Hello, I need you to answer HW. I will attach class note and powerpoint along with HW. You must follow the powerpoint and class note to understand then solve, and do not plagiarize from internet.

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Chapter 16: Redox Titrations Adapted from: Harris, D. C. Quantitative Chemical Analysis; W. H. Freeman and Company: New York, 2020; Ch. 16 1) 25.0 mL of 0.0500 M Sn2+ is titrated with 0.100 M Fe3+ in 1M HCl to yield Fe2+ and Sn4+ using a Pt indicator electrode and a standard calomel reference electrode. a. Write a balanced titration reaction b. Calculate equivalence volume (Ve) c. Write two different half-reactions for the indicator electrode d. Write two different Nernst Equations for the cell voltage Notice that the cell voltage (E ) depends on the ratio of [Fe2+]/[Fe3+] or [Sn2+]/[Sn4+] e. Calculate E after 15.0 mL of 0.100M Fe3+ has been added • Is this before, at, or after Ve? • What is in excess, analyte, titrant, or neither? • Which ratio will be easier to solve for, [Fe2+]/[Fe3+] or [Sn2+]/[Sn4+]? • Hint: you can use

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