1. WARM UP ACT Prep Passage V 5 minutes Start when the bell rings

2. Concentrations of Solutions

3. Concentration Definition Amount of solute in a quantity of solvent/solution

4. Basic Concentration Descriptions Saturated solution –Maximum amount of dissolved solute Unsaturated solution –Can dissolve more solute

5. Basic Concentration Descriptions Supersaturated solution –More solute than can normally be dissolved Increased temp. –Unstable Crystallization

6. Mathematical Concentration Units Percent by Mass o Mass of solute Mass of solution solution = solute + solvent o Unit: % x 100

7. Mathematical Concentration Units Mole Fraction o Moles of solute Moles of solution solution = solute + solvent o No unit

8. Mathematical Concentration Units Molarity o Moles of solute Liters of solution solution = solute + solvent o Unit: M

9. Mathematical Concentration Units Molality o Moles of solute Mass of solvent (kg) o Unit: m

10. Chemistry and Math All equations can be set up to find any unknown value May need to convert to get to the unit you need for a formula

11. WRAP UP 1.Calculate both the % by mass and the mole fraction of a solution of 15 g Cu and 95 g Sn. 2.Calculate the molarity of a solution of 3 moles of HCl dissolved in 850 mL of solution. 3.Calculate the molality of a solution of.837 moles of sugar in 5.59 kg of water.

12. WARM UP Which two measurements of concentration are most commonly used? Why is this? Write the formula and unit for each.

13. WRAP UP If you have a solution of 11.2 g of NaCl and 118.8 g of H 2 O (d=1.0 g/mL), that create 120 mL of solution when mixed, calculate: –% by mass –mole fraction

14. WARM UP The molality of a solution of chlorine and water is.0362 m. This solution contains 3500 g of water. How much chlorine, in grams, was used to prepare this solution?

15. WRAP UP If you have a solution of 11.2 g of NaCl and 118.8 g of H 2 O (d=1.0 g/mL), that create 120 mL of solution when mixed, calculate: –molality –molarity