1. Acid Base Chemistry

2. Acids Taste sour conduct electricity react with zinc or magnesium to produce hydrogen gas turn blue litmus paper red

3. pH = 0-7 strong acids with concentrations greater than 1.0mol/L will have a negative pH

4. Bases taste bitter conduct electricity have soapy, slippery feeling turn red litmus paper blue

5. pH = 7-14 strong bases with concentrations above 1.0mol/L will have a pH above 14

6. Naming Acids H-”ide” a H-”ick”y “ate” something “ick”y B-”ite” something delici-”ous”

7. Arrhenius (1859-1927) acids increase the hydrogen ion (H+) concentration in aqueous solution bases increase the hydroxide (OH-) concentration in aqueous solution

8. Modified Arrhenius acids increase the hydrogen ion (H+) concentration in aqueous solution however because the hydrogen ions are volatile they immediately become hydrated to form H3O+

9. Hydrogen Ions H atom = 1 proton, 1 electron H+ ion = 1 proton Therefore hydrogen ion = bare proton

10. Hydronium Ion protons are strongly attracted to the negative end of very polar water molecules H2O + H +  H3O +

11. H + = H3O + Because we don’t know the exact ratio of water to hydrogen molecules we take H3O + to mean hydrogen ions in water (aqueous)

12. pH Scale measures the relative acidity of a solution pH = “potency power of hydrogen (as hydronium)” logarithmic scale usually from 0-14

13. pH = -log 10 [H3O + ] [H3O + ] = 10 -pH

14. Example 1 What is the pH of HCl with a concentration of 8.93x10 -3 M?

15. Exxample 2 What is the pH of a solution of hydrofluoric acid created by adding 0.500g into 2.00L water?

16. Example 3 What is the concentration of a monoprotic acid with a pH of 12.22?