Lab Report to get Experiment #10
Stoichiometry of your Precipitation Response
Student's Name ____________________
Date of Experiment ___________
Time Report Submitted _________________
Instructor Changes: Weigh out about 1 . several g of CaCl2·2H2O and record the mass to +/- 0. 1 g (for case 1 . 6 g, 1 . 7 g, or 1 . 8 g). We have made this change in order that you have 2 sig figs in subsequent calculations. Have you made virtually any changes to the process? Please clarify:
Data Desks and Observation: Fill out the information sheet (below) for the experiment and submit with this form. Have careful notes during this test. Include some of the steps in which you might have lost test or lost confidence inside your technique. Write the complete well balanced equation. Make use of subscripts correctly by using the application bar or perhaps you will lose a spot. (2 points) Calculations: (10 points) for all those calculations entertain work by using a table to demonstrate the unit factor method for complete credit. Range from the correct significant figures through your data. #1 has an example for you. Record all answers in the table below.
1 ) Calculate the amount of moles of CaCl2·2H2O in the mass you weighed away and record in the desk below.
Element (molar mass)
_____ g CaCl2·2H2O
___ skin moles CaCl2·2H2O
Note: CaCl2·2H2O is usually an example of a hydrate, the 2 water substances are mounted on the crystal structure from the compound. When ever determining the molar mass, add the mass of 2 water molecules to the mass of the CaCl2.
2 . Through the balanced formula calculate the number of moles of Na2CO3 instructed to react completely with the CaCl2·2H2O and record in the table. (See lab, page seventy nine for example) Prepare a table.
3. Compute the number of grams of Na2CO3 to weigh out from the volume of moles in step 2 . Make a table.
four. Calculate the number of grams of CaCO3 that are expected to become produced. This really is your assumptive yield....