Formal Report (Be sure to
double space your report).
1.
Title page – Include name, expt title, instructor name, date, and copy the grading
rubric from the right onto the page.
(I will fill in the scores, you donÕt need to do that!)
2.
Introduction – from lab handout
a.
Name the three principal bond types.
b.
What is the essential characteristic of a
solution
that is
i)
A nonconductor
ii)
A good conductor
iii)
A poor conductor
c. Define the following terms and tell what kind
of bonding is expected in solutes that are
i)
Nonelectrolytes
ii)
Strong electrolytes
d.
What is meant by dissociation and what is
an example of a substances that dissociates?
e.
What is the meaning of the term
ÒhydrationÓ when used to describe what happens to an electrolyte which is
dissolved in water?
f.
What can be inferred about the degree of
ionization or dissociation of a substance that is a weak electrolyte?
3.
Procedure - (referenced correctly)
Summarize how you conducted the experiment because the handout did you have
concrete instructions, if you did not already do this in your lab pages. Make sure that another Chem 141 student could follow your directions!
4.
Data and Results section – Generate
a table summarizing the data gathered in the experiment. The table in the lab handout would work
nicely and it may be found in word format on my website. In addition include the following:
Part
1
o
Write the equation for the reaction that
forms the few (but important) ions in pure water.
o
Write an equation to describe the
formation of ions in aqueous acetic acid.
Part
3
o
Include the equations for the reactions
of CaCO3 and zinc with acetic acid and hydrochloric acid.
Part
4
o
Write the conventional equation, total
ionic equation, and net ionic equations for each of the processes observed
5. Discussion - Discuss any errors that might have
occurred during the experiment and how they may have affected your data. If
any
incorrect/unexpected results were obtained give the correct/expected results
and what may have happened. Such errors
could be
contamination; amount of surface area used on electrodes, amount of water used
for making aqueous compounds
etcÉAlso address
the following in the discussion
Part
1
o
Why is tap water more conductive than
distilled water?
o
Why does acetic acid form ions when it is
dissolved in water but not when it is in the pure (glacial) form?
o
The models of solid NaCl
describe it as consisting of Na+ cations
and Cl- anions. If this is the case, why is NaCl(s)
not an electrolyte?
o
Explain the distinctly different behavior
in the conductivity of NaCl(s) and NaCl(aq).
o
Explain the different behavior in the
conductivity of KClO3(s) and KClO3(l).
Part
2
o
Why is the conductivity of HCl different in the two solvents? What causes this difference?
Part
3
o
Discuss any correlation between the rates
of the chemical reactions of 6M acetic acid and 6 M hydrochloric acid and the
conductivities observed for acetic acid and hydrochloric acid in part 1?
Part
4
o
Explain any changes in conductivity you
detected for each reaction.
6.
Conclusions – Did you achieve your
objective? Explain briefly. This should be 2 or 3 sentences
7.
Post lab questions – hand write the
answers to these neatly on the pages provided
8.
Original data etc from the lab book.