Electrolytes and Solutions!

Learning Objectives!

• Review definitions of solution and electrolytes
• Can you create a particle diagram of a salt solution?
• Can you create two different concentrations of salt solutions and qualitatively demonstrate this difference?
• Can you mathematically show the difference in concentration and provide the calculations to justify it?

A solution is defined as a homogeneous mixture of 2 or more substances. An electrolyte is a substance that disassociates into ions when dissolved in water. 

An example of a solution would be salt water. 

We qualitively demonstrated the difference between two different salt solutions. These solutions contained different amounts of salt and water. One solution consisted of 100 mL of distilled water and 2.5 grams of salt. The other solution had a massive amount of distilled water at 600 mL and a mere .1g of salt. 

We then tested the electrolytes in the water by seeing if the solution would conduct electricity and how much of it. We used this scary looking thing with two prongs and a light bulb attached. The results produced are in the pictures below. 

Beaker with 100 mL of distilled water and 2.5 grams of salt.

This beaker obviously contained the 600 mL of water and .1 grams of salt! This solution was our attempt to create tap water. It was a bit difficult to create the same amount of light that the tap water did. You can compare our light to the tap water's light with the picture below!


                            Original 

Here is how we calculated our data to show the difference in concentration: REMEMBER WE WANT TO GET TO MOLES TO OBTAIN MOLARITY. MOLARITY= MOL/LITER

DIFFERENT MOLARITY = DIFFERENT CONCENTRATIONS