A solid mixture weighing 0.515 g contained only ferrous ammonium sulfate and ferrous chloride. The same was dissolved in 2 M H2SO4, and the Fe2+ required 12.85 mL of 0.1300 M Ce4+ complete oxidation to Fe3+. Calculate the for weight percent of SO42- in the original sample. (FESO4(NH4)2S04'6H2O FM 392.12; FeCl2-6H2O FM 234.84)
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- Six iron tablets containing FeSO4.7H2O were dissolved in 100-ml of 0.1M HNO3 with gentle heating. All of the Fe2+ is converted to Fe3+ by the strong oxidizing conditions. After the solution had cooled to room temperature , 2.5-ml of 35wt% NH4OH was added. The precipitate Fe2O3-xH2O that was filtered weighed 0.345g. Thermogravimetric analysis of the crude product showed a 10.5% weight loss . A. How many waters of hydration were in the precipitate B. How much iron is present in each tabletIf a sample of silver coin weighing 0.2500 gives a ppt of AgCl weighing 0.2991, what wt of AgI could have been obtained from the same wt. of sample, and what is the percentage of Ag in the coin?(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 eorsiuols
- 5. 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.calculationS H= 1 Fe = 55.8; S = 32; O= 16; 10 10g of an impure iron(11) salt were dissolved in water and made un to 200 cm of solution. 20cm of this solution, acidified with dilute sulphuric acid, required 25 cm3 of 0.04 M KMNO4(aq) before a faint pink colour appeared. (a) Write a balanced ionic equation (or half-equations) for the reaction of acidified manganate(vII) (permanganate) ions with iron(11) ions. (b) How many moles of iron(1) ions react with one mole of MnO4 ions? (c) How many moles of Fe2 react with 25 cm' of 0.04 M KMNO4(aq)? (d) How many grams of Fe2 are there in the 200 cm' of original solution? (Fe 56) (e) Calculate the % by mass of iron in the impure iron(11) salt.In a titration experiment, 25.0 ml of 0.0500M Sn was titrated with 0.10OM Fe in I M HCl to give Fe and Sn', using Pt and calomel electrodes Fe (aq) +e Fe (aq) E" = 0.732 V Sn (aq) +2e Sn E 0.139 V E(calomel) = 0.241VN Calculate E when 28.5mL of Fe is added.
- The digestion of a 0.1432 g sample of a compound containing phosphorous in a mixture of HNO3 and H2SO, resulted in the formation of CO2, H2O and H3PO4 Addition of ammonium molybdate yielded a solid having the composition (NH)3PO, 12M0O3 (MW=1876.3 g/mol). This precipitate was filtered washed, and dissolved in 50 00 mL of 0.2000 M NaOH: (NH,)3PO4-12MO03(s)+ 26OH (aq) HPO,2 (aq) +12M00,2 (aq) +14H2O(1) + 3NH3(g) After the solution was boiled to remove NH3, the excess NaOH was titrated with 14.71mL of 0.1741 M HCI to a phenolphthalein end point (back titration). Calculate the percentage of phosphorous in the solid sample. 6.19% 10.6% O 27.6% O0 238% O 19.5+ 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 rThe Fe content in a water sample from a well was determined by subjecting an aliquot of 25.00ml of sample to treatment with HNO3, excess SCN- and finally a dilution of the treated solution to 50.00mL with distilled water. A 10.00ml aliquot of a 5.97 x 10-4M Fe3 + solution was treated in the same way. It was observed that the color of both solutions was the same when the optical path of the standard solution was 3.04cm and that of the well water sample was 2.61cm. Determine the ppm of Fe in the well water sample.
- (c)Ions that react with Ag+ like SCN- can be determined electrogravimetricallyby deposition on a silver working anode:Ag(s) + SCN- ≤ AgSCN(s) + eA silver anode with initial mass of 12.4730 g was used to electrolyse 85.00 mL of asolution of 0.0245 M KSCN. At the end of the experiment, the anode weighed12.5767 g. How long did the experiment take, if a current of 100 mA was used?Calcium in a 5.00 mL urine sample was precipitated, redissolved and required 16.15 mL of 0.1157 N KMnO4. Calculate the % (w/v) of calcium in the urine.In Fe + O2 --> Fe2O3 what is the coefficient for Fe?