1. Think First 1.Get a chemistry text book and finish problems 42-57, pp. 328-337. 2.When you finish, show me your work. 3.Finish by _______ 4.If you finish early, begin the pink homework handout titled “Calculating Empirical and Molecular Formulas.” Study session after school on Thursday The mole test next class Formal lab due 4/12, 15

2. Hydrates A compound with a specific number of water molecules bound to its atoms –Example: CuSO 4 5H 2 0 Copper(ll) sulfate pentahydrate –How can you determine the formula for a hydrate? Read page 339 in the chemistry text.

3. Most Important Part: Show all your mathematical work for: Calculate the formula of the hydrate (Analyze and Conclude Question #1) Calculate Percent Error (Analyze and Conclude Question #4) In your composition book record: A hypothesis A data table A bar graph showing mass or moles before and after heating Any differences between the procedure in the book and your procedure Questions 1-5 in Analyze and Conclude on page 343 A conclusion (connect to hypothesis, error analysis, importance, future plans) Read Lab Directions First Do Lab and Collect Data Finding the Formula of the Hydrate Lab Objective: Use your knowledge of moles to find the formula of a hydrate.

4. The Mole Unit Exam Quiz on Friday/Monday over: –Calculating the number of moles, mass, or particles given the number of moles, mass or particles Calculating the molar mass of a compound How to set up the problem and show all your work –Calculate the percent composition of a compound from percentages of elements in a compound –Calculate the molecular formula –Calculate the formula of a hydrate given the number of grams of the hydrated compound and the number of grams of water released.