Name: ______
Chemistry: Mixtures Review
Test Overview:
· Vocab Matching
· Identifying sample mixtures as suspensions, colloids, or solutions
· Concentration Calculations: Molarity and Percent Concentration
· Solubility – polar/nonpolar, “like dissolves like” rule
· Solubility Factors that increase the rate of dissolving
· Solubility Curves
· Conductivity of Solutions
· Colligative Properties
1. Recognize the following vocabulary terms:
Homogeneous
Heterogeneous
Colloid
Suspension
Solution
Solute
Solvent
Concentration
Molarity
Soluble
Insoluble
Miscible
Immiscible
Polar/ nonpolar
Solubility
Saturated
Unsaturated
Supersaturated
Conductivity
Dissociation
Electrolyte
Colligative properties
Emulsion
Surfactant
2. Be able to identify solutions, suspensions, versus colloids:
______medicine (label reads “needs to be shaken”)
______whipped cream
______Copper Chloride in water
______fog
______oil & vinegar
3. What is the difference between soluble/insoluble and miscible/immiscible?
4. Explain why water and oil do not mix in salad dressing. Be sure to include the following terms in your explanation: miscible, immiscible, polar, nonpolar. Also, explain what is meant by the phrase “like dissolves like”.
5. Identify the following mixtures as miscible or immiscible:
ethanol (polar) and water ______
naphthalene (nonpolar) and water ______
6. What are colligative properties? Describe an example of a colligative property.
7. What is an electrolyte? Why do solutions with ions allow electricity to flow?
Concentration
8. What is the molarity of 2.56 moles of potassium iodide dissolved in 250. mL of solution?
9. Calculate the molarity of 198 g of barium chloride (BaCl2) in 2.0 L of solution.
10. What mass of Ag of AgNO3 is needed to prepare 750mL of a 1.5M solution?
11. What is the percent by mass of a solution with 35.5g of AgNO3 dissolved in 500. g of water?
12. What is the percent by mass of a saline solution with 45g NaCl dissolved in 200g of water?
13. How much solute is in 250g of a 6.5% glucose solution?
14. What is the molality of 2.00mol of Copper Sulfate dissolved in 8000g of solvent?
15. Stoichiometry: What mass of AgCl will be produced if .2L of 1.3M NaCl solution reacts?
NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s)
16. Stoichiometry: What volume of .6M AgNO3 will react if 75.0g of NaNO3 is produced?
NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s)
For extra practice, also complete Mixed Molarity Practice (evens/odds)
Solubility Curves (use your Solubility Curve)
17. How many grams of KI can be dissolved in 100g H2O at 20oC? ______
18. What mass of NaCl will dissolve in 100g of 100g of water at 90oC? ______
19. What substance is least soluble at 90 oC? ______
20. What is the difference between saturated, unsaturated, supersaturated?
21. Label the following solutions as saturated, unsaturated, or supersaturated in 100mL of water at the given temperature:
- ______138g of KI at 10 oC
- ______75g of KCl at 70oC
- ______30g of NaCl at 90oC
22. For the unsaturated solution (above), how much extra solute would need to be dissolved to create a saturated solution?
Solubility Curves (use your Solubility Curve)
17. How many grams of KI can be dissolved in 100g H2O at 20oC? ______
18. What mass of NaCl will dissolve in 100g of 100g of water at 90oC? ______
19. What substance is least soluble at 90 oC? ______
20. What is the difference between saturated, unsaturated, supersaturated?
21. Label the following solutions as saturated, unsaturated, or supersaturated in 100mL of water at the given temperature:
- ______138g of KI at 10 oC
- ______75g of KCl at 70oC
- ______30g of NaCl at 90oC
22. For the unsaturated solution (above), how much extra solute would need to be dissolved to create a saturated solution?