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- Calcium fluoride is considered as a relatively insoluble compound and therefore lime or slakedlime has been considered as a possible material to remove excess fluoride in water of boreholesin certain parts of the country. The solubility product of CaF2 is Ksp = 3 x 10 – 11 and that ofCa(OH)2 isKsp =8x10-61. How much lime can be added to the water to remove 10 mg of F- ion per litre ofborehole water?(The atomic masses are Ca: 40.08; F: 19.00; O: 16; H: 1)Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of thesePlease compare the solubility of ferrihydrite (Fe(OH)3) and goethite (FeOOH), with dissolution reactions provided. FeOOHgoethite + 3 H+ à Fe3+ + 2 H2O Fe(OH)3(ferrihydrite) 3 H+ à Fe3+ + 3 H2O
- What is selective precipitation? What is confirmatory test and its significance? What are the products formed when Group 1 cations are allowed to react with KOH? Why is it necessary to have an acidic environment when separating Group 1 cations from other metal ions?What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
- 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.Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.A piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.
- A mineral in a fine state of division (0.6324 g) was dissolved in 25.0 mL of 4.0 mol / L boiling HCl and diluted with 175.0 mL of H2O containing two drops of methyl red indicator. The solution was heated to 100 ° C and a heated solution containing 2.00 g of (NH4) 2C2O4 was added slowly to precipitate CaC2O4. Next, NH3 6.0 mol / L was added until the indicator changed from red to yellow, indicating that the liquid was neutral or slightly basic. After slow cooling for 1 hour, the liquid was decanted, the solid transferred to a crucible and washed five times with 0.10 wt% (NH4) 2C2O4 solution, until no Cl- was detected in the filtrate with the addition of AgNO3 solution. The crucible was dried at 105 ° C for 1 hour and then taken to an oven at 500 ° C ± 25 ° C for two hours. The mass of the empty crucible was 18.2311 g. The crucible mass with CaCO3 (s) was weighed 5 times to an average of 18.5467 g. Determine the percentage, by mass, of Ca in the mineral. Ca (40.078 g / mol); C (12.01078…Why does the solubility of a salt of a basic anion increase with decreasing pH? Write chemical reactions for the minerals galena (PbS) and cerussite (PbCO3) to explain how acid rain mobilizes trace quantities of toxic metallic elements from relatively inert forms into the environment, where the metals can be taken up by plants and animals. Why are the minerals kaolinite and bauxite in Box 12-1 more soluble in acidic solution than in neutral solution?Sometimes it is not possible to indicate the end point of a titration.a) How can one proceed then and what is the name of the type of titration that can be performed? Briefly describe. An example in which this method can be used is in the determination of mercury, which forms strong complexes with EDTA, but for which there is no suitable indicator that can indicate the end point. b) You are given the task of determining the Hg2 + concentration in a sample solution? After adding an excess of EDTA, the sample solution is titrated with a magnesium solution. 20.00 ml of a 0.0452 M EDTA solution was added to 30.00 ml of sample solutionThe excess EDTA was determined by adding 0.0500 M Mg 2+ solution, consuming 4.37 ml to the end point.