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 is the solution of this? The given answer is 74.19 mL ; 74.19 mLCOMPLEX 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, + H0None1. 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.
- A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O;. The following steps detail the transformation of Fe,O; (a9) to elemental iron. I Enough sulfur trioxide gas was bubbled to Fe,O; aqueous suspension to completely yield ferric sulfate. IL Then, 5.00 M nitric acid was added to ferric sulfate yielding aqueous solution of ferric nitrate I. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron. and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products а. Write the balanced chemical reaction (s, 1, g). (CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express your answers in 3 significant figures. High-concentration HCl is supposed to be added at the last part of the procedure. с. Briefly state its purpose.(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 eorsiuols5.2 A 5.199 g sample containing the mineral tellurite was dissolved and then treated with 50.00 mL of 0.03144 M K2Cr2O7. Upon completion of the reaction, titration of the excess Cr20, required 37.28 mL of 0.1083 M Fe* solution. Calculate the percentage by mass of TeO2 (FM 159.60) in the sample. The reactions are 3 TeO, + Cr2O,- +8 H3 H;TeO4 +2 Cr + H;O Cr:O + 6 Fe + 14 H2 Cr + 6 Fe* + 7 H:O
- Find 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),]"]+ H (a) CuCN (b) CaCO3 (c) Ag₂CO3 (d) PbBr₂ (e) Y(OH)3 Periodic Table B W Chapter... Supporting Materials Additional Materiala [Ca²+] = 5.2 x 104 M, [CO32- ] = 6.5x 10-6 M * G Please use the values in the resources listed below instead of the textbook values. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated. [Cu] = 1.9x10-10 M, [CN] = 1.9x10-¹0 M [Ag+] = 1.8x10-5 M, [CO32] = 2.7x10-² M [Pb²+] = 1.2x 10-2 M, [Br] = 2.4x10-2 M [Y³+] = 3.5x 10-16 M, [OH-] = 6.6x 10-³ M Constants and Factors №. webassign.net ● F 893 Supplemental Data L C C a Ⓒ + D rA 20 mL volume of 0.015 M KIO3 containing an excess of KI, is added to a 0.312 g sample of a Real Lemon solution containing vitamin C. The Yellow-brown solution, caused by excess I2 is titrated to a colorless starch endpoint with 11.3 mL pf 0.106M Na2S2O3. - What is the equation for I2 * starch deep blue color disappearance?