I need help with the front and back of this page. I do not understand anything. eorTA EXPERIMENT 7I bos)OXIDATION-REDUCTION TITRATIONSonidoed-reducing ogontreduced-> oxidized geent ganName Aygakah LesisHOMEWORK EXERCISESUse the net ionic equations in problems 1 and 2 for problems 3-5.1gain) 1. a.write the balanced equations for the half reactions (ionic) and the overall net ionic equationfor the titration of Mohr's salt with KMNO4.lonic MnO4 : Mn Ou iag) + sc +8H'cag)スtIonic Fe2*: Fe * (a9)3+Net ionic:b. What is the standardized molarity of a KMNO4 solution if 36.31 mL are required to titrate2.5010 g of Mohr's salt?2. a. Write the balanced equations for the half reactions and the overall net ionic equation forthe titration of H2O2 with KMnO4.Ionic MnO4 :alpIonic H2O2:Net ionic:b. How is the equivalence point detected in this titration?3. A 1.6152 g sample of a solution containing H2O2 required 11.78 mL of a 0.6134 M KMn04solution to reach the equivalence point.a. How many grams of H2O2 were present in the solution?b. What is the percent H2O2 present in the solution?heb ebyount of93 EXPERIMENT 7OXIDATION-REDUCTION TITRATIONS4. 25.5978 g of a 15.5% H2O2 solution was titrated with 0.2542 M Ca(MnO4)2, an oxidiZingagent. How many mL of the Ca(MnO4)2 solution would be required for titration? Carefullyconsider the MnO, to Ca(MnO4)2 mole ratio.5. 2.6477 g of the reducing agent FeSO4 was titrated to the equivalence point with 17.25 mLof a KMNO4 solution.a. Calculate the molarity of the KMNO4 solution.b. What volume (in mL) of the KMNO4 solution would be needed to react with 12.50grams of 30.0 % H2O2 solution?6. In a redox titration, 12.52 mL of a 0.3264 M KMNO4 solution were required to titrate1.7832 g of a reducing agent (“X"). If the reducing agent undergoes a 3-electron changeper formula unit:a. Write the two ionic half reactions and the balanced net ionic equation.Ionic MnO4:Ionic Reducing Agent:Net ionic:b. Calculate the molar mass of the reducing agent.94

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Use the net ionic equations in problems 1 añd 2 sain) 1. a. Write the balanced equations for the halfreactions (ionic) and the overall net ionic equation for the titration of Mohr's salt with KMNO4. Ionic MnO, : MnOuing) + 5c +8H'cags Ionic Fe2+: Fe スト 3+ (a9) Net ionic: b. What is the standardized molarity of a KMNO4 solution if 36.31 mL are required to titrate 2.5010 g of Mohr's salt?

Use the net ionic equations in problems 1 añd 2 sain) 1. a. Write the balanced equations for the halfreactions (ionic) and the overall net ionic equation for the titration of Mohr's salt with KMNO4. Ionic MnO, : MnOuing) + 5c +8H'cags Ionic Fe2+: Fe スト 3+ (a9) Net ionic: b. What is the standardized molarity of a KMNO4 solution if 36.31 mL are required to titrate 2.5010 g of Mohr's salt?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.22QAP

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