[Borek]

So, a high concentration of a strong electrolyte can produce a low conductivity reading.

In some very specific cases. You will need a strong electrolyte made of very large ions.

If I took my probe and measured it with a vial of an unknown substance (0.02000 M Unknown A) with equal volume and concentration, as a previously measured solution, in this case, the strong electrolyte, potassium chloride (0.02000 M KCl), and it returned a value range within the scope of the previously measured strong electrolyte (k = 2949.6 uS/cm), would it be safe to assume, that the unknown substance, then, classifies as a strong electrolyte?

If you know that concentrations are comparable and conductivities are comparable then yes, it would be a valid conclusion.

But, with your statement taken into consideration, does an individual run the risk of mis-labeling an unknown solution as a strong or weak electrolyte after measuring it with the probe, because of your quote: "... strong electrolyte made of very large ions can have very low conductivity even at high concentrations." Thus, being labeled as a weak electrolyte?

Yes, there is such a risk.

Since a non-electrolyte has no range of values, is there a particular range for strong or weak electrolytes to help distinguish it?

It could be possible to define such a range, but I have never seen it done. There is no need for that, as we usually can use other analytical methods to gain more knowledge about the substance and classify it. Conductivity alone is not enough.

[MathisFun]

It could be possible to define such a range, but I have never seen it done. There is no need for that, as we usually can use other analytical methods to gain more knowledge about the substance and classify it. Conductivity alone is not enough.

Hmm... the course has limited the use of methodology at this time. I really appreciate your input in this thread. It has gone beyond the scope of what was being asked of the student, as I made additional inquiries. Again, thanks.

[MathisFun]

My last burning question on this subject: 

The non-electrolyte, distilled water, is usually used to prep a conductivity probe, in this case, soaking it in a beaker with distilled water for 30 minutes. In doing this, it neutralizes the charge at the end of the probe, just in case, it attracted charges, which may interfere with its reading.

Would another non-electrolyte, such as, C12H22O11 (sucrose), work as well?

[Borek]

Water has a very specific properties that make it the better choice. High dielectric constant and small polar molecules mean ions are easily dissolved, they would not leave the glass surface in most other solvents.

[Arkcon]

I suppose it would, but you're going to run up against a physical problem.  Selective ion electrodes rely on a special porous surface, a glass "membrane", if you want to make an analogy.  Strange molecules, like sucrose, or non-ionic detergents like Triton-X10, or soluble proteins can "clog" the pores (for lack of a better term,) and make the electrode behave badly.

[MathisFun]

I see. Thanks for the follow-up. I think my questions for electric conductivity have been answered.

[MathisFun]

Hello, here is the results of my lab report. I appreciate all the input that was given to me by various members. There were some interesting finds...

It turns out that tap water is considered a 'weak electrolyte' because of the existence of a small amount of ions.

In comparing a conductivity probe calibration curve in a graph with a strong electrolyte and weak electrolyte, it turns out that both, when measured with different levels of concentration, would yield the same results. Here is a linked graph, as a visual representation:
http://i46.tinypic.com/2gui8g3.jpg

For the strong electrolyte, it would look similar to the linked graph, while for the weak electrolyte, the graph would also look the same, but the y-values for the calibrated values would be of a lower value, more like this,

strong electrolyte: 0-9000
weak electrolyte: 0-900

therefore, both graphs would be directly linear. The idea that the graph would be non-linear made sense, but I suppose, this isn't the answer that was sought.

Lastly, when asked what a graph of conductivity versus concentration on a non-electrolyte would look like, here is my answer, as previously posted:
If... a non-electrolyte, such as, C12H22O11 (sucrose), were to be used, it would produce the same value as distilled water, with 0.0 uS/cm... never chart beyond this value, (with no line being produced), and staying fixed at (0,0) on the graph.

It was actually a flat line, crossing through the x-axis. It was something I considered, but felt that my response at the time was stronger, since the reading for distilled water was at 0.0 uS/cm.

Again, thanks for all the input provided in this report. I really appreciate it, as it expanded beyond the scope of what was being taught.