Thursday, April 16th, 2026 (SILVER)

Objectives:

1. Students will be able to calculate the Molarity of a solution.

2. Students will be able to calculate the mass of solute necessary to make a solution of known concentration.

3. Students will experimentally determine the Molarity of three different solutions made in a laboratory investigation.

Warm-Up: 

1. Define the following: solute, solvent, solution and give an example of each.

2. Compare/Contrast solutions, colloids, and suspensions.

3. What mass of Calcium Chloride (110.98 g/mol) would be needed to make 2,375 mL (1mL = .001L) of a .7500 M solution?

4. What would be the Molarity of a solution that contains               575.0 g of Copper (III) Iodide (444.25 g/mol)dissolved to make 750.0 mL (1mL = .001L) of solution?

5. If the mass of a solution created in the lab is measured to be 78.2 grams and the density is known to be 2.35 g/mL, what would be its volume? (hint: use the density as a conversion factor).  

Daily Plan:

1st Half of Class

1. Lab- Molarity Activity (collect data)

2nd Half of Class

2. Go over Molarity Practice

Homework:

1. Complete HWQ- Limiting Reagents by midnight (Tonight)

2. Complete Molarity Activity (E.O.P 4/22)

3. Complete HWQ- Molarity by midnight (4/27)