STANDARDIZE THE Na,Si02.5H;0 WITH KIO. Weight of KIO, = 0.5325 g V ot KIO, = 250 ml N KIO, V KIOL ml. 7.0 7.0 VNazs:O.5H20, mL 8.2 7.5 N NasO.SH;0 Average N Nays:O, SH;O
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- Solution for 0.105g of the K3[Fe(C2O4)3] (MW= 437.2 g/ mol) were dissolved in sulfuric acid and got rated with 9 mL of 0.028M KMn04. What is the experimental weight percent of oxalate in the sample?A sample of iron ore weighing 800 mg was treated with HNO3 , boiled to dryness and redissolved in dilute HCl. After filtration and removal of undissolved silica, the liquid was passed through a Walden reductor. The collected sample was titrated with 0.0210 M KMnO4 , requiring 12.0 mL to reach the end point. Calc %Fe (55.845) in the ore.In the development o f an analytical method for the quantitative analysis o f iron using Atomic Absorption spectrophotometry (AAS), a linear calibration curve for standards o f 0.00, 5.00, 10.00, 15.00 and 20.00 ppm was prepared. An iron ore sample with an expected iron content o f 40-60% w/w is to be analysed by this method. An approximately 0.5-g sample is taken, dissolved in a minimum amount o f concentrated HC1 and diluted to 1 L in a volumetric flask using distilled water. A 5.00-mL aliquot is removed with a pipette. With explanation, to what volume (10, 25, 50, 100, 250 500 or 1000 mL) should the 5.00 mL aliquot be diluted, to minimize the uncertainty in the analysis?
- 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 tabletDESCRIBE THE PROCEDURE OF d) 600 mL of 3.00% (w/v) aqueous BaCl2from a 0.400 M BaCl2solution. (e) 2.00 L of 0.120 M HClO4from the commercial reagent [71.0% HClO4(w/w), specificgravity1.67]. (f) 9.00 L of a solution that is 60.0 ppm in Na+, starting with solid Na2SO4When titrated in neutral solution with 0.05000 N I2, a mixture of As2O3, As2O5, and inert material requires 20.10 ml. The resulting solution is then acidified, and excess KI is added. The liberated I2 requires 29.92 ml of 0.1500 N NaS2O3 . Calculate the sum of the weights of As2O3 and As2O5 in the sample.
- 5.00 mL of stock solution is diluted to 25.00 mL, producing solution ALPHA. 10.00 mL of solution ALPHA is diluted to 25.00 mL, resulting in solution BETA. 10.00 mL of solution BETA is then diluted to 25.00 mL, producing solution GAMMA. dilution factor for ALPHA from stock solution = 0.167 dilution factor for BETA from ALPHA solution = 0.0476 part c and d?Aleks data for AgBrO3 is 5.38 x 10^-5In an analysis of chromium in steel containing 1.76% Cr. 0.5000 g of that steel is weighed and dissolved in acid, whereupon the Cr is oxidized to Cr2O72- (dichromate), and blunt to a volume of 250 mL. A 10 mL aliquot of this solution is diluted with water and acid to a final volume of 100 mL. The resulting solution shows a transmittance of 41.7% in a 1 cm pathlength cell. When a 0.7500 g sample of unknown steel is dissolved in acid, oxidized, and diluted to 250 mL, the resulting solution exhibits a transmittance of 61.3% under identical experimental conditions. What is the percentage of Cr in the steel?
- What is the percentage of Nickel in an ore if, when analyzed by the cyanide method, 20.00mL of KCN solution (containing 1.00mmol of AgNO3 per milliliter) are used? Wt of sample used = 0.2500g0.4545 g CaCO3 was dissolved in HCl and the resulting solution was diluted to 0.25 L. Twenty-five mL aliquot of this solution required 35.2 mL of EDTA upon performing titrimetric analysis. Determine the mass of NaH2Y·2H2O to prepare 0.5 L titrant solution. NaH2Y·2H2O is a cmpound with MW = 372.2 g/mol Note: H2Y2- = EDTAA 0.1017-g sample of KBrO3 (MW = 167 g/mole) was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated iodine required 39.75 mL of a sodium thiosulfate solution. Calculate the molar concentration of the Na2S2O3. BrO3 - + 6I + 6HCl → Br - + 3I2 + 6KCl + 3H2O I2 + Na2S2O3 → 2NaI + Na2S4O6 The type of redox titration reaction is ___. a. iodimetry b. bromination c. iodometry d. diazotination The role of KBrO3 in the titration is ___. a. reducing agent b. oxidizing agent c. source of Br2 d. source of I2 At the endpoint of titration, the equivalence of sodium thiosulfate is equal to the following, EXCEPT ___ . a. equivalence of KI b. equivalence of liberated I2 c. equivalence of KBrO3 d. none of the other choices