Your second reasoning part,
because salt (as an ionic compound) has very low volatility
is not exactly right.
Table salt in its pure form at room temperature is a crystalline solid owing to its ionic character and is much less volatile than a water (liquid), that by itself need not mean that when you add this to water, it should share this property with water. To be more precise there are a handful of ionic salts that isn't even soluble in water, implying that they don't share their low volatility nature with water.
A more accurate explanation would be in terms of
- Types of bonding involved (for ionic solutes only):
Water molecules in its liquid state is bound by Hydrogen bonding. But when you add soluble salts, because these are ionic (localized non zero charge) it introduces a new kind of bonding called Ion-Dipole Bonds. To cut the story short, since this is also a stabilizing / attracting bond (in fact ion-dipole bond is stronger than Hydrogen Bond) that adds to already present Hydrogen Bonding, it essentially leads to a stronger attractive force that holds water molecules together and so making it harder for them to let go and vaporize. And hence the reason why Brine has lower volatility.
- Surface area exposed to atmosphere:
Here the essential idea is that, evaporation happens only at the surface. Also, solute molecules being more stable in soluble forms donot tend to vaporize when put in a solvent. Keeping these in mind, adding solute decrease the surface area of solvent exposed to atmosphere (or in general a lower pressure region) and so now there are lesser number of solvent molecules evaporating at a time, hence lower volatility.
Before I say anything, I should clarify that I am nowhere near a chemist, its been quite a long time since I handled any sort of equipments. So I have no idea of the precautions necessary/error associated with the various instruments.
Assuming that everything else is foolproof and the physics part is the only missing link - all I can say is about your temperature measurement part. If you measured the temperature 102.6 while the Bunsen burner is burning, its likely that you will get a wrong higher reading.
The idea is this - you have a heat source running at one end and a heat sink at the other end. Now what you are essentially measuring with a thermometer is the Temperature of the solution at Thermal equilibrium and NOT the BP. The reason for this is that even though the liquid solution can only attain its BP temperature, the area close the the burner would be steaming, now steam can attain a lot more temperature (maybe even close to temperature of the burner). So if you measure the temperature while keeping the burner running, what you are effectively measuring is sort of the average temperature of water and the steam (since the burner is continuously producing steam) and naturally its would be higher.
What I suggest you do is to give enough time for the steam to get out, which can only happen if you turn off the burner. Now you wouldn't have to worry about the water getting cooled down in this interval since water have way to high thermal heat capacity that there wouldn't be significant change during this interval.
Now assuming this is the case, I have a fairly good idea on how I would overcome it. I could post it here, but since you are doing a research, I don't want to ruin your experience, so I would highly appreciate it if you come up with a solution to this. Does that sound fair? I suggest that you come up with an idea, edit your original OP and post it there and then maybe tag me in a comment or something.