HomeworkLib
Question

A 2.67 g sample of an iron alloy (a mixture of iron with other metallic elements)...

A 2.67 g sample of an iron alloy (a mixture of iron with other metallic elements) was dissolved in hydrochloric acid to give a solution of Fe2+ ion. This solution was titrated to the end point with 39.9 mL of 0.174 M MnO4- yielding Fe3+ and Mn2+ as products. What is the percentage (to 1 decimal place) of iron in the sample?

(At. mass of Mn = 54.94, O = 16.00, Fe = 55.85)

Half Reactions:

MnO4- + 8H+ + 5e- → Mn2+ + 4H2O(l)

Fe3+ + e- → Fe2+

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
A 2.67 g sample of an iron alloy (a mixture of iron with other metallic elements)...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • A 1.026 g sample of an iron unknown requires 24.35 mL of 0.0195 M MOA solution...

    A 1.026 g sample of an iron unknown requires 24.35 mL of 0.0195 M MOA solution to reach the end point. The atomic mass of Fe is 55.85 g/mol. Balanced equation: 5Fe2+ (aq) + MnO4 (aq) + 8H(aq) 5Fe(aq) + Mn(aq) + 4H2O) Which species aids in the dissolution of the compounds and helps to facilitate the reaction? Spectator ions are omitted. c) H b) Fe3+ d) Mn2+ a) MnO4 What is the mass percent of iron in the unknown?...

  • A 0.1362g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as...

    A 0.1362g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe^2+(aq). The iron solution was titrated with Ce4+ solution according to the balanced chemical reaction shown below. After calculation, it was found that 0.0238g of iron from the ore reacted with the cerium solution. Ce^4+(aq) + Fe 2+(aq) -> Ce^3+(aq) + Fe^3+(aq). Calculate the mass percent of iron in the original ore sample. Please round your answer to the tenths place. Question 7 (2...

  • suppose you have an unknown sample containing Fe^2+, and you titrate it with KMnO4 standard solution....

    suppose you have an unknown sample containing Fe^2+, and you titrate it with KMnO4 standard solution. Calculate the percent of Fe in your sample. equation: MnO4- + 5Fe^2+ + 8H^+ --> Mn^2+ + 5Fe^3+ + 4H2O Suppose you have an unknown sample containing Feat, and you titrate it with a KMnO4 standard solution. Calculate the percentage of Fe in your sample. Equation: MnO(+5Fe2+ + 8H - Mn2+ + 5Fe3+ + 4H20 Data 0.08124M 2.49g Molarity of the KMnO4 standard solution:...

  • An acidified solution of manganate (VII) of permanganate ions, MnO4-, is a strong oxidising agent and...

    An acidified solution of manganate (VII) of permanganate ions, MnO4-, is a strong oxidising agent and will be used in an experiment to determine the percentage of iron in a sample of ammonium iron (II) sulfate hexahydrate. The titration is self-indicating because at the equivalence point the products are a different colour than the original reactants. The two half reactions are: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l) Fe^2+(aq) ---> Fe^3+(aq) + e- a) What is a redox...

  • Question 10 (2 points) A 13.9800-g sample of a salt was analyzed for its iron content...

    Question 10 (2 points) A 13.9800-g sample of a salt was analyzed for its iron content as follows: the entire sample was dissolved and diluted to 400.0 mL in a volumetric flask. A 80.00-ml aliquot of the solution required 25.38-mL of a 0.04119 M potassium permanganate solution to reach equivalence. A blank correction of 0.50 mL was required. Calculate the %(w/w) Fe in the sample. The net-ionic equation for the reaction is MnO4 (aq) + 8H+ (aq) + 5Fe2+(aq) -...

  • A 0.450−g sample of steel contains manganese as an impurity. The sample is dissolved in acidic...

    A 0.450−g sample of steel contains manganese as an impurity. The sample is dissolved in acidic solution and the manganese is oxidized to the permanganate ion MnO4−. The MnO4− ion is reduced to Mn2+ by reacting with 50 mL of 0.0800 M FeSO4 solution. The excess Fe2+ ions are then oxidized to Fe3+ by 20.5 mL of 0.0100 M K2Cr2O7. Calculate the percent by mass of manganese in the sample. ___% Mn

  • 1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M...

    1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO, to titrate the Fe- in the dissolved sample to a pink end point. The balanced redox reaction is shown below. 8 H + MnO4 + 5 Fe2+ + Mn2+ + 5 Fe3+ + 4H20 Calculate each of the following quantities. 2. (2 points) Calculate the percentage of Fe in pure iron(II) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]• 6 H20.

  • 1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5...

    1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...

  • Chromel is an alloy composed of nickel, iron, and chromium. A 0.6445-g sample was dissolved and...

    Chromel is an alloy composed of nickel, iron, and chromium. A 0.6445-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.23-mL back-titration with 0.06139 M copper(II) was required. The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 38.95 mL of 0.05173 M EDTA....

  • The Fe2+ (55.845 g/mol) content of a 2.370 g steel sample dissolved in 50.00 mL was...

    The Fe2+ (55.845 g/mol) content of a 2.370 g steel sample dissolved in 50.00 mL was determined by tiration with a standardized 0.120 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 39.51 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per grams of steel (g Fe2+1 g steel). Mno, +8H+ + 5Fe2+ = Mn2+ + 5Fe'+ + 4H,0 Number g Fe2+1 g steel

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT