1. Day 71 Notes (Ch. 17 & 20)
Electrolytes,
Acids and Bases

2. Electrolytes: Solutions that conduct electrical current easily.
Aqueous solutions of acids and bases are electrolytes.
Ionic solids that dissolve in water are electrolytes.

3. NaCl(s)  Na+(aq) + Cl-(aq)
Dissociation: Water surrounds ions and dissolves them.
Dissociation equation:
NaCl(s) 
Na+(aq) + Cl-(aq)

4. Weak Electrolyte: Partial Ionization.
Strong Electrolyte:
100% or nearly 100% dissociated.
Ionic compounds that dissolve in water conduct electricity easily because ions can move in solution.
Weak Electrolyte: Partial Ionization.
Ionic compounds that partially dissolve in water do not conduct electricity very well because only about 5% or less of the ions dissociate.
Are poor conductors of electricity

5. Nonelectrolyte: Does not dissolve in water.
Covalent or nonpolar substances are nonelectrolytes because they do not dissociate to form ions when dissolved in a solution.
Nonelectrolytes do not conduct electricity (Example: Sugar water)

6. Electrolytes: The ability of a solution to conduct an electric current.
The ammeter measures the flow of electrons (current)
through the circuit.
If the ammeter measures a current, and the bulb
glows, then the solution conducts. (Electrolyte)
If the ammeter fails to measure a current, and the
bulb does not glow, the solution is non-conducting. (Nonelectrolyte)

7. General definition:
Acids: Produce hydrogen ions, H+ , when dissolved in water.
Bases: Produce hydroxide ions, OH-, when dissolved in water.

8. Dissociation of an AcidCl Cl H H
C l H
Dissociation
equation.
HCl 
H+ + Cl-
General
Dissociation
equation.
HA 
H+ + A-
A- represents the anion

9. Acid-Base Neutralization+
Base 
Water +
Salt
HCl +
NaOH 
HOH
H2O +
NaCl

10. Some Properties of Acids
Acids taste sour
Acids react with certain metals to produce
hydrogen gas.
2 HCl(aq) + Mg(s)  H2(g) + MgCl2(aq)
Acids change the color of indicators
Blue litmus turns red
Phenolphthalein turns colorless
Methyl orange turns red

11. Acids Effect on Indicators
Blue litmus paper turns red in contact with an acid.

12. Bases Effect on Indicators
Red litmus paper turns blue in contact with a base.
Phenolphthalein turns purple in a base.

13. Neutral solutions
Red litmus stays red.
Blue litmus stays blue.

14. pH Indicators and their ranges

15. Hydro_______ic acid Naming Acids Acids without oxygen: HF =
Hydrofluoric acid
HCl =
Hydrochloric acid
HBr =
Hydrobromic acid
HI =
Hydroiodic acid
H2S =
Hydrosulfuric acid
HCN =
Hydrocyanic acid
CN- = cyanide anion

16. Naming Acids H+ + (anions with oxygen)
Acids with oxygen: “ate-ic ite-ous”
Anion name Acid name
____ate ____ic acid
___ite ___ous acid
HNO3 =
Nitr__?__ acid
Anion NO3-1 = nitrate
Nitric acid
HNO2 = Nitr__?__ acid
Anion NO2-1 = nitrite
Nitrous acid

17. Naming Acids H+ + (anions with oxygen)
Formula H+ with Anion Acid name
H2SO4
2H+ + SO42- = sulfate
Sulfuric acid
H2SO3
2H+ + SO32- = sulfite
Sulfurous acid
HC2H3O2
H+ + C2H3O2-1 = Acetate
Acetic acid
H2CO3
2H+ + CO32- = Carbonate
Carbonic acid
H3PO4
3H+ + PO43- = Phosphate
Phosphoric acid

18. Naming Acids H+ + (series of Cl and O)
Formula H+ with Anion Acid name
HCl
H+ + Cl = Chloride
Hydrochloric acid
HClO
H+ + ClO-1 = hypochlorite
Hypochlorous acid
HClO2
H+ + ClO2-1 = Chlorite
Chlorous acid
HClO3
H+ + ClO3-1 = Chlorate
Chloric acid
HClO4
H+ + ClO4-1 = perchlorate
Perchloric acid
Hypo = less oxygen
Per = more oxygen

19. Naming Bases Same method as naming ionic compounds
Formula Cation with OH- Base name
NaOH
Na+ + OH-
Sodium hydroxide
(Lye)
KOH
K+ + OH-
Potassium hydroxide
Ca(OH)2
Ca OH-
Calcium hydroxide
(Lime)
Mg(OH)2
Mg OH-
Magnesium hydroxide
(Milk of magnesia)
Al(OH)3
Al OH-
Aluminum hydroxide
NH3
(No ions)
Ammonia
(common name)
Molecules that contain nitrogen are weak bases.

20. Acids Have a pH less than 7

21. Bases have a pH greater than 7