The iodide ion concentration in a solution may be determined by the precipitation of lead iodide. Pb2+ (aq) + 21 (aq) →→→→PbI₂(s) A student finds that 22.10 mL of 0.5530 M lead nitrate is needed to precipitate all of the iodide ion in a 25.00-mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? M

The iodide ion concentration in a solution may be determined by the precipitation of lead iodide. Pb2+ (aq) + 21 (aq) →→→→PbI₂(s) A student finds that 22.10 mL of 0.5530 M lead nitrate is needed to precipitate all of the iodide ion in a 25.00-mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? M

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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[References] Use the References to access important values if needed for this question. The iodide ion concentration in a solution may be determined by the precipitation of lead iodide. Pb2+(aq) + 21(aq) PbI2(s) A student finds that 16.64 mL of 0.5820 M lead nitrate is needed to precipitate all of the iodide ion in a 25.00-mL sample of an unknown. What is the molarity of the iodide ion in the student's unknown? Submit Answer Try Another Version 1 item attempt remaining ot ot pt pt pt Previous Next ail 6,290 10 15 MAY étv W X 280
A solution contains Cr3+ and Mg2+. The addition of 1.00 L of 1.51 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 50.1 g . Find the mass of Cr3+ in the original solution.
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