A 2.500g sample containing Ce++ was treated with excess iodate to precipitate Ce(IO3)4. The precipitate was collected, dried, and ignited to produce g of CeO2. What was the original weight percent of Ce in the original solid?(15) aining only C. H. and maybe N was
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- NoneA sample of processed meat scrap weighing 4.000 g is digested with concentrated HSO. and Hg(catalyst) until the N present has been converted to NHHSO.. This is treated with excess NaOH, and the liberated NHs is caught in a 100-ml of H.SO. ( Iml 0.01860 g Na:OJ. The excess acid requires 57.60 ml of NaOH ( ImL = 0.12660 g potassium acid phthalate, KHCaH.OJ. Calculate the percentage protein in the meat scrap 4.A 0.64 g sample containing KCl ( mw = 74.6 ) is dissolved in 50mL of water and titrated to the Ag2CrO4 end point, requiring 26.2 mL of 0.15 M AgNO3 .The %w/w KCl in the sample is ?
- 6. (2 pts) Aqueous solutions of a compound did not form precipitates with Cl', Br', I, SO,²', CO;²', PO4³-, OH", or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified with HCl (aq). This compound is A) Pb(NO3)2 B) (NH4)2S C) KBr D) Li2CO3 E) AgNO3Please Provide General Accounting Question SolutionWhat is the solution of this? The given answer is 74.19 mL ; 74.19 mL
- 0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)1. A student synthesized 3.214g of Ni(NH3)„Cl2 from 4.023g of N¡C12•6H2O. He dissolved 0.81g of Ni(NH3)nCl2 in 40 mL of 1.0M HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 1T; H2O 18. (1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = ɛbc. (2) The student used 38.75 mL of 0.498M NaOH to neutralize excess HCl in 40mL of the sample. Calculate the mass percent of NH3 in the product.A2.880 g sample contain thiourea (NH,),CS (76.12 amol) was extracted into a dilute H,SO, solution and titrated with 35.42 mL of 0.008221 M Hg according to the following reaction 4(NH2)2CS+Hg*. [NH,)2CS],Hg Calculate the %((NH2),CS in the sample? 1 090.829 % 2 O0.005% 3. 03.079 9% 4 045 44 %
- COMPLEX PREPARED (preparation #3 ) cuclz H20 Starting metal salt (MXx,_H;O) Copper (T)chloride dinydrate Metal (Cu or Co) cu Halide (Cl or Br) CL Amine (en, bu, pz, or dien) bu (1] Yield of the Complex Mass of crystalline product (Exp. Yield) 29.682 (2a) Determination of Copper Calculate the mols of Na,S:O, to reach the end point, and then calculate the moles of Cu from the stoichiometry. Finally, calculate the % Cu in the sample. Show your calculations on the next page. Trial 2 Trial 1 O.103g 20.5mL Mass of product,g 0.19 21.ML Vol. of Na;S:O, to reach the end point, ml. Molarity of NazS;0, (from bottle) 0.0100M 0.0002 05 0.000 205 0.000 210 O.000 210 Mols of NazS:O, Mols of Cu Mass of Cu, g 0.0130 0.0133 % Cu in product Ave % Cu Calculations: O.100 M = mol 0.0 20SL 63.55 = 9 0.0002DS %3D O 10100 M = mol o021 니 63.55 = 0.00021 %3D 855. 0.1500 g sample of chromium ore was dissolved and the chromium oxidized to chromate ion. The solution was treated with 25.00 mL of 0.3500 M AGNO3. The resulting precipitate, from the reaction of the excess and analyte in 1: 1 mole relationship, Ag2CrO4 was removed and discarded. The excess AGNO3 required 30.50 mL of 0.200 M KSCN for titration in a 1:1 mole relationship. Calculate the % Cr2O3 in the ore if the mole relationship between Cr2O3 and CrO42- is 1:2 respectively.A 0.8965g ore sample is dissolved in nitric acid and then filtered. The aluminum is present in solution as AP". The solution is made basic with ammonium hydroxide, NH,OH, and the aluminum hydroxide, Al(OH)» (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed. The resulting alumina, Al;O; (FW 101.94), weighed 0.1605 g. Why is the solution filtered after acid dissolution? Why rinse with ammonium hydroxide solution? What chemical transformation takes place during ignition? (Show the balanced chemical equation) • Why use a desiccator during cooling? Calculate the weight percent Al (AW 26.9815) in the sample. Al(OH)) -> Al;O, + H0