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Average % Chloride: Standard deviation: Show Calculations for Trial 1: a. Mass of Chloride, g b. % Chloride Questions: 1. When the unknown sample was dissolved in 100 mL water, 6 M nitric acid (HNO3) was used to acidify the solution. Why shouldn't any acid such as HCI and H₂SO4 be used in this process? 2. For Trial 1, how many grams of AgNO3 must be added to the solution to completely react with NaCl?

Average % Chloride: Standard deviation: Show Calculations for Trial 1: a. Mass of Chloride, g b. % Chloride Questions: 1. When the unknown sample was dissolved in 100 mL water, 6 M nitric acid (HNO3) was used to acidify the solution. Why shouldn't any acid such as HCI and H₂SO4 be used in this process? 2. For Trial 1, how many grams of AgNO3 must be added to the solution to completely react with NaCl?

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
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Activity No. 8 Determination of Chloride Ion Concentration by Gravimetry Gravimetric analysis is a method in quantitative analysis where an unknown sample is dissolved in an appropriate solvent, and the analyte is converted to an insoluble form or precipitation of a known compound and then weighing the precipitate. In order to do a gravimetric analysis, a cation must be found that forms an insoluble compound with chloride. Ions such as Ag+, Pb²+, and Hg₂²+ form insoluble chlorides. Therefore, silver chloride (AgCl) could be used to determine % Chloride (CI), because it is insoluble and it can be formed pure and is easily filtered. Ag+ (aq) + Cl(aq) →→ AgCl(s) One of the most useful applications of gravimetric analysis is the determination of chloride in natural waters such as seawater and water in rivers and lakes. In this experiment the chlorine content of an unknown soluble chloride salt is to be determined. The unknown is dissolved in distilled water and dilute silver nitrate solution is added to precipitate out the chloride as AgCl. NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s) Note that all of the aqueous species in the above reaction exists as ions in solution: NaCl(aq) exists as Na+ and Cl AgNO3 exists as Ag* and NO3 NaNO3(aq) exists as Na+ and NO3 AgCl(s) is a white solid Procedure Link: https://www.youtube.com/watch?v=dERZhN-01f8
Transcribed Image Text:Activity No. 8 Determination of Chloride Ion Concentration by Gravimetry Gravimetric analysis is a method in quantitative analysis where an unknown sample is dissolved in an appropriate solvent, and the analyte is converted to an insoluble form or precipitation of a known compound and then weighing the precipitate. In order to do a gravimetric analysis, a cation must be found that forms an insoluble compound with chloride. Ions such as Ag+, Pb²+, and Hg₂²+ form insoluble chlorides. Therefore, silver chloride (AgCl) could be used to determine % Chloride (CI), because it is insoluble and it can be formed pure and is easily filtered. Ag+ (aq) + Cl(aq) →→ AgCl(s) One of the most useful applications of gravimetric analysis is the determination of chloride in natural waters such as seawater and water in rivers and lakes. In this experiment the chlorine content of an unknown soluble chloride salt is to be determined. The unknown is dissolved in distilled water and dilute silver nitrate solution is added to precipitate out the chloride as AgCl. NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(s) Note that all of the aqueous species in the above reaction exists as ions in solution: NaCl(aq) exists as Na+ and Cl AgNO3 exists as Ag* and NO3 NaNO3(aq) exists as Na+ and NO3 AgCl(s) is a white solid Procedure Link: https://www.youtube.com/watch?v=dERZhN-01f8
Data Unknown Number: 345 Trial 2 Trial 3 Mass unknown, g 0.1015 0.1205 Mass crucible, g 20.1955 19.1986 Mass crucible + precipitate, g 20.5246 19.4873 Mass precipitate, g 0.3291 0.2887 Mass chloride, g % Chloride in unknown Average % Chloride: Standard deviation: Show Calculations for Trial 1: a. Mass of Chloride, g b. % Chloride Questions: 1. When the unknown sample was dissolved in 100 mL water, 6 M nitric acid (HNO3) was used to acidify the solution. Why shouldn't any acid such as HCI and H₂SO4 be used in this process? 2. For Trial 1, how many grams of AgNO3 must be added to the solution to completely react with NaCI? Trial 1 0.1345 21.3521 21.7076 0.3555
Transcribed Image Text:Data Unknown Number: 345 Trial 2 Trial 3 Mass unknown, g 0.1015 0.1205 Mass crucible, g 20.1955 19.1986 Mass crucible + precipitate, g 20.5246 19.4873 Mass precipitate, g 0.3291 0.2887 Mass chloride, g % Chloride in unknown Average % Chloride: Standard deviation: Show Calculations for Trial 1: a. Mass of Chloride, g b. % Chloride Questions: 1. When the unknown sample was dissolved in 100 mL water, 6 M nitric acid (HNO3) was used to acidify the solution. Why shouldn't any acid such as HCI and H₂SO4 be used in this process? 2. For Trial 1, how many grams of AgNO3 must be added to the solution to completely react with NaCI? Trial 1 0.1345 21.3521 21.7076 0.3555
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