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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?

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eorTA EXPERIMENT 7 I bos) OXIDATION-REDUCTION TITRATIONS onidoed-reducing ogont reduced-> oxidized geent gan Name Aygakah Lesis HOMEWORK EXERCISES Use 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 equation for the titration of Mohr's salt with KMNO4. lonic MnO4 : Mn Ou iag) + sc +8H'cag) スt Ionic Fe2*: Fe * (a9) 3+ 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? 2. a. Write the balanced equations for the half reactions and the overall net ionic equation for the titration of H2O2 with KMnO4. Ionic MnO4 : alp Ionic 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 KMn04 solution 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 eby ount of 93
Transcribed Image Text:eorTA EXPERIMENT 7 I bos) OXIDATION-REDUCTION TITRATIONS onidoed-reducing ogont reduced-> oxidized geent gan Name Aygakah Lesis HOMEWORK EXERCISES Use 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 equation for the titration of Mohr's salt with KMNO4. lonic MnO4 : Mn Ou iag) + sc +8H'cag) スt Ionic Fe2*: Fe * (a9) 3+ 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? 2. a. Write the balanced equations for the half reactions and the overall net ionic equation for the titration of H2O2 with KMnO4. Ionic MnO4 : alp Ionic 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 KMn04 solution 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 eby ount of 93
EXPERIMENT 7 OXIDATION-REDUCTION TITRATIONS 4. 25.5978 g of a 15.5% H2O2 solution was titrated with 0.2542 M Ca(MnO4)2, an oxidiZing agent. How many mL of the Ca(MnO4)2 solution would be required for titration? Carefully consider 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 mL of 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 12.50 grams of 30.0 % H2O2 solution? 6. In a redox titration, 12.52 mL of a 0.3264 M KMNO4 solution were required to titrate 1.7832 g of a reducing agent (“X"). If the reducing agent undergoes a 3-electron change per 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
Transcribed Image Text:EXPERIMENT 7 OXIDATION-REDUCTION TITRATIONS 4. 25.5978 g of a 15.5% H2O2 solution was titrated with 0.2542 M Ca(MnO4)2, an oxidiZing agent. How many mL of the Ca(MnO4)2 solution would be required for titration? Carefully consider 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 mL of 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 12.50 grams of 30.0 % H2O2 solution? 6. In a redox titration, 12.52 mL of a 0.3264 M KMNO4 solution were required to titrate 1.7832 g of a reducing agent (“X"). If the reducing agent undergoes a 3-electron change per 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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