1. Acids and Bases

2. Properties of Acids Have a sour taste
Changes colors of substances called indicators
Aqueous Solutions are electrolytes ( conduct electricity)
React with metals: Zn + 2 HCl  ZnCl2 + H2
Reacts with carbonates: 2HCl + Na2CO3  2NaCl + H2O + CO2
Have at least one hydrogen atom attached to a negative ion.
Reacts with (-OH) to form water
pH below 7

3. Naming Acids Hydrogen comes first you know it’s an acid
The second part determines the name
Ends in “ide”… Acid name begins with hydro, the stem of the anion has the suffix “ic” and then acid is on the end
Ends in “ite”… The stem of the anion has the suffix “ous” and then acid is on the end
Ends in “ate”… The stem of the anion has the suffix “ic” and then acid is on the end
Practice problems 1-5 pg 579

4. Properties of Bases Have a bitter taste Changes colors of indicators
Feels slippery
React with (H+) to form water
pH above 7
No special naming structure just normal rules

5. Hydrogen Ions and Acidity
Hydrogen Ions from Water
Water self-ionizes
H2O + H2O  H3O+ + OH- or H2O  H+ + OH-
When water self-ionizes [H+] = [OH-] = 1.0 x 10-7
Kw = [H+][OH-] = (1.0 x 10-7)(1.0 x 10-7) = 1.0 x 10-14
Acid solutions-substance is added to water to increase [H+] so [H+] >1.0 x 10-7
Basic solutions-substance is added to water to increase [OH-] so [OH-] >1.0 x 10-7
Practice problems #6-7 pg 582

6. The pH Concept
pH is a measurement of the acidity of solutions. pH=-log [H+]
If pH>7 the solution is basic. If pH<7 the solution is acidic. If pH=7 the solution is neutral.
pOH is a measurement of the basicity of solutions. pOH=-log [OH-]
pH + pOH = 14. Also [H+][OH-] = 1.0 x 10-14
Practice problems #8-9 pg 586