A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.

A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.199QP

See similar textbooks

Related questions

Q: the determination of iron in limonite, 0.5166 g of minerals dissolve in acid and Fe2+ is titrated…

A: First find the moles of K2Cr2O7 utilized. Then using reaction stoichiometry finally the moles of…

Q: Even though most metal sulfides are sparingly soluble in water, their solubilities differ by several…

A: Given data: Molarity of Cu2+ = 0.10 M Molarity of Ni2+ = 0.10 M

Q: 0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution.…

A: Answer is explained below.

Q: 20 g of Hematite ore needed to react with 10.5g from reducing substance in .. to obtain Iron.…

Q: The aluminum in 0.200 g impure aluminum sulfate ( the sample) was precipitated with aqueous NH3and…

A: Since the weight of aluminum obtained form impure aluminum sulfate is 0.15 g. Molar mass of aluminum…

Q: 10. Determination of the presence of Aluminum ion in 30.0g of ore sample is: a standardization…

A: A standardization process is that in which the concentration of a substance is determined.…

Q: (a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000g is treated with…

Q: The following is the brief summary of how Aliquot 1 was prepared in Expt. 8: Step 1: The unknown…

A: Given data,Mass of steel sample=0.5079 gTotal volume of stock solution=200mL=0.200LVolume of stock…

Q: To adjust the thiosulfate (S2O3) solution to be used as a titrant in the copper determination,…

Q: In the determination of iron in limonite, 0.5166 g of mineral is dissolved in acid and Fe2 + is…

A: Amount of limonite = 0.5166 g 42 96 ml of 0.0213 M Na2Cr2O4 is added in the titration. Molar mass of…

Q: In the reaction, Fe2+ + Cr2O72- Fe3+ + Cr3+, which is involved in oxidation? A. Fe B. Cr2O7 C. Cr…

Q: Voltammetry is limited to analysis of inorganic samples only True or false

A: Answer: False Voltammetry is an accurate electro-analysis method and combination with…

Q: A 110.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of…

A: Answer is 172.4 ppm

Q: In the determination of iron in limonite, 0.5166 g of mineral is dissolved in acid and Fe2 + is…

A: This question is related to finding out the percentage of Fe2+ in the given iron ore sample. First…

Q: Fill in the products to complete the reaction below showing how coke (a form of elemental carbon)…

A: Given Reaction C + CO2→

Q: 10.000 grams of Clay was analyze for Iron content. Its moisture content is 2.00%. The sample was…

A: Since you have posted multiple independent questions in the same request, we will solve the first…

Q: - A silicate ore contains 12.00% Na,0 and weighs 0.5000 gram. On analysis by the J.L. Smith method,…

Q: (a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000 g is treated with…

A: What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000 g is treated with a…

Q: sources of error of determination of iron in iron ore

A: Impurities in the iron from the Blast Furnace include carbon, sulphur, phosphorus and silicon. These…

Q: AAS is the most widely used instrumentation for the analysis of metal and traces metal samples.…

Q: The sulfur from 4.00g steel is evolved as dihydrogen sulfide gas and titrated with 1.60 mL of…

Q: The iron content of a large lump of ore is determined by taking a single small sample, dissolving it…

A: A random error is a discrepancy that occurs by chance between the observed and actual values of…

Q: Gold can be determined in solutions containing high concentrations of diverse ions by ICP-AES.…

Q: blast furnace makes pig iron containing 3.6% C, 1.4% Si and 95% Fe. The ore used contains 80% FE2O3,…

Q: Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation :…

A: The given compound first undergoes dissociation in its aqueous solution as,

Q: What is the oxidation state of the metal in the dioxide of Rh, Ir, Pd, and Pt? Express your answer…

A: The dioxides of following compound are: Rh- RhO2

Q: Copper is produced from chalcopyrite concentrate from a mixed type ore containing 1.2% CuFeS2…

A: Copper is obtained fron the mixed ore chalcopyrite and azurite.

Q: Calmagite is often used as a substitute for Eriochrome Black T as indicator in the determination of…

Q: To analyze the amount of iron (Fe; Mw = 55.85 g/mol) contained in an ore sample, the sample was…

A: Given in the question, Volume of EDTA = 25 ml Molarity of EDTA = 0.2922 M Total moles of EDTA =…

Q: What types of metals are usually purified by the method of zone refining? Give an example.

A: Metals are lustrous elements. They are good conductors of heat and electricity. They are malleable (…

Q: 2. 100.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of…

A: In the given question we have to calculate the concentration of iron in 100 mL sample of spring…

Q: A 1.00 g sample of limonite iron ore, 2Fe203 · 3H20, is dissolved, reduced to Fe²+ and titrated with…

A: In a titration, equivalence point is obtained when the reactants are present in stoichiometric…

Q: 4. A small pilot plant is being tested to treat a newly found ore feed with 5.15 wt% grade Cu. The…

A: The total number of working of plant in 1 year = 360 days (5 days shut down in each year) So, ore…

Q: Potassium dichromate is used to titrate a sample containing an unknown percentage of iron (AW.…

A: We have to tell which option is correct from given choices of options by telling percentage of iron…

Q: Some quantity of metallic iron was dissolved in sulfuric acid, and then Titrated by 17,15 mL KMnO4…

A: Metallic iron dissolved in sulfuric acid in terms of FeSO4 Then by Titration with KMnO4, FeSO4…

Q: Mass of KxFe(C2O4)y · zH2O : 5.60 g Mass of sample : 0.155 g Mass of FeCl3 used in preparation :…

A: The given compound first undergoes dissociation in its aqueous solution as:

Q: A 0.2219 g sample of pure iron (MM = 55.847 g/mol) wire was dissolved in acid, reduced to the +2…

A: Given data, Mass of iron = 0.2219 g Molar mass of iron = 55.847 g/mol Volume of Cerium (IV) =…

Q: A sample of iron ore weighing 0.6248 g is dissolved in acid, the iron reduced to Fe²⁺, and the…

A: Given data,Mass of iron sample=0.6248gVolume of K2Cr2O7=33.60mLNormality of K2Cr2O7=0.1502NFormula…

Q: A sample of magnetite (impure Fe3O4) weighing 0.5000 g is fused with oxidizing flux and the ferric…

A: Magnetite is an ore of Fe with the formula Fe3O4.

Q: Define: (a) ore; (b) mineral; (c) gangue; (d) brine.

A: a) Ore: The mineral from which an element can be extracted easily and profitably is called an ore.…

Q: The sulfur from 4.00g steel is evolved as dihydrogen sulfide gas and titrated with 1.60 mL of…

Q: Write the complete chemical equation of leaching Cuo in acidic solution which produces Cu²* ions.…

A: Leaching CuO in acidic solution which produces Cu2+ ions. We have to write the complete chemical…

Q: Zone refining is used for the:(a) concentration of an ore(b) Reduction of metal oxide(c)…

A: Given options, (a) concentration of an ore (b) Reduction of metal oxide (c) Purification of…

Q: The amount of Fe in a 0.4891 gm sample of an ore was determined by redox titration with K Cr , 0 ,.…

A: Iron Ore is Fe2O3, and redox titration is done with Potassium dichromate K2Cr2O7 Mole of K2Cr2O7 =…

Q: A 1.500 g sample of iron ore, labeled A, was processed accordingly to give 0.5215 g of pure Fe2O3…

A: Mass percent :- The mass in grams of a substance present in 100 grams of the mixture is defined as…

Q: 2. Write the two defect reactions for the solution of Nb2O5 into TiO2 3. Calculate the lattice…

A: Since you have posted multiple questions in a single session we are entitiled to answer first…

Q: Then, for testing the iodide test, the acidified solution of sodium iodide (NaI) reacts with…

A: Answer: Double displacement reaction: When two compounds react with eath other by an exchange of…

Question

1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample?

2. Distinguish between equivalence point and end point.

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

Trending now

This is a popular solution!

Step by step

Solved in 4 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

The aluminum in 0.200 g impure aluminum sulfate ( the sample) was precipitated with aqueous NH3and the precipitate was filtered and ignited to 10000C to give anhydrous Al2O3 (the residue) which weighs 0.150 g. Calculate the %Al ( the %sfc) in the sample.
1,5419 g of magnetite (Fe3O4) ore; Fe+2 and Fe + 3 in concentrated HCL to form a mixtureit's unraveling. Adding HNO3 to all Fe +2s Fe +3 e and Fe+3 s NH, addingwith Fe(OH)3, precipitating into. Sediment in the form of Fe3O4 after necessary operationsand 0.8525 g. Calculate the percentage of Fe3O4 in the sample.
To analyze the amount of iron (Fe; Mw = 55.85 g/mol) contained in an ore sample, the sample was digested with acid and diluted to 50 mL with water. This solution was then treated with 25.00 mL of 0.2922 M EDTA. The excess EDTA was back titrated with 6.47 mL of 0.0843 M Zn2+ to reach the equivalence point. How many grams of Fe contained in the ore sample?
To determine the amount of magnetite. Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, resulting in a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 using NH3. Filtering, rinsing and igniting the ppt provides 0.8525 g of pure Fe2O3. Calculate % Fe in the sample.
The iron content of a large lump of ore is determined by taking a single small sample, dissolving it in acid, and titrating with ceric sulphate after reduction of Fe (III) to Fe (II). What are the possible source of random and systematic errors?
A 5.70 g iron ore was dissolved in concentrated HCl. After the dissolution, the resulting solution was made basic by adding 6.0 M NaOH slowly until the solution is slightly turbid. Urea was then added and the solution was heated for 3 hours. The precipitate was filtered using an ashless filter paper and ignited to form Fe2O3 (159.69 g/mol). The mass of precipitate is 2.1 g. Find the % Fe3O4 (231.54 g/mol) in the iron ore sample.
0.7120 g of iron ore was dissolved and the iron was reduced to Fe2+ with Jones's reagent. Fe(II) was titrated with 0.02086 M KMnO4 and consumed 39.21 mL. What is the iron content of iron ore? Report the concentration as percentage of iron (Fe%) and iron oxide (Fe2O3%).
A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaO
Solve this gravimetric analysis problem. 0.4960 g sample of CaCO3 (mw= 100) is dissolved in an acidic solution. The calcium is precipitated as CaC2O4. H20 (mw = 146) and the dry precipitate is found to weigh 0.6186 g. What is the percentage of CaO (mw=56) in the sample?
To determine the percent purity of a sample containing iron(II) ammonium sulfate; Suggest , 2 different methods for iron(II) ion. Explain in detail what errors may occur in the methods. (volhard method, gravimetric analysis, kjeldahl, etc.) Percentage content: 1-100% ; the solution concentrations to be used are 0.01-0.1M; Take the volumes of solution to be used between 1-50 mL
1. How is complete precipitation assured in the Group III Cations? 2. In the confirmatory test of Magnesium ion, why is it necessary to heat the centrifugate in water bath for 5 minutes? 3. If Magnesium hydroxide is a white gelatinous precipitate, why is the confirmatory result indicated a blue precipitate?
Iron (55.845 g/mol) can be determined gravimetrically by precipitation as Fe(OH)3 (106.867 g/mol) and subsequent inflammation of the precipitate to convert it to Fe2O3 (159.69 g/mol). A 0.7873 g sample to be analyzed was weighed and transferred to a 400 mL beaker, where it was dissolved in 50 mL of H2O and 10 mL of 6M HCl. Then 2 mL of concentrated HNO3 was added to the solution. After boiling to remove excess HNO3 and nitrogen oxides, the solution was diluted to 200 mL, brought to boiling, and Fe(OH)3 was precipitated by the slow addition of 1:1 NH4OH solution until an odor of NH3 was detected (indicating the presence of excess NH3 in the medium). The solution was left in a water bath at 80 ºC for 30 min at rest. The precipitate was then filtered and washed with several portions of hot 1% m/v NH4NO3 until no Cl– was detected in the wash water. Finally, the precipitate was ignited at 500-550 °C, then left in a desiccator to cool and weighed as Fe2O3, resulting in a mass of 0.4512 g.…

SEE MORE QUESTIONS

Recommended textbooks for you

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

SEE MORE TEXTBOOKS