1. Solutions!

2. Classification of Matter Matter Pure Substanc es Mixtures HomogeneousMixturesHeterogeneousMixturesElementsCompounds

3. Heterogeneous Mixtures See visibly different regionsSee visibly different regions –Granite –Dirt –Cereals –Oil & Vinegar See a boundarySee a boundary –Ice cube in water

4. Homogeneous Mixtures (SOLUTIONS) Particles very small – on atomic scaleParticles very small – on atomic scale –Can’t see particles –Can’t sort particles –Can’t get trapped by filter –Can’t scatter light Particles evenly distributedParticles evenly distributed Particles do not separateParticles do not separate

5. CuSO 4 (aq) Which is a solution & how do you know?

6. Solution Homogeneous mixture of 2 or more substances in a single physical state (phase)

7. FINDING CONCENTRAION: We can measure how much HCl, NaHCO 3, PbNO 3 is mixed with the water…

8. Concentration: measurement that describes how much solute is in given amount of solvent or solution NOTE: Many, many different units to express concentration - Pick the unit by the task at handNOTE: Many, many different units to express concentration - Pick the unit by the task at hand

9. Percent By mass mass (solute) x 100% mass (solution) By volume volume (solute) x 100% volume (solution)

10. Mass solution = Mass solute + Mass solvent

11. PPM (parts per million) PPM = grams solute X 1,000,000PPM = grams solute X 1,000,000 used when solute is present in very small amounts (The Regents don’t follow this rule)used when solute is present in very small amounts (The Regents don’t follow this rule) like % except you multiply by 1,000,000 instead of 100 grams solution

12. LET’S PRACTICE: About 0.0043 g of O 2 can be dissolved in 100 mL of water at 20 o C. Express in ppm. [Memorize: 1 mL water has mass of 1 g] What is the solvent? Water How much solvent is there? 100 mL = 100 g How much solute is there? 0.0043g How much is the total solution? 100 g +.0043 g = 100.0043g

13. LET’S PRACTICE: About 0.0043 g of O 2 can be dissolved in 100 mL of water at 20 o C. Express in ppm. THE EQUATION ppm = 0.0043g X 1,000,000 100.0043g ppm = 43 ppm [Memorize: 1 mL water has mass of 1 g]

14. NOW YOU TRY: CO 2 gas has solubility of 0.0972 g/100 g water at 40 o C; Express in parts per million ppm = 0.0972 g solute X 1,000,000 100.0972 g solution = 971 ppm

15. HERE’S ANOTHER: What is the concentration in ppm of a solution with 30.0 g NaNO 3 in 70.0 g water? ppm = 30.0 g NaNO 3 X 1,000,000 100.0 g solution = 300,000 = 3.0 X 10 5 ppm

16. LAST ONE: How many grams of KOH are needed to be dissolved in water to make 2000.0 grams of a 10.0 ppm solution? 10 ppm = X grams KOH X 1,000,000 2000.0 g solution X = 0.02 grams KOH