2. An iron ore was analyzed by dissolving a 1.1324-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe2O3 XH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe2O3 (159.69 g/mol). Calculate the %Fe;O4 (231.54 g/mol) and its G.F in the sample. [Hints: 6 Fe,O, → 4 Fe,0, + 0,1

2. An iron ore was analyzed by dissolving a 1.1324-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe2O3 XH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe2O3 (159.69 g/mol). Calculate the %Fe;O4 (231.54 g/mol) and its G.F in the sample. [Hints: 6 Fe,O, → 4 Fe,0, + 0,1

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: A 0.1285-g sample of impure Na2CO3 was dissolved in 20.00 mL of 0.2034 M HCl. The excess HCl was…

A: We will first find out the actual mass of Na2CO3 present in the sample by calculating the moles of…

Q: Twenty tablets of an iron food supplement whose total mass was 22.131 g were crushed and perfectly…

A: Answer: This question is based on the relation between mass, molar mass and number of moles and by…

Q: The KCIO3 in a 0.1862-g sample of an explosive was determined by reaction with 50.00 mL of 0.01162 M…

Q: A 0.2417g sample of a compound composed of C,H,O,CI only, is burned in oxygen yielding 0.4964g of…

A: Mass of the sample 1 = 0.2417 gAtoms present in compound = C, H, O, ClMass of CO2 obtained = 0.4964…

Q: Standard Sodium Chloride Weighed mass of NaCl Purity of NaCl Molar concentration of NaCl using…

A: Molar concentration of NaCl :M = (m × p)/ ( V × Mw ) where M is molarity, m is mass, p is purity,…

Q: The amount of sulfate in a solid sample was determined by first dissolving 562.2 mg of sample in…

Q: A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 99.50 mL of 1.500 M NaCl, and the PbCl₂…

A: The balanced chemical equation for the precipitation of lead (II) chloride can be written as:…

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: A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with…

Q: The purity of a pharmaceutical preparation of sulfanildamide (C6H4N2O2S), is prolonged oxidizing the…

A: Mass of sample = 0.5136 g Molarity of NaOH = 0.1251 M Volume of NaOH required = 50.00 mL = 0.050 L

Q: 31. 10.0 mL. of concentrated of H3PO4(aq) is diluted to the final volume of 250.0 mL. Then 15.0…

A: Given that : The initial volume of H3PO4 = 10.0 mL The final volume of H3PO4 = 250.0 mL Molarity of…

Q: on, and then titrated with pre. n't need to know the formula

A: Calculation of mass percentage of iron. Mass of iron = 55.845g/mol.

Q: Write the balanced equation for the reaction of aqueous Pb(ClO3)2 Pb ( ClO 3 ) 2 with aqueous NaI.…

A: Information of question

Q: In one gravimetric analysis, the iron (Fe) in a 1.6374 g of impure iron compound was dissolved with…

Q: The concentration of KClO3 in the explosive sample can be determined by reaction with Fe(II): ClO3-…

A: The chemical reaction between KClO3 and Fe2+ is represented as follows:…

Q: When 15.11 ml of 0.102 M K2SO4 solution reacts with 35.00 ml of 0.114 M Pb(C2H3O2)2. predict the…

A: Data given: Volume of K2SO4 solution = 15.11 mL = 0.01511 L (1 L = 1000 mL) Concentration of K2SO4…

Q: The Fe2+ (55.845 g/mol) content of a 2.433 g steel sample dissolved in 50.00 mL of an acidic…

Q: A sample of copper oxide weighing 2.013 g is dissolved in acid, the pH adjusted, and excess KI…

Q: A 6.586-g sample containing magnesium chloride and sodium chloride was dissolved in sufficient water…

A: Mass of sample = 6.586 g Mass of sample solution = 500 mL Mass of AgCl formed from 50 mL solution =…

Q: Iron was analyzed by dissolving 1.1324 g sample in concentrated HCL, The solution was diluted in…

A: A multiple choice question based on mole concept, which is to be accomplished.

Q: The arsenic in a 1.208-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The…

Q: The hydrogen sulfide in a 40.0-g sample of crude petroleum was removed by distillation and collected…

A: Mass of CdSO4 = 0.079 g Mass of sample = 40.0 g

Q: 0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

100%

2. 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
Fe2O3 XH2O by addition of NH3. After filtration and washing, the residue was ignited at a high
temperature to give 0.5394 g of pure Fe2O3 (159.69 g/mol). Calculate the %Fe;O4 (231.54 g/mol)
and its G.F in the sample.
[Hints: 6 Fe,0,
→ 4
4 Fe,0, +
+0,]
3

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

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 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
A sample consisting of Na2CO3 (105.96), NaOH (39.99) and inert matter weighs 1.179 g. It is titrated with 0.300 N HCI with phenolphthalein as the indicator, and the solution becomes colorless after the addition of 48.16 ml. Methyl orange is then added and 24.08 ml more of the acid are needed for the color change. What is the percentage of NaOH and N22CO3? *
0.9545 g of calcium nitrate salt, Ca (NO3) 2, is weighed, dissolved in concentrated HCl solution and added to 500 ml with water. It is diluted, 100 ml sample taken here is precipitated as CaC2O4, burned in the ash furnace and It is converted to CaCO3 and then to CaO. Since it comes to 0.2500 g when weighed, the amount of Ca in the sample and calculate its% (Ca: 40 g / mol, O: 16 g / mol)
A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is added to turn the solution yellow. Zimmermann–Reinhardt reagent is added, and the solution is diluted to 150mL. It is then titrated with 31.30 mL of 0.045 M potassium permanganate. a) How many moles of MnO4- were used to titrate the iron in the sample? b) How many moles of Fe2+ were in the sample? c) What is the mass of iron in the sample? d) What is the % w/w of Fe in the sample?
The zinc content of a 1.55 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HCl is then neutralized with with NaOH. The reaction of HClHCl with Zn is shown. Zn(s)+2HCl(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 8.92 mL of 0.548 NaOH to neutralize the excess HCl. What is the mass percentage (%w/w) of Zn in the ore sample?
A solid sample of Zn1OH22 is added to 0.350 L of 0.500 Maqueous HBr. The solution that remains is still acidic. It isthen titrated with 0.500 M NaOH solution, and it takes 88.5mL of the NaOH solution to reach the equivalence point.What mass of Zn1OH22 was added to the HBr solution?