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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- What mass of AgI can be produced from a 0.512-g sample that assays 20.1% Al13? Precipitates used in the gravimetric determination of uranium include NazU2O7 (634.0 g/mol), (UO;);P¿O, (714.0 g/mol), and V205 - 2U03 (753.9 g/ mol). Which of these weighing forms provides the greatest mass of precipitate from a given quantity of uranium?A 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
- 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.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 856. The phosphorus content in a 0.3004-g sample was precipitated as (NH4);PO4 .12M0O3 a slightly soluble precipitate. The precipitate was filtered, washed, and further redissolved in acid. The resulting solution was treated with an excess of Pb²* resulting in the formation of 0.3017 g of PbMoO4. Calculate the % w/w of P2Os.||
- 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.1.5g sample contains sulfur S (aw332) has been dissolved. The sulfur is precipitated as BaSO4 (mw = 233). If the weight of the precipitate is 0.65g the * :percentage of sulfur in the sample is 5.95% 31.69% 7.82% 7.18% OA 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) 2.660