A solid sample containing some Fe2* ion had a total mass of 0.891 g. It required 18.3 mL 0.029M KMNO4 to titrate the Fe2+ in the dissolved sample to a pink end point. a. How many moles of MnO4 ion were required? moles b. How many moles of Fe2* were present in the sample? moles c. How many grams of iron were present in the sample? (The atomic mass of iron is 55.845 g/mol.) g d. What was the mass percent of iron in the sample? %

A solid sample containing some Fe2* ion had a total mass of 0.891 g. It required 18.3 mL 0.029M KMNO4 to titrate the Fe2+ in the dissolved sample to a pink end point. a. How many moles of MnO4 ion were required? moles b. How many moles of Fe2* were present in the sample? moles c. How many grams of iron were present in the sample? (The atomic mass of iron is 55.845 g/mol.) g d. What was the mass percent of iron in the sample? %

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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Tungsten trioxide (WO,) has a rich yellow color and is often used as a pigment in ceramics and paints. To test a ceramic vase for its WO, content, a 10.15 g sample of the vase was ground and reduced with Pb(Hg) to convert any WO, to W³+. The resulting W3+ was transferred to 500.0 mL of 1.00 M HCI. A 100.00 mL aliquot of the HCl solution required 14.78 mL of 0.08271 M potassium permanganate (KMNO,) to reach the purple endpoint. A blank required 0.26 mL. Balance the redox reaction. redox reaction: MnO, + W3+ Mn2+ + WO3+ Determine the percent WO, in the ceramic sample. percent WO3: %
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Emma titrated 20.00 mL of an HCL(aq) solution that has an unknown concentration with 0.1240 M NaOH(aq). The equivalence point is reached after adding 25.46 mL of NaOH(aq). a. Write out the complete balanced equation for the reaction that occurs in this titration. b. How many moles of NaOH were added to the HCl solution? c. How many moles of HCl were in the original 20.00 mL solution? d. What was the concentration of HCl in the original 20.0 mL solution?
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