Prepare 20 mL of~1 M CaCl2. Because the CaClz solution will be used as an excess reagent to prepare a precipitate of Ca(103)2, it is not necessary to know its molarity with accuracy. An approximate solution prepared with non-volumetric glassware is sufficient. Using a balance, weigh out the calculated mass of CaCl2•2H2O into a tared 150-mL beaker. Record the actual mass of salt used below. The calculated and actual masses should agree to +0.1 g or better. Use a graduated cylinder to add 20.0 mL of distilled water to the flask. Stir the solution with a stirring rod or a stir bar and stir plate until the salt is fully dissolved. Since this solution was not made volumetrically, a better description of the concentration of a solution prepared in this manner is weight percent (wt%) units, calculated as (g solute/g solution) x 100%, where g solution = g solute + g solvent. Calculate and report the wt % of Ca2+ of this solution, assuming water has a density of 1.0 g/mL. 3.50 8 9 3.5099 Approximate mass of CaCl2-2H20 needed Actual mass of CaCl2•2H2O weighed Wt% Ca²+ in the solution Calculation:
Prepare 20 mL of~1 M CaCl2. Because the CaClz solution will be used as an excess reagent to prepare a precipitate of Ca(103)2, it is not necessary to know its molarity with accuracy. An approximate solution prepared with non-volumetric glassware is sufficient. Using a balance, weigh out the calculated mass of CaCl2•2H2O into a tared 150-mL beaker. Record the actual mass of salt used below. The calculated and actual masses should agree to +0.1 g or better. Use a graduated cylinder to add 20.0 mL of distilled water to the flask. Stir the solution with a stirring rod or a stir bar and stir plate until the salt is fully dissolved. Since this solution was not made volumetrically, a better description of the concentration of a solution prepared in this manner is weight percent (wt%) units, calculated as (g solute/g solution) x 100%, where g solution = g solute + g solvent. Calculate and report the wt % of Ca2+ of this solution, assuming water has a density of 1.0 g/mL. 3.50 8 9 3.5099 Approximate mass of CaCl2-2H20 needed Actual mass of CaCl2•2H2O weighed Wt% Ca²+ in the solution Calculation:
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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How do you solve for the wt% of Ca 2+ in the solution?
Transcribed Image Text:Prepare 20 mL of ~1 M CaCl2. Because the CaCl2 solution will be used as an excess reagent
to prepare a precipitate of Ca(IO3)2, it is not necessary to know its molarity with accuracy.
An approximate solution prepared with non-volumetric glassware is sufficient.
Using a balance, weigh out the calculated mass of CaCl2•2H2O into a tared 150-mL beaker.
Record the actual mass of salt used below. The calculated and actual masses should agree to
±0.1 g or better. Use a graduated cylinder to add 20.0 mL of distilled water to the flask. Stir
the solution with a stirring rod or a stir bar and stir plate until the salt is fully dissolved.
Since this solution was not made volumetrically, a better description of the concentration of
a solution prepared in this manner is weight percent (wt%) units, calculated as (g solute/g
solution) x 100%, where g solution = g solute + g solvent.
Calculate and report the wt
g/mL.
of Ca2+ of this solution, assuming water has a density of 1.0
3.50 8 9
3.5099
Approximate mass of CaCl2•2H20 needed_
Actual mass of CaCl2•2H2O weighed
Wt% Ca²+ in the solution
Calculation:
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