12:06 A *A * ll 68%iZoom vLeave• RECBreakoutRoomsGROUP WORKAn iron ore was analyzed by dissolving a 1.1324 gsample in concentrated HCI.The resulting solution was diluted with water and theiron (III) was precipitated as the hydrous oxideFe,O3.xH,O by the addition of NH3. After filtration andwashing, the residue was ignited at a high temperatureto give 0.5394 g of pure Fe,03 (159.69g/mol).Calculate (a) % Fe (55.847g/mol) and (b) %Fe,04(231.54g/mol) in the sample.•. 28UnmuteStart VideoShareParticipantsMoreII

Answered: Image /qna-images/answer/17f8a7d6-01ab-4658-a942-5dd31a481219.jpg

GROUP WORK An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HCI. The resulting solution was diluted with water and the iron (III) was precipitated as the hydrous oxide Fe,03.xH,O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe,O3 (159.69g/mol). Calculate (a) % Fe (55.847g/mol) and (b) % Fe,04(231.54g/mol) in the sample.

GROUP WORK An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HCI. The resulting solution was diluted with water and the iron (III) was precipitated as the hydrous oxide Fe,03.xH,O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe,O3 (159.69g/mol). Calculate (a) % Fe (55.847g/mol) and (b) % Fe,04(231.54g/mol) 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...

See similar textbooks

Related questions

Q: In a titration of HNO₃, you add a few drops of phenol-phthalein indicator to 50.00 mL of acid in a…

A: The total volume of acid we have taken to finally reach the endpoint = 50 + 30 = 80 mL And the total…

Q: MGNH&PO4-6H2O has a solubility in water of 0.023 g/100mL. Suppose a student obtains 0.7193 g of…

A: Solution:- Given the solubility of MgNH4PO4.6H2O is 0.023 g/100 mL Mass of precipitate = 0.7193 g…

Q: Write the balanced equation for the reaction of aqueous Pb(CIO,), with aqueous Nal. Include phases.…

A: Given,Molarity of NaI = 0.210 Mvolume of NaI = 0.600 Lvolume of Pb(ClO3)2 = 1.50 L

Q: Barium (Ba) can be analyzed in solutions by forming BaSO4 (s) precipitate. Ba (2+) + SO4(2-) -->…

A: The amount of Ba2+ ions in the sample of barium compound is unknown and is to be calculated to…

Q: Mixtures of CaCl₂ and NaCl are used to melt ice on roads.A dissolved 1.9348-g sample of such a…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: In the laboratory you are given the task of separating Ca and Fe" ions in aqueous solution. For each…

A: We are authorized to answer one question at a time, since you have not mentioned which question you…

Q: A stock solution containing Mn2+ ions was prepared by dissolving 1.460 g pure manganese metal in…

A: The molarity is one of the measure of concentration of the solution. This is defined as the no of…

Q: In the laboratory you are given the task of separating Ag* and Ba²+ ions in aqueous solution. For…

A: According to solubility rules, All sulfates are soluble except Ca+2, Ba+2, Ag+, Pb+2, Sr+2, Hg+2.…

Q: A powder contains FeSO 7 H₂O (molar mass = 278.01 g/mol), among other components. A 3.630 g sample…

A: The objective of this question is to determine the mass of FeSO4.7H2O in a 3.630 g sample of a…

Q: 2. The arsenic in a 1.203-g sample of a pesticide was converted to H3ASO4 by suitable treatment. The…

A: Given that,Weight of pesticide = 1.203gVolume of = 40 mLMolarity of = 0.05871 MVolume of = 9.63…

Q: e "No" Y or N Reagent Formula of Precipitate if YI 1. K2CO3 2. Nal 3. NazSO4

A: We have to separate the ions of Pb+2 and Fe+2 ions in aqueous solution with the help of potassium…

Q: Tungsten trioxide (WO,) has a rich yellow color and is often used as a pigment in ceramics and…

Q: The zinc content of a 1.42 g ore sample was determined by dissolving the ore in HCI, which reacts…

A: Given, mass of ore sample = 1.42 g. The ore was dissolved in 150 mL of 0.600 M HCl, and the…

Q: A 0.7785 g sample containing hydrazine (N2H4, rocket fuel) was dissolved and diluted to 250.0 mL in…

A: Answer: This question is based on stoichiometric calculation where we have to convert the moles of…

Q: A 0.51960.5196 g solid sample containing a mixture of LaCl3LaCl3 (molar mass = 245.26 g/mol) and…

A: The reactions of LaCl3 & Ce(NO3)3 with KIO3 are represented as follows: LaCl3 +3 KIO3 →…

Q: Suppose a student needs to standardize a sodium thiosulfate, Na, S,0,, solution for a titration…

Q: The zinc content of a 1.50 g ore sample was determined by dissolving the ore in HCI, which reacts…

Q: In the laboratory you are given the task of separating Ca2+ and Co2+ ions in aqueous solution. For…

A: Since you have asked multiple question, as per our company guidelines we are supposed to answer…

Q: A student is given 1.5621 g of pure CuO. To recover the Cu present in the compound, the dark powdery…

A: The balanced reaction taking place is given as, => Mg (s) + Cu2+ (aq) ------> Cu (s) + Mg2+…

Q: 100.0 mL of 0.60 M aqueous Pb(NO3)2 is mixed with excess aqueous KI. What mass of precipitate is…

Question

12:06 A *
A * ll 68%i
Zoom v
Leave
• REC
Breakout
Rooms
GROUP WORK
An iron ore was analyzed by dissolving a 1.1324 g
sample in concentrated HCI.
The resulting solution was diluted with water and the
iron (III) was precipitated as the hydrous oxide
Fe,O3.xH,O by the addition of NH3. After filtration and
washing, the residue was ignited at a high temperature
to give 0.5394 g of pure Fe,03 (159.69g/mol).
Calculate (a) % Fe (55.847g/mol) and (b) %
Fe,04(231.54g/mol) in the sample.
•. 28
Unmute
Start Video
Share
Participants
More
II

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A compound containing barium (Ba) and oxygen, weighed 2.018 g, was dissolved to produce barium ions in solution. The barium ions are then separated from the solution by precipitating method. The precipitate formed was 3.018 g of BaCrO4. Determine the chemical formula of the compound.
A powder contains FeSO4⋅7H2OFeSO4⋅7H2O (molar mass=278.01 g/mol),(molar mass=278.01 g/mol), among other components. A 3.125 g3.125 g sample of the powder was dissolved in HNO3HNO3 and heated to convert all iron to Fe3+.Fe3+. The addition of NH3NH3 precipitated Fe2O3⋅?H2O, Fe2O3⋅xH2O, which was subsequently ignited to produce 0.469 g Fe2O3.0.469 g Fe2O3. What was the mass of FeSO4⋅7H2OFeSO4⋅7H2O in the 3.125 g3.125 g sample? mass of FeSO4⋅7H2OFeSO4⋅7H2O:
When aqueous FeCL3 is combined with 100.00 mL of a base solution containing Ba(OH)2, 0.567g of rust-red solid is precipitated. Assuming that barium hydroxide was completely consumed through this reaction, what was the molar concentration of the original Ba(OH)2 solution.
Please help me solve this. I need to see the steps taken with explanations so that I can keep this as study notes. A 1.345 gram sample of a compound containing barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ions (Ba+2), which was then completely precipitated out with excess potassium chromate to give 2.012 grams of barium chromate, BaCrO4. (a) How many moles of barium ions(Ba+2) were in the original sample? (b) How many grams of barium ions (Ba+2) were in the original sample? (c) How many grams of oxygen ions(O-2) were in the original sample? (d) What is the percentage by mass of O ions (O-2) in the original(1.345g) sample? .
A 4.908-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 2% H2 O2. Reaction: SO2 (g) + H2O2 → H2SO4 A 27.00-mL portion of 0.00826 M NaOH was introduced into the solution of H2 SO4, following which the excess base was back-titrated with 15.15 mL of 0.01165 M HCl. Calculate the sulfur concentration in the sample in parts per million. Concentration ppm
In the laboratory you are given the task of separating Ca2+ and Fe2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the lons, give the formula of the precipitate. If it cannot, type "No" Y or N 1. 12. 3 Reagent Formula of Precipitate if YES ка K₂SO4 Na CO
A 57.0 mLmL sample of a 0.108 MM potassium sulfate solution is mixed with 37.0 mLmL of a 0.106 MM lead(II)(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s). Find the theoretical yield and percent yield.
Analytical chemistry
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 17.07 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.
The zinc content of a 1.07 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HC1 is then neutralized with with NaOH. The reaction of HC1 with Zn is shown. Zn(s) + 2 HCl(aq) → ZnCl₂ (aq) + H₂(g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 9.96 mL of 0.540 M NaOH to neutralize the excess HC1. What is the mass percentage (%w/w) of Zn in the ore sample? %W/W = % Zn
In the laboratory you are given the task of separating Pb²+ and Cu²+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. HBr 2. 3. Na₂SO4 K₂CO3