1. Chemistry, Ch. 13: Solutions
Vocabulary
Soluble
Solvent
Solute
Suspension
Electrolyte
Saturated solution
Unsaturated solution
Supersaturated solution
Solubility
Miscible
Immiscible

2. Vocabulary *Soluble: Capable of being dissolved
*Solvent: The dissolving medium in a solution (thing that does the dissolving)
*Solute: The substance dissolved in a solution
*Suspension: Particles in a solvent are so large that they settle out unless mixture is constantly stirred

3. Vocabulary
Electrolyte: Substance that dissolves in water to give a solution that conducts electric current
*Unsaturated solution: Solution that contains less solute than a saturated solution under the existing conditions
*Saturated solution: Solution contains the maximum amount of dissolved solute

4. Vocabulary
*Supersaturated solution: Solution that contains more dissolved solute than a saturated solution contains under the same conditions
*Solubility: The amount of substance required to form a saturated solution with a specific amount of solvent at a specified temperature

5. Vocabulary
Miscible: Liquids that dissolve freely in one another in any proportion
Immiscible: Liquid solutes and solvents that are not soluble in each other

6. Kool-Aid Contents: Which is it?
The sugar in Kool-Aid:
solute
The water in Kool-Aid:
solvent
Video: supersaturated solution
immiscible

7. Which is it?
electrolyte
suspension

8. Solubility Graphs (Fig. 13-15)
Not all solutes have the same solubility

9. What mass of KClO3 will dissolve in 100 g of water at 10°C?
If a solution has 15 g of KNO3 dissolved in 100 g of water at 10°C, is it unsaturated, saturated, or supersaturated?
Unsaturated

10. What is the maximum mass of KNO3 that will dissolve in 500 g of H2O at 40°C?
64g KNO3 = x
100g H2O g H2O
320g KNO3

11. Molarity Measure of concentration of a solution
Molarity = moles of solute
L of solution
Abbreviated: M (“molar”)
3M HCl = “3 molar” HCl
= 3 moles HCl
1 L solution

12. Example 1 2 moles NaCl = 0.57 M NaCl 3.5 L
You have 3.5 L of solution that contains 2 moles of sodium chloride. What is the molarity of the solution?
2 moles NaCl = M NaCl
3.5 L

13. Example 2
You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain?
0.5 M = x
0.8 L
x = 0.4 mol HCl

14. Example 3
You have 4.5 L of solution that contains 175 g of copper (II) sulfate. What is the molarity of the solution?
175 g CuSO4 1 mol CuSO4 = 1.10 mol CuSO4
g CuSO4
1.10 mol CuSO4 = M CuSO4
4.5 L