/18, 15:36] Nur Izyan Izzati: d. In a synthetic reaction, 4.1268 g copper(II) sulfate pentahydrate and 12.3098 g potassium oxalate monohydrate were reacted to form 5.6009 g copper(II) oxalate complex, and the balanced reaction is shown below: [ CuSO4.5H2O + K2C2O4.H2O --> K2Cu(C2O4)2.2(H2O) + K2SO4 + 5H2O i. Calculate the molarity of copper(II) sulfate and pottasium oxalate reacting solutions, state the limiting reactant. (Molecular weight CuSO4.5H2O = 250.2 g mol-1, K2C2O4.H2O = 184.2 g mol-1) ii. Determine the percentage yield of copper(II) oxalate based on the

/18, 15:36] Nur Izyan Izzati: d. In a synthetic reaction, 4.1268 g copper(II) sulfate pentahydrate and 12.3098 g potassium oxalate monohydrate were reacted to form 5.6009 g copper(II) oxalate complex, and the balanced reaction is shown below: [ CuSO4.5H2O + K2C2O4.H2O --> K2Cu(C2O4)2.2(H2O) + K2SO4 + 5H2O i. Calculate the molarity of copper(II) sulfate and pottasium oxalate reacting solutions, state the limiting reactant. (Molecular weight CuSO4.5H2O = 250.2 g mol-1, K2C2O4.H2O = 184.2 g mol-1) ii. Determine the percentage yield of copper(II) oxalate based on the

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 70AP

See similar textbooks

Similar questions

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-
A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.
A. 1.4639 g sample of limestone was analyzed for Fe, Ca and Mg. The iron was determined as Fe2O3, yielding 0.0357 g Calcium was isolated as CaSO4, yileding a precipitate of 1.4058 g and Mg was isolated as 0. 0627 g of MgP2O7. Report the amount of Febas %w/w Fe2O3, Ca as %w/w CaO and Mg in the limestone sample as % w/w MgO
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)
A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?
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.
Thallium(I) sulfide is a blue-black lustrous crystal that was once used to manufacture photo-electric detectors. 16 Tl(s)+S8(s)------>8Tl2S(s) If 9.6 mol of Tl(s) were reacted with 5.5 mol of S8(s), a) Ti b) S8 would be the limiting reagent and ... mol of Tl2S(s) would be produced.
A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
What mass (in grams) of Na2S2O3 is needed to dissolve 0.44 g of AgBr in a solution volume of 1.0 L, given that Ksp for AgBr is 3.3×10−13 and Kf for [Ag(S2O3)2]3− is 4.7×1013?
Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudburymineral complex. The first step in processing these ores involves “roasting” the ore in air to produce the metalor metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped.Suppose that you roast 1.00 kg of the mineral maucherite, Ni11As8. The balanced equation for thereaction is:2 Ni11As8 + 31 O2 → 22 NiO + 8 As2O5(a) How many kg of NiO can be produced?(b) How many kg of the pollutant As2O5 can be produced?(c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O2 by mass,and that the density of air at 25°C is 1.2 g/L.Molar masses: Ni11As8 1245.0 g/mol NiO 74.69 g/mol As2O5 229.84 g/mol
Think that an alloy Cu-60wt%Ag is slowly cooled from the Liquid Phase Field. How many grams of total alpha are present at 778°C? The total alloy amount is 1000grams
Fe2S3 -----> 2Fe + 3S What mass of sulfur (S) is produced from the thermal decomposition of 12.5g of Fe2 S3?