Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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
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...
See similar textbooks
icon
Related questions
Question

How do you solve for the wt% of Ca 2+ in the solution?

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:
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:
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Iodine Titrations
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS