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A solution contains Cr* and Mg²+. The addition of 1.00 L of 1.53 M NaF solution is required to cause the complete precipitation of these ions as CrF3 (s) and MgF,(s). The total mass of the precipitate is 49.8 g . You may want to reference (Pages 331 - 336) Section 8.5 while completing this problem. Part A Find the mass of Cr+ in the original solution. „3+ 9.25 m = g Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining First, write balanced precipitation reactions showing the formation of the two solids. Use the mole ratios to set up an equation relating the moles of each solid back to the number of moles of F added. This should give you one equation with two variables. If you consider the number of moles of CrF3 to be x and the number of moles of MgF2 to be y, then you can relate the mass of each to the mass of the sample using their molar masses. This will give you a second equation with two variables. Solving both equations simultaneously will give you the number of moles of one of the solids, which can then be converted to the mass of Cr3+.

A solution contains Cr* and Mg²+. The addition of 1.00 L of 1.53 M NaF solution is required to cause the complete precipitation of these ions as CrF3 (s) and MgF,(s). The total mass of the precipitate is 49.8 g . You may want to reference (Pages 331 - 336) Section 8.5 while completing this problem. Part A Find the mass of Cr+ in the original solution. „3+ 9.25 m = g Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining First, write balanced precipitation reactions showing the formation of the two solids. Use the mole ratios to set up an equation relating the moles of each solid back to the number of moles of F added. This should give you one equation with two variables. If you consider the number of moles of CrF3 to be x and the number of moles of MgF2 to be y, then you can relate the mass of each to the mass of the sample using their molar masses. This will give you a second equation with two variables. Solving both equations simultaneously will give you the number of moles of one of the solids, which can then be converted to the mass of Cr3+.

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...
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A solution contains Cr* and Mg²+. The addition of 1.00 L of 1.53 M NaF solution is required to cause the complete precipitation of these ions as CRF3 (s) and MgF,(s). The total mass of the precipitate is 49.8 g . You may want to reference (Pages 331 - 336) Section 8.5 while completing this problem. Part A Find the mass of Cr+ in the original solution. ΑΣφ 9.25 m = Submit Previous Answers Request Answer Incorrect; Try Again; 4 attempts remaining First, write balanced precipitation reactions showing the formation of the two solids. Use the mole ratios to set up an equation relating the moles of each solid back to the number of moles of F added. This should give you one equation with two variables. If you consider the number of moles of CrF3 to be x and the number of moles of MgF2 to be you can relate the mass of each to the mass of the sample using their molar masses. This will give you a second equation with two variables. Solving both equations simultaneously will give you the number of moles of one of the solids, which can then be converted to the mass of Cr³+. Y, then
Transcribed Image Text:A solution contains Cr* and Mg²+. The addition of 1.00 L of 1.53 M NaF solution is required to cause the complete precipitation of these ions as CRF3 (s) and MgF,(s). The total mass of the precipitate is 49.8 g . You may want to reference (Pages 331 - 336) Section 8.5 while completing this problem. Part A Find the mass of Cr+ in the original solution. ΑΣφ 9.25 m = Submit Previous Answers Request Answer Incorrect; Try Again; 4 attempts remaining First, write balanced precipitation reactions showing the formation of the two solids. Use the mole ratios to set up an equation relating the moles of each solid back to the number of moles of F added. This should give you one equation with two variables. If you consider the number of moles of CrF3 to be x and the number of moles of MgF2 to be you can relate the mass of each to the mass of the sample using their molar masses. This will give you a second equation with two variables. Solving both equations simultaneously will give you the number of moles of one of the solids, which can then be converted to the mass of Cr³+. Y, then
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