OWLV2 Online teachin XCthe Deep Blue Compound ( +https://cvg.cengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator%=Dassignment-take&takeAssignmentS[References]The deep blue compound Cu(NH3)4SO4 is made by the reaction of copper(II) sulfate and ammonia.CUSO4 (aq) +4 NH, (aq) → Cu(NH3)4SO4 (aq)If you use 27.0 g of CuSO4 and excess NH3, what is the theoretical yield of Cu(NH3),SO, ?g Cu(NH3)4SO4If you isolate 22.0 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4SO4?Submit AnswerTry Another Version8 item attempts remainingShow Hintsearch

The stoichiometry is directly related to the quantitative relationship present between chemicals…

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Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter26: Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 26.15QAP

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Give typed full explanation A stock solution of lithium phosphate (Li3PO4, MM= 115.794361 g/mol) is prepared by dissolving 295.8 g Li3PO4 in deionized water to a final total volume of 1.000 L. Suppose a 1.000-mL aliquot is taken from this stock solution and transferred to a new container to which deionized water is added until the total volume is 50.00 mL. A new 1.000-mL aliquot is taken from this 50.00 mL solution and transferred to a third container to which deionized water is added until the total volume is 25.00 mL. Calculate the number of individual lithium ions (Li+) in the final 25.00-mL solution. Note that lithium phosphate is a strong electrolyte that completely dissociates in water (note that (aq) means the species is a solute in an aqueous solution): Li3PO4 (aq) 3 Li+ (aq) + PO43– (aq) Report your answer to two significant figures. Use scientific notation. Example: 1.0*10^23 (this notation means 1.0 1023)
The Philippine Toxic and Hazardous Wastes Act places limits on the quantities of toxic substances thatmay be discharged into the sewerage system. Guidelines on hexavalent chromium (Cr6+) limits the dischargeamount to just 0.50 mg/L. If an industry dumps hexavalent chromium in the form of potassium dichromate(K2Cr2O7), what is the maximum allowable concentration of hexavalent chromium in molesper liter of sewage water?
A 0.7336-g sample of an alloy that contains copper and zinc is dissolved in 8 M HCl and diluted to 100 mL in a volumetric flask. In one analysis, the zinc (At. Mass = 65.38 g/mol) in a 25.00-mL portion of the solution is precipitated as ZnNH4PO4, and isolated as Zn2P2O7 (FM = 304.70g/mol), yielding 0.1163 g. The copper (At. Mass = 63.55 g/mol) in a separate 25.00-mL portion of the solution is treated to precipitate CuSCN (121.63 g/mol), yielding 0.2383 g. Calculate the %w/w Zn and the %w/w Cu in the sample.
A solution of sodium thiosulfate, Na2S2O3 was standardized by dissolving 0.188 g of KIO3 (MM = 214.00) in water, adding a large excess of KI, and acidifying with HCl. The liberated iodine required 18.25 mL of the thiosulfate solution to decolorize the blue starch/iodine complex. Calculate the molarity of Na2S2O3 solution. Stoichiometry of the reaction is: 1 mol IO3- = 3 mol I2 = 6 mol S2O32-
1A. What weight (in grams) of oxalic acid (MW= 90 g/mol) will be required to prepare 1 liter of 0.25 N? 1b. What weight in milligrams of potassium iodate would liberate sufficient iodine to consume 25.9mL of 0.1N sodium thiosulfate? Mw potassium iodate is 214 g/mol
. Fulgurites are the products of the melting that occurswhen lightning strikes the earth. Microscopic examinationof a sand fulgurite shows that it is a globule with variablecomposition that contains some grains of the definitechemical composition Fe 46.01%, Si 53.99%. Determinethe empirical formula of these grains.
An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)
Pls give with reason, the type and name of the reaction.
The use of silica to form slag in the production of phospho-rus from phosphate rock was introduced by Robert Boyle morethan 300 years ago. When fluorapatite [Ca₅(PO₄)₃F] is used inphosphorus production, most of the fluorine atoms appear in theslag, but some end up in toxic and corrosive SiF₄ (g).(a) If 15% by mass of the fluorine in 100. kg of Ca₅(PO₄)₃F forms SiF₄, what volume of this gas is collected at 1.00 atm andthe industrial furnace temperature of 1450.°C?(b) In some facilities, the SiF₄ is used to produce sodium hexa-fluorosilicate (Na₄SiF₆) which is sold for water fluoridation: 2SiF₄(g)+Na₂CO₃(s)+H₂O(l) →Na₂SiF₆(aq)+SiO₂(s)+CO₂(g)+2HF(aq) How many cubic meters of drinking water can be fluoridated toa level of 1.0 ppm of Fusing the SiF₄ produced in part (a)?
A student determined the chloride content of a commercial salt by using the Mohr method. A 0.7725 -g sample of the salt was dissolved in distilled water and diluted to a final volume of 250. mL. A 25.-mL aliquot of the analyte solution was then titrated against a standard 0.0347 M AgNO3(aq) solution to the chromate end-point. A blank-corrected volume of 25.96 mL was recorded. Calculate the percent chloride in the sample.
A 0.5 g sample of an alloy containing 30% (m/m) iron (MM 55.84 g/mol) is dissolved in acid and diluted to 1 L with deionized water. A 10 mL aliquot was taken for analysis, conveniently diluted and included with an excess of ammonium hydroxide, which led to the formation of a reddish solid. After filtration and washing, the solid was calcined to Fe2O3 (MM 159.69 g/mol). Calculate the mass of this final product.
The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.

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