1. Moles 1 mole = 6.022 x 10 23 1 mole = 6.022 x 10 23 1 pair = 2 1 pair = 2 1 dozen = 12 1 dozen = 12 Etc. Etc. 1 mole of atoms = the atomic weight on periodic table 1 mole of atoms = the atomic weight on periodic table

2. Practice calculations How much would a mole of KNO 3 weigh? How much would a mole of KNO 3 weigh? How much would a mole of acetic acid (CH 3 COOH) weigh? How much would a mole of acetic acid (CH 3 COOH) weigh? How much would a mole of copper (II) phosphate (Cu 3 (PO 4 ) 2 ) weigh? How much would a mole of copper (II) phosphate (Cu 3 (PO 4 ) 2 ) weigh?

3. More practice problems How many moles is 3.0 grams of sugar (C 6 H 12 O 6 )? How many moles is 3.0 grams of sugar (C 6 H 12 O 6 )? 35.0 g of CaCO 3 is how many moles? 35.0 g of CaCO 3 is how many moles? 0.17 moles of Na 2 HPO 4 is how many grams? 0.17 moles of Na 2 HPO 4 is how many grams?

4. Concentration Units Molarity (moles of solute/liter of solution) Molarity (moles of solute/liter of solution) If a solution of HCl contains 3.15g of HCl in 25mL, what is the molarity of the solution? I want to make 500mL of a 0.05M NaOH, how may grams of NaOH do I need? I want to make 500mL of a 0.05M NaOH, how may grams of NaOH do I need?

5. pH scale Neutral pH? Neutral pH? Acidic pH? Acidic pH? Basic pH? Basic pH? pH = -log[H+] pH = -log[H+] Log scale therefore pH of 1 is 10x more acidic than a pH of 2 Log scale therefore pH of 1 is 10x more acidic than a pH of 2

6. pH scale continued A solution has a [H+] of 0.01M. What is its pH? A solution has a [H+] of 0.01M. What is its pH? The [H+] is 0.005M pH = ? The [H+] is 0.005M pH = ? Windex has a pH of ____, what is its [H + ]? Windex has a pH of ____, what is its [H + ]? SnoBowl has a pH of ____, what is its [H + ]? SnoBowl has a pH of ____, what is its [H + ]? As pH increases acidity decreases As pH increases acidity decreases

7. Acids/ Bases & Life pH of blood must be between 7.3-7.5 pH of blood must be between 7.3-7.5 How is this done? How is this done? Buffers: substance which resists changes in pH Buffers: substance which resists changes in pH Carbonate buffer system is important for maintaining pH in biological systems Carbonate buffer system is important for maintaining pH in biological systems

8. Acid Rain Demonstration Which areas are more susceptible to the effects of acid rain, areas with thin soils and granite underneath or areas with carbonate soils? Why? Which areas are more susceptible to the effects of acid rain, areas with thin soils and granite underneath or areas with carbonate soils? Why? CaCO 3 + H +  Ca 2+ + HCO 3 - Limestone weathering 2KAlSi 3 O 8 + 2H + + H 2 O  Al 2 Si 2 O 5 (OH) 4 + 4SiO 2 + 2K + Feldspar weathering

9. Acid Rain Chemistry 107 LocationpHw/acidw/base Richards6.626.86.85 Winona6.666.766.74 snow6.966.56.59 distilled6.045.856.35 Tap (dorms)6.666.296.5 snow5.983.595.63 well water6.736.286.57 Lake Winona6.246.046.07 Mississippi6.236.045.93 Richards6.426.326.45 Root River7.266.837.2 Mississippi7.27.196.99 distilled7.434.293.94? campus (tap)7.57.187.5 faucet (house)7.197.057.13 distilled6.193.76.94 Somsen76.737.22 Lake Winona7.266.877.26 Tap (dorms)7.157.077.28