An analytical chemist has a solution containing chloride ion, Cl¯. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AGNO3. As a way to indicate the endpoint of the titration, she added 1.13 g of potassium chromate, K2CrO4. As she slowly added the silver nitrate to the solution, a white precipitate formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution at this point was 60.8 mL. How many moles of chloride ion were there in the original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable approximations. Ksp for Ag, CrO4 is 1.1 x 10-12, K, for AgCl is 1.8 x 10-10 moles of Cl¯ in the original solution moles of Cl¯ in the final solution

Chemistry & Chemical Reactivity
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Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section: Chapter Questions
Problem 28PS: Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 ...
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An analytical chemist has a solution containing chloride ion, Cl¯. She decides to determine the amount of chloride ion in
the solution by titrating 50.0 mL of this solution by 0.100 M AGNO3. As a way to indicate the endpoint of the titration, she
added 1.13 g of potassium chromate, K2CrO4. As she slowly added the silver nitrate to the solution, a white precipitate
formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another
precipitate. The volume of the solution at this point was 60.8 mL. How many moles of chloride ion were there in the
original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable
approximations. Ksp for Ag, CrO4 is 1.1 x 10-12, K, for AgCl is 1.8 x 10-10
moles of Cl¯ in the original solution
moles of Cl¯ in the final solution
Transcribed Image Text:An analytical chemist has a solution containing chloride ion, Cl¯. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AGNO3. As a way to indicate the endpoint of the titration, she added 1.13 g of potassium chromate, K2CrO4. As she slowly added the silver nitrate to the solution, a white precipitate formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution at this point was 60.8 mL. How many moles of chloride ion were there in the original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable approximations. Ksp for Ag, CrO4 is 1.1 x 10-12, K, for AgCl is 1.8 x 10-10 moles of Cl¯ in the original solution moles of Cl¯ in the final solution
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