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A 1956 dime is made of a silver-copper alloy and has a mass of 2.490 g. The dime was dissolved in pitric acid and a blue solution remained. The solution was quantitatively transferred to a 100-mL volumetric flask and brought to volume with water. (a) A 50.00-mL portion of the solution was reacted with excess sodium chloride solution. The precipitate formed, AgCl, was filtered, washed, and dried. The mass of the precipitate was found to be 1.375 g. (i) Write the net ionic equation for the reaction of the silver ion with sodium chloride. (ii) Determine the mass of silver in the precipitate. (iii) What is the percent silver in the dime?

A 1956 dime is made of a silver-copper alloy and has a mass of 2.490 g. The dime was dissolved in pitric acid and a blue solution remained. The solution was quantitatively transferred to a 100-mL volumetric flask and brought to volume with water. (a) A 50.00-mL portion of the solution was reacted with excess sodium chloride solution. The precipitate formed, AgCl, was filtered, washed, and dried. The mass of the precipitate was found to be 1.375 g. (i) Write the net ionic equation for the reaction of the silver ion with sodium chloride. (ii) Determine the mass of silver in the precipitate. (iii) What is the percent silver in the dime?

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter6: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 66E: You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into...
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FREE-RESPONSE QUESTIONS Calculators can be used in this section. A periodic table anda formula chart with constants are provided at the back of this book. 1. A 1956 dime is made of a silver-copper alloy and has a mass of 2.490 g. The dime was dissolved in nitric acid and a blue solution remained. The solution was quantitatively transferred to a 100-miL volumetric flask and brought to volume with water. (a) A 50.00-mL portion of the solution was reacted with excess sodium chloride solution. The precipitate formed, AgCI, was filtered, washed, and dried. The mass of the precipitate was found to be 1.375 g. (i) Write the net ionic equation for the reaction of the silver ion with sodium chloride. (ii) Determine the mass of silver in the precipitate. (iii) What is the percent silver in the dime? Absorbance of Copper(II) Nitrate Solution 1.0 0.9 0.8 0.7 y = 0.17x - 0.0062 0.6 0.5 0.4 0.3 0.2 0.1 0.00 1.00 2.00 3.00 4.00 5.00 6.00 Concentration (mg/mL) Copper(II) Nitrate Standard Curve Concentration (mg/mL) Absorbance 5.00 0.843 4.00 0.672 3.00 0.507 2.00 0.336 1.00 0.161 (b) A 1.5-mL portion of the remaining solution in the volumetric flask was analyzed with a UV-Vis spectrophotometer at 740 nm and the absorbance was 0.420. Calibration curve data and a graph are presented above. (i) What is the copper(II) ion concentration in the solution? (ii) Calculate the percent silver in the dime. Absorbance
Transcribed Image Text:FREE-RESPONSE QUESTIONS Calculators can be used in this section. A periodic table anda formula chart with constants are provided at the back of this book. 1. A 1956 dime is made of a silver-copper alloy and has a mass of 2.490 g. The dime was dissolved in nitric acid and a blue solution remained. The solution was quantitatively transferred to a 100-miL volumetric flask and brought to volume with water. (a) A 50.00-mL portion of the solution was reacted with excess sodium chloride solution. The precipitate formed, AgCI, was filtered, washed, and dried. The mass of the precipitate was found to be 1.375 g. (i) Write the net ionic equation for the reaction of the silver ion with sodium chloride. (ii) Determine the mass of silver in the precipitate. (iii) What is the percent silver in the dime? Absorbance of Copper(II) Nitrate Solution 1.0 0.9 0.8 0.7 y = 0.17x - 0.0062 0.6 0.5 0.4 0.3 0.2 0.1 0.00 1.00 2.00 3.00 4.00 5.00 6.00 Concentration (mg/mL) Copper(II) Nitrate Standard Curve Concentration (mg/mL) Absorbance 5.00 0.843 4.00 0.672 3.00 0.507 2.00 0.336 1.00 0.161 (b) A 1.5-mL portion of the remaining solution in the volumetric flask was analyzed with a UV-Vis spectrophotometer at 740 nm and the absorbance was 0.420. Calibration curve data and a graph are presented above. (i) What is the copper(II) ion concentration in the solution? (ii) Calculate the percent silver in the dime. Absorbance
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