I have no idea where to even start with this problem on my pre-lab!

Question

For part of the experiment, you will need to prepare 100 mL of 0.025 M CH3CO2H, starting from commercial "glacial" acetic acid, which has a concentration of 17.4 M. This is best done by making two dilutions, in order to avoid either having to measure out an extremely small volume of glacial acetic acid, or having to make a very large volume of diluted acid. For example, you could measure out 1.00 mL of glacial acetic acid, dilute it to 50.00 mL in a 50 mL volumetric flask, and then take 7.2 mL of this solution, and it dilute it to 100.00 mL in a 100 mL volumetric flask.

Verify this procedure will result in 100 mL of 0.025 M acetic acid.

Part 2:
Devise a method similar to that in the previous question to make 100.00 mL of 0.025 M NH3, from concentrated ammonia, which has a concentration of 14.5 M?

Part 3:
Consider the conductance of the following 0.025 M solutions. Use the data to classify each solute as either a nonelectrolyte, a weak electrolyte, or a strong electrolyte:
Solute, conductance (mS), SE/WE/NE
A, 3.5, ?
B, 7.6, ?
C, 0.0, ?
D, 0.2, ?
E, 6.5, ?
F, 0.3, ?
G, 2.9, ?

Answer 1

a. 17.4 M x (1.00mL/50.00mL) = 0.348M
Then 0.348 x (7.2 mL/100 mL ) = 0.025M

b. Use a as a template.
c. I would call the 7.6 and 6.5 SE, the zeros are NE (of course) while 3.5 and 2.9 are WE. I don't know how you want to handle athe 0.2 and 0.3. Those could be non-electrolytes that had a small contamination OR they could be very weak solution of WE.

Answer 2

Thanks so much