A solution of HClO4 is adjusted with 0.4125 g of primary standard purity HgO (216.6 g / mol) in a KBr solution. The reaction between HgO and KBr is as follows. HgO (s) + 4 Br- + H2O → HgBr42- + 2 OH- What is the molarity of HClO4 if 46.51 mL of acid is used to neutralize the OH-? What is the pH of the buffer obtained by mixing 50.0 mL 0.200 M NaH2PO4 with 50.0 mL 0.120 M HCl?

A solid mixture containing MgSO4 is dissolved in water and treated with an excess of Ba(NO3)2, resulting in the precipitation of 0.6 g of BaSO4.The molecular weight of BaSO4 is 233 g/mol. Number of moles of MgSO4 in the mixture is? O 0.00257mol O 0.52700 mol O 0.05720 mol O 0.25700 mol O 0.02570 mol

1. An impure sample of compound A is contaminated with two impurities B and C. The sample is to be purified by recrystallization using ethanol as the solvent. The solubility properties of the three components are summarized below. Solubility in Solubility in ethanol Solubility in 50 mL Solubility in 50 mL ethanol at -78 °C at - 0°C ethanol at -78 °C ethanol at - 0°C (g) (g) Compound A 0.12 g/mL 0.02 g/mL Impurity B 0.58 g/mL 0.04 g/mL Impurity C 0.005 g/mL 0.0003 g/mL The impure (7.5 g) sample contains 5.0 g of compound A, 1.5 g of B and 1.0 g of C and is recrystallized using 50 mL of ethanol. The sample is boiled with 50 mL of ethanol, filtered by gravity and then cooled in ice and filtered by suction. a) How much compound A should be obtained as the final product? Will the sample be contaminated with any of the impurities? Explain (using calculations to support your answer-fill in the missing masses in the table above). Hint: For this question you should calculate the mass of each…

The decomposition of N,0, can be described by the equation 2 N,0,(soln) → 4NO, (soln) + O,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. 1 (s) [N,O3] (M) 2.576 215 2.250 456 1.934 755 1.602 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0 s to 215 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 215 s to 456 s? average rate of reaction: M/s What is the average rate of reaction for the time interval from 456 s to 755 s? average rate of reaction: M/s

A saturated liquid feed of 500 mol/hr containing 40 mole % water is to be fractionated at 101.325kPa (abs) in order to form a distillate containing 70 mole % water and a bottoms product of 10 mole % water. NOTE: This is actually NOT an ideal solution, e.g. Raoult’s Law does NOT apply.Equilibrium data is available on Blackboard. Assume a distillate reflux ratio (if necessary) of 3:1. a)  Calculate the flowrates (mol/hr) of the distillate and bottoms. b)  Determine the theoretical number of trays and the feed tray number for the specified operation. c)  Determine the minimum reflux ratio, RMIN and the minimum number of theoretical trays at total reflux. d)  Compare the results of (a-c) to the ideal system considered in the previous assignment.

Table Q4 shows the solubility of liquid trichlorohexane in toluene (also liquid) at equilibrium at different temperatures, where species 1 is trichlorohexane and species 2 is toluene. These data are obtained at 1 atm. X1 0.037 0.050 0.085 0.135 0.199 0.288 0.364 0.482 0.500 0.585 Table Q4 Temperature (°C) 92.18 100.00 107.11 111.96 113.84 112.87 109.63 101.91 100.00 90.05 (a) Plot a properly labeled T-x₁ diagram of this binary mixture at 1 atm. (b) Estimate the composition of each phase at 110°C for this binary mixture. (c) At 110°C and 1 atm, trichlorohexane is added dropwise into an initially pure toluene until the mole fraction of trichlorohexane reaches 0.5. Assuming equilibrium is preserved during every addition of trichlorohexane, describe what you would see if the whole process is conducted in a transparent beaker. (d) At 100°C, determine the A12 and A21 in the two-constant Margules equation. Justify any assumptions that you make.

(a) Consider the following chemical reaction: 3FE203(s) + CO(g) → 2Fe304(s) + CO2(g) AH° = ? Use the following thermochemical data to determine the enthalpy change of this reaction. (6) 2FE2O3 (s) AH° = -1652 kJ 4Fe(s) + 302(g) C(s,graphite) + ½O2(g) → CO(g) 3Fe(s) + 202 (g) → CO2(g) AH° = -110.5 kJ Fe304(s) C(s,graphite) + O2(g) AH° = -1117 kJ AH° = +395.5 kJ (b) What is the standard enthalpy of formation of carbon dioxide? (2)

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Alumina from bauxite separation stage calculations A crucial step in the production of aluminum from bauxite ore is the separation of alumina from the remaining mineral impurities in the ore. In the Bayer process this is accomplished by treating bauxite with aqueous NaOH to produce NaAIO2 (alumina). NaOH(aq) + Al(OH)3(s) → NaAIO2(aq) + 2H2O(1) Since NaAIO2 is water soluble while the residual mineral constituents of bauxite are not, a separation can be achieved by allowing the minerals to settle out and decanting the aqueous solution of NAAIO2 and unreacted NaOH. In order to further recover any NAAIO2 entrained in the settled mineral solids, this "mud" is repeatedly washed with water and allowed to settle, and the wash water is decanted. The figure below shows one stage of this washing-settling process. Wash water Slurry - Open to air Mixer/Wash tank Setling tank Decanted solution System boundary Washed mud In this stage, a feed slurry consisting of 10 wt% solids, 11 wt% NaOH, 16 wt%…

A solution containing sodium fluoride is mixed with a solution containing cadmium nitrate to form a solution that is 0.0050 M in NaF and O.00250 M in Cd(NO3)2. If the Ksp for CDF2 is 6.44x10-3, then Q > K and a precipitate of CDF2 will form. O Q < K and more CDF2 will precipitate since the solution is not supersaturated. O Q < K and CdF2 does not precipitate. Q = K and the system is at equilibrium.