1. Section 4.5 Solution Stoichiometry

2. Determining concentration Making Solutions
In This Section:
Using Molarity
Determining concentration
Making Solutions
Direct Addition
Dilution
Solution Stoichiometry and Titrations

3. Stoichiometry so Far 2 HCl + CaCO3  H2O + CO2 + CaCl2
mol mol mol mol mol
g g g g g

4. Molarity Conversion Factor: mol <-> liters
A solution is 0.35 molar (3.5 mol/l) in NiCl2
Converting from Liters to Moles:
How many moles are contained in 450 mL of this solution?
Converting from Moles to Liters:
What volume of this solution contains 2.24 mol NiCl2?

5. Solution Stoichiometry

6. Determining Solution Concentration:
Molarity = mol solute/liter solution
What is the concentration of a solution made by dissolving 23.5 g NiCl2 into a volume of 250 mL?

7. Preparing Solutions: Direct Addition
How many grams of NiCl2 would you use to prepare 100 mL of a M solution?

8. Preparing Solutions: Dilution from a concentrated solution
How many mL of a 2.60 M NiCl2 solution would you use to prepare 100 mL of a M solution?

9. Titrations: The idea

10. Titrations: This week’s lab
Part 1. “Standardizing” a solution of base:
23.8 mL of an NaOH solution is used to neutralize
1.020 g H2C2O4-2H2O. What is the concentration of the NaOH solution?

11. Titrations: This week’s lab
Part 2. Determining the molar mass of an acid:
35.2 mL of the same NaOH solution is used to neutralize g of an unknown diprotic acid. What is the molar mass of the acid?