Calculate the equilibrium concentrations of all species when 10 mL of 0.90M Fe2+ is mixed with 10 mL of 0.10M Fe3+, 10 mL of 0.20M Cr2072-and 10 mL of 0.2M Cr3*all buffered to a pH = 3. 6FE2++ Cr2O72-+ 14H+ „ 6F23++ 2Cr3++ 7H2O K = 1 x1059
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- 1ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.Calculate the equilibrium Ni2+ concentration of a solution that has beenprepared by mixing 50.0 ml of Ni2+ 0.030 mol / L with 50.0 ml of EDTA0.050 mol / L. The mixture was buffered to pH 3.0. Kf= 4.2 x 1018 , alfa4= 2.6x10-11A solution containing Mg2+ was buffered to pH 9.81 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)
- A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 MNa2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer untilthe pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, onwhich the solution will turn red. Calculate for the molarity of the unknown.Calculate the molar solubility of AgSCN (Ksp = 1.1 x 10^-12) in a solution maintained at pH 9.00 and where the concentration of ammonia is 0.1 M. HSCN: pKa = 4.0 [Ag(NH3)2]^+ : Kf1 = 2.04 x 10^3; Kf2 = 8.13 x 10^3A sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930M
- A 110.00 mL solution of 0.00195 M A3B2 is added to a 160.00 mL solution of 0.00155 M C3D4. What is pQsp for A3D2?Calculate the equilibrium concentration of Zn2 + in a solution that was prepared by mixing 75.0 mL of Zn2 + 0.030 mol / L with 75.0 mL of 0.050 mol / L EDTA. The mixture was buffered to pH 4.0. Kf = 3.2 x 1016, α4 = 3.8 x 10-9In the MgO experiment, you made a buffer solution by combining 57 mL of 17 M NH3 with 7.0 grams of NH4Cl (FW = 58.49) and then diluting to give a total volume of 100 mL. Calculate the pH of this buffer solution given the pKb for ammonia is 4.76.
- 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/LUse systematic treatment of equilibrium to calculate the molar solubility of AgIO3 in an aqueous solution with a pH of 2.00. Ignore activity coefficients. Ksp for AgIO3 is 3.17*10-8 and Ka for HIO3 is 0.17.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)