The solubility of Ag2CrO4 (Ksp = 1.2 x 10^-12) is several times greater than that of AgCl (Ksp = 1.82 x 10^-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 as an indicator for 100 mL of sample solution, what is the concentration (M) of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?
The solubility of Ag2CrO4 (Ksp = 1.2 x 10^-12) is several times greater than that of AgCl (Ksp = 1.82 x 10^-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 as an indicator for 100 mL of sample solution, what is the concentration (M) of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The solubility of Ag2CrO4 (Ksp = 1.2 x 10^-12) is several times greater than that of AgCl (Ksp = 1.82 x 10^-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 as an indicator for 100 mL of sample solution, what is the concentration (M) of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?
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Step 1: For step 1, the solubility product of given species is written and moles are calculated using amount
VIEWStep 2: For step 2, further calculation is done for the determining concentration of chloride ion
VIEWStep 3: For step 3,the final step of calculation is done and the concentration of chloride ion is calculated
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