Don't used Ai solution Using the thermodynamic data given in the following table, calculate an activity diagramshowing the stability fields of gibbsite {Al(OH)3}, kaolinite {Al2SizOs(OH)4},pyrophyllite {Al2Si4O10(OH)2}, Ca-beidellite{Ca1/6Al7/3Si11/3010(OH)2},andlaumontite {CaAl2Si4O12 4H₂O} at 25°C. Your diagram should have aCa2+/(aH)2 as they-axis and aH4SiO40 as the x-axis. Also, plot the lines representing saturation with quartzand amorphous silica:AG° (kJ mol)AG° (kJ mol)gibbsite-1151laumontitekaolinite-3800 CaCa2+-6711-553.58pyrophyllite-5275 H₁SiO4º 0Ca-beidellite-1316.6-5388 H2O(1)-237.15Note, you will need to calculate 7 boundaries: gibbsite-kaolinite,gibbsite-laumontite, kaolinite-laumontite, laumontite-Ca-beidellite,kaolinite-Ca-beidellite, kaolinite pyrophyllite, and pyrophyllite-Ca-beidellite.

First boundary lineFirst, let's write out the chemical formulas: Gibbsite: Al(OH)₃ Kaolinite:…

Answered: Using the thermodynamic data given in…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter20: Chemistry Of Selected Transition Elements And Coordination Compounds

Section: Chapter Questions

Problem 38QRT

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An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)
To determine the amount of magnetite. Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, resulting in a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 using NH3. Filtering, rinsing and igniting the ppt provides 0.8525 g of pure Fe2O3. Calculate % Fe in the sample.
To measure the nickel content in steel, the alloy is dissolved in 12 M HCl and neutralized in the presence of citrate ion, which maintains iron in solution. The slightly basic solution is warmed, and dimethylglyoxime (DMG) is added to precipitate the red DMG-nickel complex quantitatively. The product is filtered, washed with cold water, and dried at 110°C. a) If 1.1634 g of steel gives 0.1795 g of precipitate, what percentage of Ni is in the steel?
Please 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
Please write a balanced formula for U(VI) (as uraninite; UO2) using Mn2+ as a reductant for U(VI) and MnO2 pyrolusite as a product.
An ore containing magnetite, Fe3O4 was analyzed by dissolving a 1.5419 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
Pyrolusite (MnO2) is dissolved in hydrochloric acid:MnO2 + HCl → MnCl2 + H2O + Cl2The chloride was passed into potassium iodide solution where it liberated iodine:Cl2 + KI → KCl + I2The iodine liberated was estimated by adding sodium thiosulfate, the reaction beingI2 + Na2S2O3 → NaI + Na2S4O6If 5.6 g of crystallized sodium thiosulfate, Na2S2O3 5H2O ,were used up, how many grams of manganese were present?MW (g/mole): I =126.9; Mn =54.94; Cl = 35.45; K = 39.09; Na = 23; S = 32
Use the data provided for stock concentration and mass to calculate the concentrations of each solution. Solution A) A stock solution of 0.0100 M solution of K3[Fe(CN)6] is provided. Calculate the volume of the stock solution needed to prepare 100.0 ml of .00200 M K3[Fe(CN)6]. Deionized water should be used to dilute the solution. Solution B) Calculate the volume of solution A needed to prepare 50.0 ml of .0010 M K3[Fe(CN)6]. Deionized water should be used to dilute this solution.
An ore containing magnetite, Fe3O4, was analyzed by dissolving a 1.5419-g sample in concentrated HCl, giving a mixture of Fe2+ and Fe³+. After adding HNO3 to oxidize any Fe²+ to Fe³+, the resulting solution was diluted with water and the Fe³+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe₂O3. Calculate the %w/w Fe3O4 in the sample.
A 1.1324 g sample of magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe2+ and Fe3+. Nitric acid was added and the solution was boiled for a few minutes, which converted all of the iron to Fe3+. The Fe3+ was then precipitated as Fe2O3*xH2O by addition of NH3. After filtration and washing, the residue was ignited at a high temp to give 0.5394 g of pure Fe2O3. What is the percent Fe and the percent Fe3O4 in the sample?
The minerals chalcocite (Cu2S) and malachite (CU2CO3(OH)2) are two primary sources of copper. What is the oxidation state of copper in each of these minerals .a O The oxidation state of copper in chalcocite is +1, and in malachite it is +1. .b O The oxidation state of copper in chalcocite is +1, and in malachite it is +2. .C The oxidation state of copper in chalcocite is +2, and in malachite it is +1 .d O The oxidation state of copper in chalcocite is +2, and in malachite it is +2.
6. Most minerals can be considered to be salts of weak acids and strong bases. Identify the weak-acid and strong-base components in each of the following minerals: a. Olivine [Mg2SiO4] b. K-feldspar [KAISI3Og] c. Diopside (CaMgSi,O) d. Kaolinite [Al₂Si₂O5(OH)4] olling

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