1. Acids produce Hydrogen ions in solution
2. Hydrogen ions (H+ ) aka Hydronium (H3O+) aka Proton
3. Acids are also known as Proton donors. They give an H to another species
4. Acids react with Metals to produce a salt soln and hydrogen gas (H2)
5. Table K lists acids. Hydrochloric, Sulfuric, and Nitric are strong acids the rest are weak. Acetic acid is an organic acid.
6. Monoprotic acids have 1 acidic hydrogen. Diprotic 2, Triprotic 3
7. Strong acids ionize completely, weak acids do not ionize completely this explains differences in strength.
8. Acids have a pH below 7
9. Electrolytes are solutions that conduct electricity because electrolytes contain mobile ions.
10. All acids, bases and salts are electrolytes. Strong acids are strong electrolytes etc.
11. Bases are metal hydroxides and ammonia.
12. Bases produce the hydroxide ion (OH-) in solution
13. Bases accept an H from an acid.
14. Alcohols are not bases.
15. Bases don’t react with metals. Drano is a base.
16. Ammonia is the only weak base on Table L.
17. The word alkaline refers to a base.
18. Bases have a pH above 7.
19. Salts are ionic compounds. They are strong electrolytes because they dissociate into ions when placed in water. This is referred to as dissolving.
20. PH measures the amount of hydrogen ion in solution. The more H+ the lower the pH.
21. When H+ = OH- the solution is neutral with a pH of 7.
22. Neutralization = Acids and bases react with each other to form a salt and water.
23. Titration experiments are performed to find the Molarity or Volume of an acid or Base. The formula is on Table T
24. When using a diprotic acid or dihydroxide base in a titration formula the molarity of the acid or base is doubled. H+ reacts with OH- in a 1 to 1 ratio to form water.
25. Table M lists acid base indicators. Be careful some indicators only work in the acid or base range and not both. Depending on the color you should be able to estimate pH. Remember the lab!!!
26. Here is a table with pH examples
pH [H+] [OH-] Molartiy of acid
2 1 x 10-2 1 x 10-12 0.01
9 1 x 10-9 1 x 10-5 0.000000001
Titration examples:
How many mL of 2.0 M NaOH is needed to neutralize 10 mL of 1.0 M HCl?
How many mL of 2.0 M Mg(OH)2 is needed to neutralize 10mL of 1.0 M HCl?