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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- 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 ?Please Provide General Accounting Question Solution1. 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.
- A 25.00-mL solution containing Cl- was treated with excess AgNO3 to precipitate 9.53 g of (FM 143.321). What was the molarity of Cl- in the unknown? C) 4.550 D) 0.3048 O A) 3.578 B) 2.660A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.27² +1052 Zn [Zn(H₂0) 3 (CO3)3 + EXCESS (052 2 Mile Zy [24 (H₂O)) ((0₂)₂ + Excess Co znoks E2₁ (H₂0ls (03) + Excess con 2 MUR 724103 A- How many moles OF 20003 will be prodnad & each Raction B. Explain In Detail te types of chanical Butching That i Hanned yosh alshes
- 1. A sample of feldspar weighing 1.500g is decomposed, and eventually there is obtained a mixture of KCI and NaCi weighing 0.1801 g. These chlorides are dissolved in H20, a 50-mL pipetful of 0.08333 N AGNO3 is added, and the precipitate is filtered off. The filtrate requires 16.47 mL of 0.100ON KCNS, with ferric alum as indicator. Calculate the percentage of K20 in the silicate.The unknown solution contained… (multiple choice)What are the respective concentrations (M) of Cu+2 and Cl- afforded by dissolving 0.200mol CuCl2 in water and diluting to 345 mL?A) 0.200 and 0.200 B) 0.580 and 1.16 C) 0.200 and 0.400 D) 1.16 and 2.32E) 0.580 and 0.290
- 30.0 ml solution of I was treated with 50.0 mL of 0.365 M AgNO. Agl (s) was filtered off, and the filtrate (plus Fe3+) was titrated with 0.287 M KSCN. When 37.60 mL had been added, the solution turned red. How many milligrams of I were in the original solution? (Given At. Mass of lodine = 126.9)(5) A standard sclution of hydrated iron(II) sulphate, FeSO,.XH20, was preparcd by dissolving 5.8 g of the salt in a volumetric flask and making it up to 250 mL (250 cm³). Twenty-five millilitres (25 mL (25 cm³)) of this solution was acidified and found to react exactly with, 22.8 cm³ (22.8 mL), of 0.018 M potassium 3 permanganate solution. The half-equations for the reaction are: JAS 00 MAC aJTT MNO4 (aq) + 8H*(aq) Fe*(aq) + Mn2“(aq) + 4H20(1) → Fe*(aq) + e MOTTAMIMAXE 2+ (i; What is the indicator for the titration of a solution of iron (II) sulphate and potassium permanganate soluticn? (ii) Indicate the colour at the end point if the permanganate is in the burette. blood ofieido rosd sl (iii) Why is it necessary to acidify the iron(II) solution before titration? o sd am eorsiuolsFind Ecell = 0.48V. Use dhis regult along with the equilibrium conlentretion of Lu“ (mol/L) wheun 24. C[Cu (NH3), ) = 0.10 mol /L and [N H3] = 6.1 mol/h to calceulate the cqnillibriem Lonstant for the formation of [cu(NH3),]"]