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Give a lab cation separation scheme for Al3+, Ca2+, Ni2+ cations based on Ksp values and complex ion formations (if any).
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- Calculate the molar solubility of calcium oxalate in a solution that has been buffered so that its pH is constant and equal to 4.00. Data: Kps of CaC2O4 = 1.7x10 -9 ; Ka1 of H2C2O4 = 5.60x10-2 and Ka2 = 5.42x10-5 . Use systematic treatment.Calculate the conditional formation constant (K'' NiY) of the [NiY]2- complex in 0.050 M NH3 and 0.090 M NH4Cl buffer solution. The formation constants of nickel amine complexes are respectively K1 = 102.75, K2 = 102.20, K3 = 101.69, K4 = 101.15, K5 = 100.71, K6 = 10-0.01. (KNiY = 4.2x1018, KNH3 = 1.74x10-5)A pink solid has the formula CoCl3 5NH3 H2O. A solution of this salt is also pink and rapidly precipitates 3mol AgCl(s) on titration with silver nitrate solution. When the pink solid is heated, it loses 1mol H2O to give a purple solid with the same mole ratio of NH3:Cl:Co as the pink solid. The purple solid releases two of its chloride ions rapidly; then on dissolution and titration with AgNO3, release one of its chloride ions slowly. Deduce the structures, draw and name 2 octhahedral complexes
- Write equilibrium expressions, mass balance and charge balance equations for a system that is a mixture of ZnS and NH3. The relevant equilibria are the dissolution and ionization of ZnS, acid dissociation equilibria for NH3 and H₂S and the complexation of Zn²+ and NH3 according to the below reactions: Zn²+ + NH3 Zn²+ + 2 NH3 Zn²+ + 3 NH3 Zn²+ + 4 NH3 Make a plot of the solubility of ZnS as a function of the Zn(NH3)²+ Zn(NH3)2²+ Zn(NH3)3²+ Zn(NH3)4²+ [Bonus analytical concentration of NH3 with reasonable assumptions;A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508 nm after the addition of 1,10-phenanthroline, pH 4 buffer, and hydroxylamine. Then, a water sample treated similarly exhibited an absorbance of 0.109 au. Which of the following statements is true? (A) The Fe concentration of the water sample is higher than 100 ppm. B) The Fe concentration of the water sample is equal to 100 ppm. It is impossible to estimate the Fe content of the water sample from information presented. D) The Fe concentration of the water sample is lower than 100 ppm.Calculate the conditional formation constant of the complex [CuY]*, KNry, in a buffer containing 0.050 M NH3 and 0.090 M NH,Cl given that the %3D successive formation constants of the copper amines are: K1 = 1.9 x 10, K2 = 3.6 x 10°, K3 = 7.9 x 10- and Ka = 1,5 x 102. Cu2' (aq) + NH3(aq) [Cu(NH,)) |Cu(NH3)) + NH3(aq) = [Cu(NH; )2) K2 (aq) 21 |Cu(NH,)2) + NH3(4) [Cu(NH,)s + NH,(a4) [Cu(NH, )3 nc) K3 [Cu(NH,)4) K, (aq) 21 3 (aq) (aq)
- 10-mL aliquots of an environmental water sample were pipetted into five 50.00-mL volumetric flasks. Exactly 0.00, 5.00, 10.00, 15.00, and 20.00-mL of a standard solution containing 11.1 ppm Fe3+ were added to each, followed by an excess of thiocyanate ion to give the red complex Fe(SCN)2+. After dilution to volume, the instrumental response for each of the five solutions measured with a colorimeter was found to be 0.240, 0.437, 0.621, 0.809, 1.809, respectively. Using Excel and the LINEST function, what was the concentration in the water sample (including error)? [HINT: consider the type of calibration scheme used.]A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 12.9 mL of a 0.481 M stock solution was diluted with solvent to make 100.0 mL of the first calibration standard solution and, secondly, 86.6 mL of that first calibration solution was diluted to 100 mL to make the second calibration standard. What is the molar concentration of the second calibration standard solution? Report your answer to 3 significant figures.Determining Ksp of Lead(II) lodide Postlab 1. Which method of plotting data from this experiment allows the best extrapolation to obtain Ksp? Explain why this is so. X X EE= Normal BIIIU 田=T由三三 2. Explain the difference between "ion product" and Ksp. What conditions are necessary for the ion product to approach the value of Ksp? Saved Normal BIIU 田三T 的 l1 1.
- The standard curve was made by spectrophotographic analysis of equilibrated iron(III) thiocyanate solutions of known concentration. You are asked to analyze a Fe(SCN)2+Fe(SCN)2+ solution with an unknown concentration and an absorbance value of 0.4150.415 . The slope-intercept form of the equation of the line is ?=4558.4?+0.0147y=4558.4x+0.0147 . The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe3+Fe3+ concentration of the unknown solution?Aluminium (III) reacts with the Chelating agent HL to give a complex AlL3 that is readily soluble in CHCl3. A spectrophotometric study shows that when a 1.77 x10-4 M aqueous solution of aluminium was extracted with CHCl3 containing 0.01M HL, the analytical concentration of aluminium at pH 4.5 in the two phases were 1.5 x 10-4 M [Al3+]upper) and 2.73 x10-5 M ([AlL3]lower) . What is the distribution coefficient at pH 4.8.Calculate the pH of a buffer solution containing 10.0 cm3 of 0.100 mol dm–3 NaOH and 20.0 cm3 of 0.500 mol dm–3 ethanoic (acetic) acid made up to a total of 50.0 cm3 in a volumetric flask at 298 K. The pKa of ethanoic acid at 298 K is 4.77