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- 1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.What is the gravimetric factor for analysis of Fe in magnetite ore if the precipitate is Fe2O3 ?MM=molar mass a. MMFe/MMFe2O3 b. 2MMFe/3MMFe2O3 c. MMFe/2 MMFe2O3 d. 2MMFe/MMFe2O3A 5.186 gram sample of the anti-malarial pesticide DDT was dissolved in 100.0 mL of alchohol and 10.00 mL aliquots were taken for analysis. One such aliquot was decomposed with metallic sodium, and the liberated chloride ion was precipitated as AgCl. Express the results of this analysis in terms of %DDT (C14H9Cl5, FW = 354.49) based on the recovery of 150 mg of AgCl (FW = 143.32).
- You are a chemist, you know that in the analysis for total hardness, formation of Ca-EDTA complex in the presence of magnesium-calmagite indicator or Mg-Ind complex involves the following process: Based on the chemical reactions provided, what is equivalent to KMg-Ind?The iron content of a large lump of ore is determined by taking a single small sample, dissolving it in acid, and titrating with ceric sulphate after reduction of Fe (III) to Fe (II). What are the possible source of random and systematic errors?Hardness in groundwater is due to the presence of metal ions, primarily Mg2+and Ca2+. Hardness is generally reported asppm (mg/L) CaCO3or mmol/L Ca2+. To measure water hardness, a sample of groundwater is titrated with EDTA, a chelating agent, in the presence of the indicator eriochrome black T, symbolized here as In. Eriochrome black T, a weaker chelating agent than EDTA, is red in the presence of Ca2+and turns blue when Ca2+is removed. A 50.00-mL sample of groundwater is titrated with 0.0850M EDTA. Assume that Ca2+accounts for all of the hardness in the groundwater. If 10.10 mL of EDTA is required to titrate the 50.00-mL sample, what is the hardness of the groundwater in molarity Ca2+and in ppm CaCO3?
- Solve this gravimetric analysis problem. 0.4960 g sample of CaCO3 (mw= 100) is dissolved in an acidic solution. The calcium is precipitated as CaC2O4. H20 (mw = 146) and the dry precipitate is found to weigh 0.6186 g. What is the percentage of CaO (mw=56) in the sample?To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)
- what mass in grams of Na2S2O3 is needed to dissolve 4.7 g of AgBr in a solution volume of 1.0 L given that Ksp for AgBr is 3.3 x 10^-13 and Kf for [Ag(S2O3)2]^3- is 4.7 x 10^13?You are a chemist, you know that in the analysis for total hardness, formation of Ca-EDTA complex in the presence of magnesium-calmagite indicator or Mg-Ind complex involves the following process: Based on the chemical reactions provided, what is equivalent to KCa-EDTA?A first-stage recovery of magnesium from seawater is precipitationof Mg1OH22 with CaO:Mg2+(aq) + CaO(s) + H2O(l)---->Mg(OH)2(s) + Ca2+(aq) What mass of CaO, in grams, is needed to precipitate 1000lb of Mg(OH)2?