1. Types of Chemical Reactions and Solution Stoichiometry – Part 2
Chapter 4
Part 3
Types of Chemical Reactions and Solution Stoichiometry – Part 2

2. Calculations
All calculations must use factor label method or dimensional analysis
Ratio is NOT acceptable

3. Using Molarities in Stoichiometric Calculations

4. Using Molarity to Calculate Grams of Solute
SAMPLE EXERCISE How many grams of Na2SO4 are required to make L of M Na2SO4?
Plan: Use the definition of molarity to determine the number of moles of solute, and then convert moles to grams using the molar mass of the solute.
Solve: Determine moles of solute
Using Molar Mass to determine grams

5. Calculating Molar Concentrations of Ions
SAMPLE EXERCISE What are the molar concentrations of each of the ions present in a M aqueous solution of calcium nitrate?
Plan: Use the subscripts in the chemical formula of the compound to determine the relative concentrations of the ions.
Solve: The chemical formula for calcium nitrate is Ca(NO3)2. Because there are two NO3– ions for each Ca2+ ion in the compound, each mole of Ca(NO3)2 that dissolves dissociates into 1 mol of Ca2+ and 2 mol of NO3–. Thus, a solution that is M in Ca(NO3)2 is M in Ca2+ and 2  M = M in NO3–.

6. Acid – Base Titration
The analytical technique in which one can calculate the concentration of a solute in a solution.

7. Titration

8. Titration

9. Volumetric analysis
Titration –deliver a measured volume of a known concentration of titrant into a solution containing the analyte.
Titrant – solution of known concentration that is added
Analyte- solution of unknown concentration that can be analyzed
Measure the volume of titrant added to neutralize the analyte using a color indicator.
Titration - Use known volumes of each solution and known concentration of titrant to calculate the concentration of the analyte.

10. Acid Base Titrations
Equivalence point – stoichiometric equivalent quantities of acid and base
Indicator – chemical that changes color at the end point
Acid-base indicators change color at end point.
Indicator is chosen so end point corresponds to equivalence point of titration.

11. Using Mass Relations in a Neutralization Reaction
SAMPLE EXERCISE How many grams of Ca(OH)2 are needed to neutralize 25.0 mL of M HNO3?
Solution

12. Determining the Quantity of Solute by Titration
SAMPLE EXERCISE The quantity of Cl– in a municipal water supply is determined by titrating the sample with Ag+. The reaction taking place during the titration is below. The end point in this type of titration is marked by a change in color of a special type of indicator. (a) How many grams of chloride ion are in a sample of the water if 20.2 mL of M Ag+ is needed to react with all the chloride in the sample? (b) If the sample has a mass of 10.0 g, what percent Cl– does it contain?
Solution. (a) Plan: We begin by using the volume and molarity of Ag+ to calculate the number of moles of Ag+ used in the titration. We can then use the balanced equation to determine the moles of Cl– in the sample and from that the grams of Cl–.

13. Solution
(b) Solve:  
Comment: Chloride ion is one of the most common ions in water and sewage. Ocean water contains 1.92% Cl–. Whether water containing Cl– tastes salty depends on the other ions present. If the only accompanying ions are Na+, a salty taste may be detected with as little as 0.03% Cl–.

14. Conclusion
Use Molarity to calculate molarity and then use stoichiometry to determine moles or grams in a chemical reaction.
Use titration to neutralize solution of unknown concentration with color indicator. The titrant has known concentration and measured volume. Using stoichiometry, the unknown concentration can be determined.