2+ as (6) A sample of an ore was analyzed for Cu* follows. A 1.25 g sample of the ore was dissolved in acid and diluted to volume in a 250 mL volumetric flask. A 20 ml portion of the resulting solution was transferred by pipet to a 50 mL volumetric flask and diluted to volume. An analysis showed that the concentration of Cu²* in the final solution was 4.62 ppm. What is the weight percent of Cu in the original ore?

2+ as (6) A sample of an ore was analyzed for Cu* follows. A 1.25 g sample of the ore was dissolved in acid and diluted to volume in a 250 mL volumetric flask. A 20 ml portion of the resulting solution was transferred by pipet to a 50 mL volumetric flask and diluted to volume. An analysis showed that the concentration of Cu²* in the final solution was 4.62 ppm. What is the weight percent of Cu in the original ore?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter10: Fuels, Organic Chemicals, And Polymers

Section: Chapter Questions

Problem 115QRT

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Addition of an excess silver nitrate to a 0.5012 g sample yielded a mixture of AgCl and Agl that weighed 0.4700 g. The precipitate was then heated in a stream of Cl2 to convert the Agl to AgCl. 2 Agl (s) + Cl2 (g) 2 AgCI (s) + 12(g) The precipitate was found to weigh 0.3900 g after this treatment. Calculate the percentages of NH4I and NH4CI, respectively. 19.71, 25.07 25.07, 28.72 28.72, 19.95 O 25.07, 19.71 O 19.95, 28.72
A mined alloy sample weighing 2.0840 g is dissolved in minimal amounts of concentrated HNO3 before diluted to 50 mL. Ten mL of this diluted sample was titrated using 0.091 M KSCN and required 14.20 mL to reach the endpoint. Calculate the concentration of silver (%w/w) in the mined alloy. (Hint: A dilution factor (DF) is needed in the formula.) Titration reaction: Agt + SCN- → A9SC'N(s) FW: Ag = 107.87 %3D
A mixture of solid chlorides was known to contain some or all of the following cations: Ag ,Al^3+Cr^3+,Ca^2+,and/or Zn^2+ . A student performed the following steps: 1.Water was added to the solid and the mixture was stirred well. After several minutes, some of the solid did not dissolve. The mixture was centrifuged and the supernatant was decanted from the solid (solution A). 2. NH4CI(aq) was added to solution A followed by NH3(aq) until the solution was basic to litmus. A gray-green precipitate was formed. The mixture was centrifuged and the supernatant (solution B) was decanted. The solid dissolved in NaOH(aq) and H2O2(aq) to form a light yellow solution. The solution was heated to dryness to remove the H2O2 and the solid was redissolved in HCI(aq). When ammonia was added to make the solution basic, a light yellow solution formed and no solid precipitated. 3. (NH4)2C204(aq) was added to solution B, and a precipitate formed. The mixture was centrifuged and the supernatant (solution C)…
An ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)
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
A solution containing chloride ion was analyzed by the Volhard method. A 50.00 mL sample containing chloride ion was treated with 25.00 mL of 0.2500 M silver nitrate. The precipitated AgCl was removed from the solution by filtration, and 1.00 mL of 0.1000 M Fe3+ was added to the filtrate. This new solution was then titrated with 10.67 mL of 0.2380 M KSCN. What is the concentration of chloride ion in the original solution?
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A 0.5962 g sample of iron ore is dissolved in perchloric acid (HCIO4). All iron present is oxidized to Fe3*. The solution is filtered to remove solid matrix materials and made basic with addition of ammonium hydroxide. The iron precipitates as the Fe(OH)3.XH2O gel. The precipitate is collected in a cistern crucible and ignited to produce Fe203. What is the wt. % of iron in the sample if the analysis produced 0.3210 g Fe2O3? Fe3+ + 3 OH → Fe,O3 + → Fe203 H2 18.83% 9.415% 56.49% O 37.66%
To determine the amount of magnetite, Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, giving 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 by adding NH3. Filtering, rinsing, and igniting the precipitate provides 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
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 silver ion in a 25.00-mL sample was converted to dicyanoargentate (l) ion by the addition of an excess solution containing Ni(CN), ²: Ni(CN), + 2 Ag' → 2Ag(CN)2" Ni2 The liberated nickel ion was titrated with 43.77-mL of 0.02408M EDTA. concentration of the silver solution. Molar Masses: Ni = 58.69 Ag Calculate the molar - 107.9

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