaction is called _______________________
when water is the solvent.
3. Energy is ______________ when the ________ between solute and solvent break. (
)
4. Energy is _______________ when bonds between solute and solvent _________. (
)
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C. Solubility
1. Solubility is the ________________ of ________________ that will dissolve in a given
amount of _______________ at a certain _______________________ (pressure.)
2. Factors that affect solubility:
A. Nature of Solute and Solvent:
General rule:
_______________ dissolves _______________
__________________ in __________________
__________________ in __________________
Example:
B. Temperature:
1. As temperature increases, the solubility of gases ____________________.
2. For an endothermic solid: If the temperature drops when the solute and
solvent are mixed, raising the temperature will ________________ solubility.
3. For an exothermic solid: If the temperature rises when the solute and solvent
are mixed, raising the temperature will ____________________ solubility.
C. Pressure:
1. As pressure increases over a gas, solubility ___________________.
3. Factors that affect the Rate of Dissolving:
A. __________________________
B. __________________________
C. _________________________
D. All three of these factors affect the ________________ over which the solvent can
come into contact with the ________________.
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D. Molarity: (M)
molarity = moles of solute
liters of solution
M= n
v
unit = mol
L
Ex #1) What is the molarity of a solution formed by mixing 10.0 g of sulfuric acid with enough
water to make 100.0 mL of solution?
Ex #2) How many grams of bromine are needed to prepare 0.500 L of a 0.0100 M solution of
bromine in water?
Ex #3) Describe how would you prepare 100.0 mL of 0.7500 M potassium nitrate?
Ex #4) What volume of 0.600 M sodium hydroxide can be prepared from 4.8 g of solute?
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