An iron ore was analyzed by dissolving a 2.9912-g sample in concentrated HCI. The resulting solution was diluted with water, and the iron(IlI) was precipitated as the hydrous oxide Fe203-XH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.8394 g of pure Fe203 (159.69 g/mol). If the sample came from an extracted ore that is 50 kg in total, how much iron can be extracted from it? A 9.815 g Fe B 9.815 kg Fe 13.94 g Fe 13.94 kg Fe

An iron ore was analyzed by dissolving a 2.9912-g sample in concentrated HCI. The resulting solution was diluted with water, and the iron(IlI) was precipitated as the hydrous oxide Fe203-XH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.8394 g of pure Fe203 (159.69 g/mol). If the sample came from an extracted ore that is 50 kg in total, how much iron can be extracted from it? A 9.815 g Fe B 9.815 kg Fe 13.94 g Fe 13.94 kg Fe

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

Similar questions

A 0.7041-g sample of impure mercury(II) oxide was dissolved in an unmeasured excess of potassium iodide. Reaction. Calculate the percentage of HgO in the sample if titration of the liberated hydroxide required 40.67 mL of 0.1064 M HCl.
A 6.586-g sample containing magnesium chloride and sodium chloride was dissolved in sufficient water to give 500 mL of solution. Analysis for the chloride content of a 50.0-mL aliquot resulted in the formation of 0.5923 g of AgCl. The magnesium in a second 50.0-mL aliquot was precipitated as MgN H4 PO4 ; on ignition, 0.1796 g of Mg2P2O7 was found. Calculate the percentage of Mg Cl2 x 6H2O and of NaCl in the sample. a. ________% MgCl2 x 6H2O b. ________% NaCl
The arsenic in a 1.203-g sample of a pesticide was converted to H₃AsO₄ by suitable treatment. The acid was then neutralized, and 40.00 mL of 0.05871 M AgNO₃ was added to precipitate the arsenic quantitatively as Ag₃AsO₄. The excess Ag+ in the filtrate and in the washings from the precipitate was titrated with 9.63 mL of 0.1000 M KSCN, and the reaction was: Ag⁺ + SCN⁻→ AgSCN(s).Find the percentage of As₂O₃ in the sample. *
1.3562 g of table salt was taken and dissolved in 250 mL of water. Calculate the % chloride amount in the sample (Cl= 35.5 g/mol), since 3.5 mL of 0.1 M AGNO3 is consumed when 25 mL of this sample is titrated with the Mohr method.
Please write out steps and supply the answer!
the number of moles of Aluminum in 1.3741 g was calculated to be 0.051 moles and that the chemistry student weighed out. For every mole of Aluminum that you start with, you can create one mole of Alum [KAl(SO4)2 ⋅12 H2O(s)]. What is the theoretical yield before drying the Alum precipitate?
A 1.560 g sample of metal ore was dissolved and the metal (Fw=48.12g/mol) was oxidized to a metal oxide anion A2 containing one metal atom per anion molecule (Fw=212.12g/mol). The solution was treated with 20.00 mL of 0.0750 M BNO3 solution. The resulting precipitate of B2A (Fw=416.88g/mol) was removed and discarded. The excess BNO3 (Fw=179.55g/mol) required 11.22 mL of 0.0995 M KD (Fw-60.12g/mol) for complete reaction. Calculate the percent of metal in the ore. Within reason do not round until the end. Report your final answer to the three significant figures. [number]% metal
Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
The arsenic in a 1.208-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The acid was then neutralized, and 44.00 mL of 0.05854 M AgNO, was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag* in the filtrate and in the washings from the precipitate was titrated with 9.69 mL of 0.1000 M KSCN, and the reaction was 3. Ag* + SCN → A£SCN(s) Find the percentage of As2 O3 in the sample. Percentage of As2 O3
The iron content of iron ore can be determined by titration with K₂Cr₂O₇ according to the equation 14H⁺(aq) + Cr₂O₇²⁻(aq) + 6Fe²⁺(aq) → 6Fe³⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l) Diphenyl amine is used as an indicator as it changes color from green to purple when the endpoint is reached. A sample of iron ore with a mass of 1.753 g was dissolved with HCl and then treated with a reducing agent to convert any Fe³⁺ in the ore to Fe²⁺. Titration with 0.0765 M K₂Cr₂O₇ solution required 40.25 mL of the solution to reach the endpoint. The molar mass of Fe is 55.85 g/mol. Calculate mass percent iron in the ore.
A student is given 1.5621 g of pure CuO. To recover the Cu present in the compound, the dark powdery solid was dissolved in 15.0 ML of 6 M HCl and the solution was diluted to 50.0 mL with water. How many grams of Mg is needed to displace all of the copper (II) ions from the solution? Mg(s) + Cu^2+(aq) --> Cu(S) + Mg^2+(aq)
A student is given 1,7709 g of pure CuO. To recover the Cu present in the compound, the dark powdery solid was dissolved in 15.0 mL of 6 M HCl and the solution was diluted to 50.0 mL with water. How many grams of Mg is needed to displace all of the copper (II) ions from the solution? Mg(s) + Cu2+(aq) --> Cu(s) + Mg2+(aq)