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. Lab Questions 1) Why must the electrodes on the conductivity...
Image transcription text
Lab
Questions
1) Why must the electrodes on the conductivity apparatus, as well as all the beakers, be rinsed with
distilled water after each conductivity test?
2) Why is distilled water a weaker conductor than tap water?
3) Why does solid sodium chloride act as a non-electrolyte while an aqueous while an aqueous NaCl
solution acts as a strong electrolyte?
4) Classify each of the following as non-ionized, partially-ionized, or ionized.
Write each compound as it exists in aqueous solution e.g. NaCl (aq) > Na (aq) + CI (aq)
HCI (aq) - a strong acid
Ca(OH)2 (aq) - a strong base
HC2H3 02 (aq) - a weak acid
Ba(OH)2 (aq) - a weak base
5) For the chemical reaction
H2SO4 (aq) + 2 NaOH (aq) > Na2SO4 (aq) + 2 H20 (1)
Write the complete ionic equation:
Write the net ionic equation:
6) For the chemical reaction
KNO3 (aq) + Nacl (aq) > NaNO; (aq) + KCI (aq)
Write the complete ionic equation:
Write the net ionic equation:
3
Image transcription text
Name:
Chem 9, Section:
Lab Partner:
Experiment Date:
Electrical Conductivity of Aqueous Solutions
Conductivity Testing - Evidence for Ions in Aqueous Solution
Solution
Observations:
Conductivity
Strong, Weak, or
Ionized,
Non-electrolyte
Partially
red LED | green LED
ionized, or
Non-ionized
examples:
LiOH (aq)
red bright, green dim
high
strong electrolyte
ionized
HNO2 (aq)
red dim, green off
low
weak electrolyte
partially ionized
methanol (1)
red off, green off
none
non-electrolyte
non-ionized
distilled water,
H2O (1)
tap water,
H20 (1)
solid sodium chloride,
NaCl (s)
sodium chloride
solution, NaCl (aq)
solid calcium
carbonate, CaCO3 (s)
calcium carbonate
solution, CaCO3 (aq)
acetic acid,
HC2H302 (aq)
Answer & Explanation
Solved by verified expertAnswered by CarloAgosto on coursehero.com
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