1. Solutions Parts of a Solution Molarity, Molality, Mole Fraction, Dilution

2. Types of Mixtures Mixtures : a blend of two or more kinds of matter, each of which retains its own properties and characteristics Homogeneous vs. Heterogeneous Mixtures Homo = same Hetero = varied

3. Solutions Solution : homogeneous mixture of two or more substances in a single phase Parts of a Solution : Solute – dissolved particlesEX. Salt, sugar Solvent – dissolving mediumEX. Water, alcohol Aqueous = capable of being dissolved

4. Concentrated vs. Dilute

5. What is Molarity? Moles of solute per volume of solution Equation is GIVEN on Reference Table!

6. Moles of solute per volume of total SOLUTION Mol of solute Liters of solution mol L M Moles of solute per mass of SOLVENT Mol of solute Kg of solvent mol kg m

7. What is molality? Moles of solute per mass of solvent Equation is NOT GIVEN on Reference Table!

8. Molarity Examples EXAMPLE : 3.50 L of solution contains 90.0 g of NaCl. What is the molarity of the solution? EXAMPLE : 0.800 L of a.500 M HCl solution. How many moles of HCl does this solution contain?

9. Molality Examples EXAMPLE : Solution was prepared by dissolving 17.1 g of sucrose (C 12 H 22 O 11 ) in 125 g of water. Find the molal concentration of solution. EXAMPLE : A solution iodine (I 2 ) in carbon tetrachloride (CCl 4 ) is used when iodine is needed for certain chemical tests. How much iodine must be added to prepare a 0.480 m solution of iodine in CCl 4 if 100.00 g of CCl 4 is used?

12. What is mole fraction? MOLE FRACTION (  ) = EXAMPLE : What is the mole fraction of xenon in a mixture that contains 0.584 g of xenon 86.40 g of argon and 3.62 g of neon ?

13. Dilutions How many solute parts? 13 What’s the only difference?

14. How can you dilute a concentrated solution? DILUTION = EXAMPLE : What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H 2 SO 4 solution?