1. Ch Acids & Bases

2. HCl + H2O  H3O+ + Cl– A. Definitions Acids
Ionize to form hydronium ions (H3O+) in water
HCl + H2O  H3O+ + Cl–

3. NH3 + H2O  NH4+ + OH- A. Definitions Bases
Dissociate or ionize to form hydroxide ions (OH-) in water
NH3 + H2O  NH4+ + OH-

4. A. Definitions Indicator
substance that changes color in an acid or base
Examples:
litmus - red/blue
phenolphthalein - colorless/pink
goldenrod - yellow/red
red cabbage juice - pink/green

5. B. Properties ACIDS BASES sour taste corrosive electrolytes
turn litmus red
react with metals to form H2 gas
bitter taste
corrosive
electrolytes
turn litmus blue
slippery feel

6. C. Uses ACIDS H3PO4 - soft drinks, fertilizer, detergents
H2SO4 - fertilizer, car batteries
HCl - gastric juice
HC2H3O2 - vinegar

7. C. Uses BASES NaOH - lye, drain and oven cleaner
Mg(OH)2 - laxative, antacid
NH3 - cleaners, fertilizer

8. A. Strong vs. Weak Strong Acid/Base 100% ions in water
strong electrolyte
HCl, HNO3, NaOH, LiOH - +
Weak Acid/Base
few ions in water
weak electrolyte
HC2H3O2, NH3 - +

9. B. pH Scale pH a measure of the concentration of H3O+ ions in solution
measured with a pH meter or an indicator with a wide color range 7
INCREASING
ACIDITY
NEUTRAL
BASICITY 14

10. pH of Common Substances
B. pH Scale
pH of Common Substances

11. A. Neutralization Reaction
Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.

12. A. Neutralization Reaction
ACID + BASE  SALT + WATER
HCl + NaOH  NaCl + H2O =
Neutralization does not always mean pH = 7.

13. A. Neutralization Reaction
KOH + HNO3  H2O + KNO3
Acid?
Base?
Salt?
HNO3
KOH
KNO3

14. B. Titration
standard solution
unknown solution
Titration
Process in which a standard solution is used to determine the concentration of an unknown solution.

15. B. Titration Endpoint (equivalence point)
Point at which equal amounts of H3O+ and OH- have been added.
Determined by…
indicator color change
dramatic change in pH