The Experiment:
Mass Percent and Mole Solutions:
Create specific molar and mass percent solutions using sugar, salt, and kool-aid. Use the molar masses below for each material.
Assume one mole of Salt = 40.0g
Assume one mole of sugar = 100.0g
Assume one mole Kool-Aid = 2.0g
Molar Solutions: Create a 0.5 and a 1.0M solution for each of the three materials. To do this, measure out the necessary moles of each material for whatever size volumetric flask is being used. Be sure to first measure the mass of the solid; add the solid to the flask, then fill the volumetric flask with liquid. The equation for molarity is given below. Fill in the table below with the correct amounts for each material.
| Molarity | = |  |
moles of solute |  |
| total volume of solution (in Liters) |
Solid |
Molarity of Solution |
Volume of Flask (in Liters) |
Moles of Solid needed |
Mass of Solid added to flask |
Sugar |
0.5 |
|
|
|
Sugar |
1.0 |
|
|
|
Kool-Aid |
0.5 |
|
|
|
Kool-Aid |
1.0 |
|
|
|
Salt |
0.5 |
|
|
|
Salt |
1.0 |
|
|
|
Mass Percent Solutions: Using only Sugar, create a 5%, 10%, and 20% solution by mass. Create each solution using 100.0mL (100.0g is same thing) of water. Fill in the table below for each of the three mass%.
| Mass % | = | 100 | x | |
mass of solute | |
| mass of solute + mass of solvent |
Solution Type |
Mass of Solid Added (g) |
Mass of H2O added (g) |
Total mass of Solid + H2O mixed (g) |
Total Solution Volume after mixing (mL) |
Mass of 50ml of mixed solution (g) |
Solution Density (g/mL) |
5% |
|
100.0g |
|
|
|
|
10% |
|
100.0g |
|
|
|
|
20% |
|
100.0g |
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|
|
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