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Write the principle behind the following methods of refining :
(i) Hydraulic washing
(ii) Vapour phase refining
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- The cumulative formation constants for the reaction of Co21 with ammonia are log b1 5 1.99, log b2 5 3.50, log b3 5 4.43, log b4 5 5.07, log b5 5 5.13, and log b6 5 4.39. (a) Write the chemical reaction whose equilibrium constant is b4. (b) Write the reaction whose stepwise formation constant is K4 and find its numerical value.A sample of 0.10 M CH3COOH(aq) of volume 25.0 cm3 is titrated with 0.10 M NaOH(aq). The Ka for CH3COOH is 1.8 x 10-5. (a) What is the pH of 0.10 M CH3COOH(aq)? (b) What is the pH after the addition of 10.0 cm3 of 0.10 MNaOH(aq)? (c) What volume of 0.10 M NaOH(aq) is required to reach halfway to the stoichiometric point? (d) Calculate the pH at that halfway point. (e) What volume of 0.10 M NaOH(aq) is required to reach the stoichiometric point? (f) Calculate the pH at the stoichiometric point.A 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0 mL. After acidification, silver nitrate was added to a 25.00 mL aliquot where the resulting precipitate was filtered, washed and then redissolved in an ammoniacal solution of potassium tetracyanonickelate(II) according to the reaction: Ni(CN), + 2 AgBr) → 2 Ag(CN), + Ni? + 2 Br The liberated nickel ion required 26.73 mL of 0.02089 M EDTA. The bromate ion in a 10.00 mL aliquot was reduced to bromide with As* prior to the addition of silver nitrate. The same procedure was followed and the released nickel ion was titrated with 21.94 mL of the EDTA solution. Calculate the percentage of impurity in the sample. Br (79.904) a. 24.45% b.34.38% c. 41.17% d. 65.62%
- Describe the changes in pH that take place during the titration of: (a) a weak acid with a strong base, (b) a weak base with a strong acid .Write the relevant chemical reaction and mass-balance expression for 0.1 M NaCl.(iv) The Ksp for zinc oxide is 3.5 x 1017. What concentration of zinc sulfate (in mol/L) must be dissolved in water in contact with solid zinc oxide to obtain a solution pH of 5.9?.
- (b) An unknown solution containing 25.00 mL of Ni2+ in dilute HCI is treated with a known excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a few drops of indicator are added. The excess unreacted EDTA back titrated with 0.02299 M Zn²*, which requires 17.00 mL to reach the red end point. What is the molarity of Ni2+ in the unknown solution?a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaO
- As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na*B(C,H,). Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non-negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K,CO, and all ammonium is present as NH,Cl. A 5.045 g soil sample was dissolved to give 0.500 L of solution. A 125.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K* and NH ions completely. B(C,H,), + K* KB(C,H,),(s) Compound Formula mass 358.33 g/mol KB(C,H,), NH,B(C,H,), K, CO, B(C,H ), + NH NH,B(C,H,), (s) 337.27 g/mol 138.21 g/mol The resulting precipitate amounted to 0.247 g. A new 250.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH as NH,. NH,CI 53.492 g/mol The resulting solution was then acidified, and excess sodium…(4) The amount of oxalic acid in a sample of 3+ rhubarb was determined by reacting with Fe as outlined in the following reaction. In a typical analysis, the oxalic acid in 10.62 g of rhubarb was extracted with a suitable solvent. The complete oxidation of the oxalic acid to 3+ CO, required 36.44 mL of 0.013 M Fe*.What is the weight percent of oxalic acid in the sample of rhubarb? 2FE3" (aq) + H2C,O,(aq) + 2H2O(1) → 2Fe?* (aq) + 2C02(g) + 2H;0 (aq)What is the best synthesis and purification method with regards to cobalt(II) sulphate (CoSO4.7H2O)