 Find
the popsicle stick with your name on it and
sit there
 Put your Net Ionic Reaction lab in the basket
 Take out your notes from last night
 Work on the following with your table:
• What volume (in mL) of a 0.150 M HNO3 solution will
completely react with 35.7 mL of a 0.108 M Na2CO3
solution according to the following balanced chemical
equation:
• Na2CO3(aq) + 2HNO3(aq) –> 2NaNO3(aq) + CO2(g) + H2O(l)
• If you finish, calculate the mass (in grams) of carbon
dioxide that forms
 Substances
that dissolve in water to form
charged particles are called electrolytes
• Strong electrolytes dissolve a lot – lots of charged
particles
 Examples: NaCl, HCl and NaOH (all strong acids and
bases), all soluble ionic compounds
• Weak electrolytes dissolve a little – only a few
charged particles
 Weak acids and bases (e.g. HCH3COO)
• Nonelectrolytes don’t form charges at all
 Examples: sugar, AgCl
 Take
15 minutes to read the background
information and formulate a plan
• You need to determine what the murder weapon
was and what its molarity is
 Work
with the other two people at your
table
 By the end of the day today, you should
know the identity of the murder weapon
(not the concentration)
 Brainstorm
how you will determine the
molarity of the murder weapon
 Section 4.6 – due Monday
 Review questions 1-13 due Tuesday (grab
one from on top of the projector before you
leave!)
 Create
a particle view for the following
molar solutions. Begin with the 2.0 M
solution containing 20 particles.
• 2.0 M HCl
• 1.0 M HCl
• 0.5 M HCl