Q2- A 30.0 mL H2C2O4 acidified solution, was treated with 25.0 mL of 0.102 M KMNO4 solution. The reaction: 2MNO4- + 5 H2C,0,+ 6H → 2MN²++10CO2 + 8H20 The excess permanganate required 8.34 ml of 0.053 M Fe2* solution, the reaction MnO4 + 5FE2++ 8H+ g Mn²+ +5FE3* + 4H2O Find the molarity of the H2C204 solution
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- Q2- A 30.0 mL H¿C2O4 acidified solution, was treated with 25.0 mL of 0.102 M KMNO4 solution. The reaction: 2MNO4- + 5 H2C2O4+ 6H → 2Mn2+ +10CO2 + 8H20 The excess permanganate required 8.34 mL of 0.053 M Fe2* solution, the reaction Mno4 + 5FE2++ 8H+ g Mn²+ +5FE3+ + 4H2O Find the molarity of the H2C2O4 solutionSix 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 tabletQ2- A 30.0 mL H2C204 acidified solution, was treated with 25.0 mL of 0.102 M KMNO4 solution. The reaction: 2MNO4- + 5 H2CO4+ 6H → 2MN2* +10CO2 + 8H20 The excess permanganate required 8.34 mL of 0.053 M Fe2* solution, the reaction Mno“ + 5FE2++ 8H+ g Mn2+ +5FE3+ + 4H20 Find the molarity of the H2C2O4 solution
- A 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.A 0.64 g sample containing KCI ( 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 KCI in the sample isExactly 0.2220 g of pure NazCO; was dissolved in 100.0 mL of 0.0731 M HCl. What mass in grams of CO2 were evolved? Na2CO3 + 2HCI → 2NaCl + CO2 + H2O Na=23 C=12 O=16 Cl=35.5 H=1
- The 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.A sample of Al;(SO.); weighing 7.52-g was dissolved in enough water and diluted to 250.0-mL. 100.0-mL of the dilution was transferred to another flask, 10.0-mL of 0.050M EDTA, 20-ml of buffer solution, 50-mL of alcohol and 2.0-ml dithizone TS were added. The resulting solution required 8.7-mL of 0.031M ZnSO, to reach the endpoint. (Note: Each ml of 0.050M EDTA is equivalent to 16.66-mg Al:(SO.);•18H;0). Compute for the percent purity of the sample.2. In one gravimetric analysis, the aluminum in a 1.2g sample of impure NHAI(SO4)2 was precipitate as hydrous ALO3.XH2O. The precipitate was filtered and ignited at 1000 °C to give anhydrous Al2O3 which weighed 0.1798g. Calculate the % Al inthe sample. 3. A sample of 0.4500g impure potassium chloride was dissolved in water treated with excess silver nitrate solution. 0.8402 g of silver chloride was precipitated. What is the percentage of potassium chloride in the sample?
- 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(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 eorsiuolsA 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 ?