Chp. 6 Guided Notes
Name:_____________________________
Types of Mixtures:
1. Heterogeneous: not the same throughout
2. _________________: uniform throughout (completely mixed)
Heterogeneous Mixtures:
3. ____________________: a mixture that looks uniform when stirred or shaken that separates into different
layers when it is no longer agitated.
a. Example: oil & vinegar , orange juice
4. Colloids: A mixture of very tiny particles of pure substances that are dispersed in another substance but do
not settle out of the substance.
a. Particles in a colloid are much smaller than those in a suspension and _________________settle at
the bottom.
b. The particles stay ______________________ throughout the mixture.
Heterogeneous Liquid-Liquid Mixtures:
5. Liquids that will not dissolve into one another are _______________________(they do not mix)
a. Example: Oil & Vinegar
b. The oil is less dense & __________________above the vinegar
6. Some immiscible liquids can mix in__________________.
a. Example:
7. An ______________________is any mixture of immiscible liquids in which the liquids are spread
throughout one another
Homogenous Mixtures:
8. Uniform throughout Example: Salt water
9. ______________are homogeneous mixtures of two or more substances uniformly spread throughout a
single phase
10. There are 2 main parts to a solution:
a. ___________The substance that dissolves in a solution
b. ___________The substance that dissolves the solute to make a solution
11. Two or more liquids that form a single layer when mixed are __________________
12. Miscible liquids can be separated by______________________.
Chapter 6 Section 2: Dissolving & Solubility
1. Solutes with a larger surface area will dissolve ______________
a. Is dissolving a chemical change?
b. _____________it is a ________________Change (pg. 60)
2. A substance in small pieces dissolves faster than the same substance in big pieces.
3. Stirring or shaking a solution helps the solute dissolve faster
a. “Movement” does what to the particles in a substance?
b. Adds ____________which increases the speed of the particles
4. Solutes dissolve faster when the solvent is ____________.
5. Substances can be Soluble and Partly Soluble
6. ______________: dissolves in water
7. Partly Soluble: does not completely dissolve in water.
Water is the ______________ Solvent.
8. Water’s structure helps it dissolve charged particles.
a. Why? What is the structure of water?
b. Water is a _________________molecule which allows it to dissolves substances easily
9. Water will not dissolve all substances.
10. Water cannot dissolve substances that are considered “_________________”
11. _________________ is the quantity of solute dissolved in a given a solution
12. Solutions can have different concentrations depending on the amount of solute & solvent
13. A solution that is _________________has a large amount of solvent compared to solute
14. A Concentrated Solution has a large amount of dissolved _________________.
15. Unsaturated solutions can dissolve more solute.
16. They have more space available for particles to move (spread out).
17. *Considered “____________________” as long as a solution can dissolve more solute.
18. A Saturated Solution is a solution that cannot dissolve any more solute at the given conditions
19. __________________ is the greatest quantity of a solute that will dissolve in a given quantity of
solvent to produce a saturated solution.
Chp. 6 Section 2 Continued
1. Heating a saturated solution usually allows you to dissolve even_______________ solute.
2. The Solubility of most solutions will increase as the temperature increases.
3. A ___________________ ____________________ is a solution holding more dissolved solute than is
specified by its solubility at a given temperature.
4. Concentration can be measured/expressed in grams per 100g of solvent or as a mass percent or in grams
per 100g of solution.
5. Molarity = moles of solute / liters of solution
6. ______________is the preferred concentration unit because it expresses the molar amount of solute
present*
Chapter 6 Section 3
Acids, Bases, & pH
1. An ___________is a substance that creates hydrogen ions H+
a.
will form Hydronium (H3O+) ions when dissolved in water.
2. Acids have a pH _______________7
3. Indicators can be used to determine the acidity of a substance.
a. Litmus paper can be used as an acid indicator
i. Acids will turn blue litmus paper ____________.
Acids & Electricity
4. All acids can conduct electricity when dissolved in water because all acids for hydronium ions (H3O+).
5. __________________acids will conduct electricity better than weak acids
6. _____________created as acids dissolve in water move throughout the solution conducting electricity.
a. Sulfuric Acid in water conducts electricity in car batteries.
7. Weak acids _____________ionize completely & will not conduct electricity
a. Example: Acetic Acid (Vinegar)
8. Fewer ions (charges) = ______________conductivity
Bases
9. Some bases produce __________ions (OH-)
a. Bases cause red Litmus paper to turn _______________
10. Can be very dangerous if not diluted with water
11. Bases have a pH ______________7
pH Scale
1. pH values correspond to the concentration of hydronium ions & hydroxide ions.
2. The Scale ranges from ________ to __________.
3. A reaction between hydronium ions & hydroxide ions to form water molecules
4. The resulting solution is more ______________than either of the reactants.

Some acid-base reactions do not result in neutral solutions

The pH of the resulting solution depends on the amounts of acid & base that are combined
Chapter 6 Section 4: Acids & Bases in the Home
 Bases in the home…
 Soaps (emulsifier)
 Cleaning Products
 Detergents
 Ammonia Solutions
 Disinfectants (Bleach)
 Antacids are weak ________________that neutralize excess stomach acid.
 Shampoos are made of detergents that are able to remove dirt & oil without leaving a residue.
Review:

Which creates H+ ions?

Which creates OH- ions?

Which can conduct electricity & why?

Which have a pH below 7?

Which have a pH above 7?

What category do suspensions & colloids fall into?

How are they similar and different?

What are immiscible liquids?

Example: