To Do

Finish reading Chapter 4.

Text homework for Chapter 4.

Quiz #2 on Friday, February 12

Lon-Capa assignment #3.
1
Exam
Tuesday, 2/16, 7:00-8:30 pm;
rooms online.
 Conflict exam; 2/16, 5:00-6:30 pm;
in 153 Mechanical Eng. Bldg. Sign
up in 367 Noyes Lab
 Review sessions


To be announced
2
Dissolving of an Ionic Compound
3
NaCl Dissolves
4
5
p129
6
p129
Solubility Rules
7
8
p130
Precipitation Reactions




Know how to use the solubility
rules (you will be given them on
the exam).
Know how to write equations from
reactants (ionic reactants).
Understand what solutions “look”
like at a very magnified level.
Be able to do stoichiometry
calculations.
9
Clicker Question
When lead(II) nitrate and potassium iodide are mixed,
which are the possible products?
1.
2.
3.
4.
PbI
PbI2
K(NO3)2
KNO3
a) 1 & 3
b) 1 & 4
c) 2 & 4
d) 2 & 3
10
Solubility Rules
Given:
Pb(NO3)2(aq) + 2KI(aq) → PbI2 + 2KNO3
PbI2 must be the solid.






Solubility Rules
Most nitrate salts are soluble.
Most salts of sodium, potassium,
and ammonium cations are
soluble.
Most chloride salts are soluble.
Exceptions: Ag+ and Pb2+.
Most sulfate salts are soluble.
Exceptions: Ca2+, Ba2+, and Pb2+.
Most hydroxide salts are only
slightly soluble. Soluble ones are:
Na+, K+, and Ca2+.
Most sulfide, carbonate, and
phosphate salts are only slightly
soluble.
11
Clicker Question
Which solution is
the most
concentrated?
(note: this is #90
from Chapter 4)
12
Practice Problems


You dissolve 10.0 g of NaCl in
150.0 mL of solution. Determine
the concentration in molarity.
Describe how to make 250.0 mL
of 0.100M NaOH from a stock
solution of 8.00M NaOH.
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