CP CHEMISTRY
Solubility, Concentration, & Molarity Lab
Purpose:
Name: ___________________________________
____ period
To investigate the solubilities of several salts, determine what factors affect the
concentrations of such salt solutions, and perform molarity calculations.
Procedures and Observations:
Part 1: Solubility of Table Salt
1.
Go to: http://phet.colorado.edu/en/simulations/category/chemistry. Click on Salts and
Solubility simulation and click on Run Now!
2.
Familiarize yourself with how the simulation for Table Salt works. Once you are ready to
proceed, make sure you reset all for the simulation.
3.
Shake the container. What happens to the bound Na+ and Cl- ions as they enter the water?
______________________________________________________________________________
4.
Keep shaking the container. Is there a point at which no more sodium and chloride ions
will dissolve? How do you know?
______________________________________________________________________________
5.
What do we call a solution that has as many ions as it can hold? ______________________
6.
What happens if you add additional, solid NaCl after the maximum has been reached?
______________________________________________________________________________
7.
What happens when more water is added to a saturated solution?
______________________________________________________________________________
8.
What happens to the ions bound together as a solid when the solution’s volume is reduced?
_____________________________________________________________________________
Part 2: Concentration and Saturation
1.
Go to: http://phet.colorado.edu/en/simulations/category/chemistry. Click on the
Concentration simulation and click on Run Now!
2.
Familiarize yourself with the simulation. Move all the sliders and notice what happens as
solid solute is added and evaporation occurs.
CP CHEMISTRY, Solubility, Concentration, & Molarity Lab, page 2
3.
Put the concentration meter in the bottom of the beaker. Add solid solute to the water.
How does the concentration change as the solid solute is added? State two ways you
can determine how the concentration has changed.
__________________________________________________________________________
__________________________________________________________________________
4.
How does the concentration change as additional water is added to the container?
__________________________________________________________________________
5.
How does the concentration change as evaporation occurs?
__________________________________________________________________________
6.
How do you know when a solution is saturated?
__________________________________________________________________________
7.
When a solution is saturated, and additional solid solute is added, what happens?
__________________________________________________________________________
8.
Why do you think this is?
__________________________________________________________________________
9.
How does adding this additional solute change the concentration of the saturated solution?
__________________________________________________________________________
10.
How does evaporation change the concentration of a saturated solution?
__________________________________________________________________________
Part 3: Molarity
1.
Go to: http://phet.colorado.edu/en/simulations/category/chemistry. Click on the
Molarity simulation and click on Run Now!
2.
What is the equation for molarity?
CP CHEMISTRY, Solubility, Concentration, & Molarity Lab, page 3
3.
Familiarize yourself with how the simulation functions. Be sure to click on the show values
box.
4.
How can you determine if a solution is saturated? How does it appear in the simulation?
____________________________________________________________________________
5.
Determine the saturation concentrations for the following solutions in the data table below.
Write in the saturation concentration in the empty box next to each solution.
6.
Using the simulation and the cobalt(II) nitrate solution, complete the Molarity table below.
Moles of
Compound (mol)
Liters of Solution
(L)
Molarity of
Solution (M)
Moles of
Compound (mol)
Liters of Solution
(L)
Molarity of
Solution (M)
0.53
0.79
0.78
0.59
0.86
0.34
0.88
1.8
1.0
0.20
0.64
1.1
0.67
0.67
0.95
0.62
Conclusions and Calculations:
For questions 1-5, circle one of the choices provided in the statements.
1.
Adding pure water to a saturated solution (with no solids) would cause the concentration of
that solution to increase/decrease/remain the same.
2.
Adding pure water to a saturated solution (with some solids) would cause the concentration
of that solution to initially increase/decrease/remain the same.
3.
Adding a solid salt to a saturated solution causes the concentration of that solution to
increase/decrease/remain the same.
4.
Evaporation acting on an unsaturated solution causes the solution’s concentration to
increase/decrease/remain the same.
CP CHEMISTRY, Solubility, Concentration, & Molarity Lab, page 4
5.
Evaporation acting on a saturated solution causes the solution’s concentration to increase/
decrease/remain the same.
For the following questions, be sure to show all work!!
6.
Can you dissolve 0.35 moles of potassium permanganate, KMnO4, into 500 mL of water?
Why or why not? (Hint: use the data table in Part 3, Step #5)
7.
Can 1750 mL of water dissolve 4.6 moles of copper sulfate, CuSO4? Why or Why not?
8.
What is the solution concentration formed from 3.6 moles of NaCl dissolved in 1.3 L
of water?
9.
What is the solution concentration formed from 2.1 moles of BaCl2 dissolved in 1.9 L
of water?
10.
How many moles of solute are present in 0.75 L of a 0.89 M solution?