The concentration of Fe2+ in a solution is determined by titrating it with a 0.1683 M dichromate solution. The balanced net ionic equation for the reaction is:Cr2O72-(aq) + 6Fe2+(aq) + 14H3O+(aq) = 2Cr3+(aq) + 6Fe3+(aq) + 21H2O(l) In one experiment, 23.05 mL of the 0.1683 M dichromate solution is required to react completely with 20.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2+ solution.
The concentration of Fe2+ in a solution is determined by titrating it with a 0.1683 M dichromate solution. The balanced net ionic equation for the reaction is:Cr2O72-(aq) + 6Fe2+(aq) + 14H3O+(aq) = 2Cr3+(aq) + 6Fe3+(aq) + 21H2O(l) In one experiment, 23.05 mL of the 0.1683 M dichromate solution is required to react completely with 20.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2+ solution.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter4: Chemical Reactions In Solution
Section: Chapter Questions
Problem 4.21QE
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The concentration of Fe2+ in a solution is determined by titrating it with a 0.1683 M dichromate solution. The balanced net ionic equation for the reaction is:Cr2O72-(aq)
- +
6Fe2+(aq) + 14H3O+(aq) =
2Cr3+(aq)
- +
6Fe3+(aq) + 21H2O(l)
In one experiment, 23.05 mL of the 0.1683 M dichromate solution is required to react completely with 20.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2+ solution.
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