Chapter 4 Study Guide: Solubility
Know all labs!
Understand lab questions
Understand procedures and concepts
- 4.1: Dissolving a solid in water
o Qualitatively a saturated solution vs. unsaturated solution
o Uniformity- evenly distributed
o Calculating concentrations
- 4.3: Comparing the Concentrations of Saturated Solutions
o Quantitative solubility vs. qualitative
o Know the process/steps for finding solubility
o Solubility= characteristic property
- 4.4: The Effect of Temperature on Solubility
o Understand solubility graphs
o Solids- Solubility increases as temperature increases
- 4.6: Methanol as a Solvent
o Use different solvents to distinguish between solutes
o Use different solutes to distinguish between solvents
- 4.8: Two Gases
o
o
o
o
Properties of Hydrogen
Properties of Carbon Dioxide
How we understand these properties
Test tube up vs. test tube down (density relative to air)
Reading Sections:
-
4.5: Wood Alcohol (Methanol) vs. Grain Alcohol (Ethanol)
o Same densities but different melting and boiling points
Hydrogen
o Flammable, less dense than air, no reaction with limewater, insoluble in water
Carbon Dioxide
o Non-flammable, more dense than air, reacts with limewater, insoluble in water
Review All Handouts:
-
Vocabulary
Concentrations
Finding the solubility of a saturated solution- Lab 4.3 (2 problems!)
Lots of Solubility graph problems
Review worksheets (analyzing problems)
o What effects solubility?
Properties of Gases (know the properties!)
o What test is best to indicate the presence of that gas?
1. Review Solubility vocabulary. You should be very familiar with all of these words!
2. You should be able to determine concentration of solutions (concentration boxes) Try
this:
4g/60cm3
g/60cm3 ?
g/100cm3 ?
3. Review Lab 4.1
What does uniformity in color mean?
The amount of solid that will dissolve in a solvent depends upon…
Name 3 substances that are widely known solvents:
What does saturated solution mean? What does it look like?
A green, saturated solution is created when 23.50g of solute is dissolved in 100 cm3 of
water. Einstein mixed 3.54g of the green solute into 15.05 cm 3 of water. His lab
partner, Newton mixed 5.45g of the green solute into 23.15 cm3 of water.
Did either have a saturated solution? Calculate their concentrations.
4. Review “Quantitative Solubility” Sheet based on Lab 4.3.
How do find the concentration per 100? Check you answers with your neighbor. Can
you do this by yourself?
Which substance was more soluble in water? (Hint check “Post Lab 4.3”)
5. Look over your Chapter 4 Quiz Study Guide
6. Does heating a solution always increase the solubility? Read over Post Lab 4.4
information.
7. Do you know how to use a solubility curve graph?
Look over “Solubility Curve Practice 1” and “Solubility Practice 2” OR “Solubility Curve
Challenge.”
Try these:
What temperature is required to dissolve 110 g of sodium nitrate in 100 cm 3 of water?
If 20 g of sodium chloride is dissolved in 100 cm3 of water at 20ºC, is the solution
saturated? How do you know if a solution is saturated?
A mass of 10 g of sodium nitrate is dissolved in 10 cm3 of water at 80ºC. As the solution
is cooled, at what temperature will a precipitate first appear?
A mass of 20 g of potassium sulfate is dissolved in 100 cm3 of water at 70ºC. The
solution is cooled to 45º C. How many grams of potassium sulfate will precipitate out of
solution?
8. When you used methanol as a solvent, what did you learn? Summarize below.
Sugar
Citric acid
Magnesium carbonate
Magnesium
Moth flakes
What information helps you know how to separate these substances?