[jtwain2007]

How and why would the solutes salt, sugar, baking soda, and rubbing alcohol alter the boiling point of water?

When we were conducting our testing, we go the following results:

Plain Water
Trial 1: 100 degrees C
Trial 2: 100 degrees C
Water and NaCl
Trial 1: 106 degrees C
Trial 2: 105 Degrees C
Water and Table Sugar
Trial 1: 104 degrees C
Trial 2: 103 degrees C
Water and Isopropyl Alcohol
Trial 1: 102 degrees C
Trial 2: 103 degrees C
Water and Baking Soda
Trial 1: 103 degrees C
Trial 2: 103 degrees C

I'm just confused by the concept that explains these results.

[billnotgatez]

Forum rules require you show your work so far so we can help you.
Spoon feeding answers is not our method.
Please read forum rules - see the link near the top of the page.

you modified yur post after I had posted and it becomes confusing to those who view afterward.
Please read forum rules.

[billnotgatez]

WIKI and GOOGLE can be your friends.

I would think this link would help
http://en.wikipedia.org/wiki/Boiling-point_elevation

Please read forum rules

[mkurek]

The vapor pressure of a solution is always less than that of the pure solvent. So then the boiling point of a solution will always be higher than that of the pure solvent.

There is an equation to predict boiling point elevation: T=Km

Where K is the boiling point constant, and m is molality, and T represents the change in boiling point so to calculate the new boiling point you have to add T to the boiling point of the pure solvent.

So water has a K of about .5 and a boiling point of 100 C. Let's say we make a 1 molal solution.

T = (.5)(1) = .5

100 + .5 = 100.5

Hope that helps give you a push in the right direction!