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- The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.What is the dominant iron species in water samples ? What environmental factors may have contributed. why is it necesseyy to to investigate Fe3+ concentration and total Fe concentration dpeedtaely ? Why do we need to do the sample to determine total Fe concentration ? And how did then determine Fe2+ concentration?You want to separate Cd2* and Fe2+ (initial concentration 103 mol/L) by means ofprecipitation of the corresponding sulphides. Is therea pH range in which one of the two metals is precipitated quantitatively(concentration in the solution less than or equal to 10" mol/L) is precipitatedwhile the other is still completely_in solution?Calculate and name this pH range where pH values below 0are set equal to O. Illustrate the situation graphically by drawing
- Silica (SiO2) is an impurity that must be removed from ametal oxide or sulfide ore when the ore is being reduced toelemental metal. To do this, lime (CaO) is added. It reactswith the silica to form a slag of calcium silicate (CaSiO3),which can be separated and removed from the ore.(a) Write the balanced equation for this process.(b) Can this be considered a Lewis acid–base reaction? Ifso, what is the Lewis acid and what is the Lewis base?Surface water in an open area of the Indian Ocean adjacent to Kenja has an alkalinity 2320 micromoles/liter and a total carbonate concentration of 2.03 x 10^-3 moles/liter. Calculate the concentrations of HCO3- and CO32-, and also the pH of this sea water.Given this series of equilibrium reactions. See Image(a) Which way should the reaction to “tend” at high pH? Why?(b) Which way should the reaction to “tend” at low pH? Why? (c) What Fe(III) species would be least soluble?
- The pH of a 0.2 M solution of CuSO4 is 4.0. Write chemical equations to explain why a solution of this salt is neither basic [from the reaction of SO42-(aq) with water] nor neutral, but acidic.Write balanced net ionic eqautions for (include phase subscripts): Ag+ and 0.5M Na2SO4 Ba2+ and 0.5M Na2SO4 Ba2+ and 0.5M Na2S2O3 Cu2+ and 0.2M NaI Pb2+ and 0.2M NaI Cu2+ and 0.2M NH3 Cu2+ and 6M NH3 Fe3+ and 6M NH3Write the equilibrium expressions, charge balance equation, and the mass balance equations for 0.100 M aqueous HO2CCO2H and show that the number of equations you list is equal to the number of unknowns in the solutions. Hint: Do not forget the auto protolysis of water.
- Calculate the molar concentration of OH- in a 0.724 M solutionof hypobromite ion (BrO-; Kb = 4.0 x 10-6). What isthe pH of this solution?Calculate the pH of an aqueous solution prepared by dissolving 5.61 g of KOH pellets in water and diluting to a final volume of 0.500 L. (At. wts: K = 39.10, O = 16.00, H = 1.008)Calculate the molar concentration of OH- in a 0.724 M solution of hypobromite ion 1BrO-; Kb = 4.0 * 10-62. What is the pH of this solution?