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- What is the concentration of ions in the soil solution after fertilizer application? Suppose that 122 pounds of K+ were applied per acre, then a gentle rain soaked the top 10 inches of soil to field capacity, which for the given soil was about 16% water by volume. If the K+ was applied as KCl, it is plausible that it all dissolved and distributed relatively uniformly with the infiltrating water. If so, then what was the K+ concentration in the soil solution in mol K+/L solution? Note that the volume can be computed like we do for an acre-furrow-slice (AFS), as area times depth. This is going to be a relatively small number, so please report your answer in mol K+/L solution to at least 5 decimal places.One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?If 500mL of 0.10M Ca2+ is mixed with 500mL of 0.10M SO42-, what mass of calcium sulfate will precipitate? Ksp for CaSO4 is 2.40 • 10-5. express answer to 3 significant figures. And include units.
- 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.One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?Ksp for AgCl is 1.77E-10. What is the molar solubility of AgCl in a solution of 0.36 M NaCl?Include at least 3 significant figures in your answer.
- TOPIC: GRAVIMETRY SHOW THE SOLUTION The mercury in a 0.7152-g sample was precipitated with an excess of paraperiodic acid, H5IO6, according to the following reactions:5 Hg+2 + 2 H5IO6 ---> Hg5(IO6)2(s) + 10 H+The precipitate was filtered, washed free of precipitating agent, dried and found to weigh 0.3408-g. Calculate the percentage of Hg2Cl2 in the sample. Molar Masses: Hg5(IO6)2 = 1448.75 Hg2Cl2 = 472.09 Answer: 38.82% Hg2Cl2 An iron ore was analyzed by dissolving a 1.1324-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron (III) was precipitated as the hydrous oxide Fe2O3·xH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe2O3. Calculate (a) % Fe, and (b) % Fe3O4 in the sampleMolar Masses: Fe2O3 = 159.69 Fe = 55.847 Fe3O4 = 231.54 Answer: 33.32% Fe and 46.04% Fe3O4MnSO4•H2O is soluble in water at 25°C, with a solubility of 70.0 g per 1000 g of solution. A saturated solution of MnSO4•H2O has a density of 1.02 g mL-1. When MnSO4•H2O dissolves in water, it absorbs roughly 3.05 kJ/mol of energy. MnSO4•H2O = 169.03 g/mol; H2O = 18.02 g/mol; MW: MnSO4•H2O = 169.03 g/mol. Which of the following is TRUE about a 0.32 M solution of MnSO4•H2O in water? a. A 0.32 M solution contains 70.0 g MnSO4•H2O b. A 0.32 M solution of MnSO4•H2O is unsaturated c. A 0.32 M solution of MnSO4•H2O is supersaturated d. A 0.32 M solution of MnSO4•H2O is saturatedMnSO4•H2O is soluble in water at 25°C, with a solubility of 70.0 g per 1000 g of solution. A saturated solution of MnSO4•H2O has a density of 1.02 g mL-1. When MnSO4•H2O dissolves in water, it absorbs roughly 3.05 kJ/mol of energy. MnSO4•H2O = 169.03 g/mol; H2O = 18.02 g/mol; MW: MnSO4•H2O = 169.03 g/mol. What is the mole fraction of MnSO4•H2O in its saturated solution?
- Solid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.The Ksp of Fe3(PO4)2 is 5.51⋅10-21 M. Calculate the solubility of Fe2+ and PO43- in a saturated solution.The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?