# Chemistry

An iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe2+(aq). The iron solution was titrated with 38.54 mL of 0.471 M Ce4+ solution according to the balanced chemical equation below.

Ce4+(aq) + Fe2+(aq) -> Ce3+(aq) + Fe3+(aq).

Calculate the mass of iron in the original ore sample. Please round your answer to the nearest hundredths place.

mol of Ce4+ = 38.54 mL x 0.471 M = 18.15 mmol
mol of Fe = mol of Fe2+ = mol of Ce4+ = 18.15 mmol
mass of iron = 18.15 x 55.84 = 1013.50 mg = 1.01g

Did I do this problem correctly. And did I round to the hundredths place appropriately?

1. 👍 0
2. 👎 0
3. 👁 850
1. it is correct.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chimestry

(Iron ore is impure Fe_2O_3. When Fe_2O_3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing 950kg , 533kg of pure iron is obtained). What is the mass

asked by Inni on September 11, 2012
2. ### chemistry

a piece of metallic iron (10 moles) was dissolved in concentrated hydrochloric acid. the reaction formed iron (II) chloride and hydrogen gas. how many moles of iron (II) chloride were formed?

asked by dee on March 26, 2014
3. ### Chemistry

Iron ores have different amounts of iron per kilogram of ore. Calculate the mass percent composition of iron for each iron ore: Fe2O3{\rm Fe_2O_3} (hematite), Fe3O4{\rm Fe_3O_4} (magnetite), FeCO3{\rm FeCO_3} (siderite).

asked by Ana on March 5, 2014
4. ### chemistry

A 3.75-G SAMPLE OF IRON ORE IS TRANSFORMED TO A SOLUTION OF IRON(II)SULFATE, FeSO4,AND THIS SOLUTION IS TITRATED WITH 0.150 M K2Cr2O7. IF IT REQUIRES 43.7 mL OF POTASSIUM DICHROMATE SOLUTION TO TITRATE THE IRON(II)SULFATE

asked by malissa on October 23, 2012

A galvanic cell is based on the following half-reactions: Fe2+ + 2e- --> Fe(s) E= –0.440 V 2H+ + 2e- --> H2(g) E= 0.000 V where the iron compartment contains an iron electrode and [Fe2+] = 1.00 x 10-3 M and the hydrogen

asked by Kaili on March 9, 2012
1. ### Chemistry

A 0.1300 g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe2+(aq). The iron solution was titrated with Ce4+ solution according to the balanced chemical reaction shown below. After calculation, it

asked by Bob on March 13, 2009
2. ### Chemistry

A 0.5962g sample of iron ore is dissolved in acid producing Fe3+. Through a series of reactions, the iron precipitates as the Fe(OH)3. The precipitate is heated, forming solid Fe2O3. What is the mass % of iron in the sample if the

asked by Chris on December 6, 2010
3. ### Chemistry

A piece of metallic iron (10 moles) was dissolved in concentrated hydrochloric acid. The reaction formed hydrogen gas and iron chloride. How many grams of HCl were consumed? Don't forget the units. Fe+2HCl---->FeCl2+H2