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Consider the dissolution of A(OH)2 in a medium with [OH-] = 0.15 M.
- Construct an ICE table for the dissolution of A(OH)2 in this medium.
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- Explain the principle of electrostatic precipitation in gas cleaning .2. State the processes that can be adopted to purify and test the purity of sodium benzoateA student determined the concentration of total reducible iodine in the aqueous phase based on the average of their 'best two' determinations in Part 1 to be 0.0185 M. They also determined the concentration of 12 in the CH2Cl2 phase based on the average of their 'best two' determinations in Part 2 to be 0.0200 M. Determine what the concentration of 13 in water would be based on this student's previous work. Report your final answer, in mol/L, to 4 decimal places and only include the numerical value (no units). Do not use scientific notation for this question. Do not give handwriting solution.
- Give some examples of secondary standard solutions, and give the reasonThe distribution constant for iodine between an organic solvent and H2O is 85. Find the concentration of iodine remaining in the aqueous layer after extraction of 50mL of 1.00x10-3 M iodine with two portion of 25mL organic solvent?Write the formula for a micelle of a Cr (OH) 3 sol obtained as a result of the hydrolysis reaction of Cr2 (SO4) 3. The stabilizer is Cr2 (SO4)3 solution Cr2(SO4)3 + 6H2O 2Cr(OH)3 + 3SO2 +3O2 please write the micelle equation
- Describe the effect, if any the following procedural errors would have on the calculated value of the Ksp. Is the dissolution of Ca(IO3)2 in water endothermic or exothermic? Write an equation for the process, including the heat of reaction.Briefly explain the principles involved in the separation of the components of a mixture by solvent extraction.Can precipitation give a confirmatory result on Group V cations: K, Na, and NH4?
- If you were to have a stock solution with a concentration of 1.475 M and performed a serialdilution as shown in Fig. 5.1, what would the concentrations be in flasks A, B, C, and D?When dissolving salt in water, what would be the effect on the dissolution rate if a 1, 0g chunk were dissolved instead of 1.0 g of crushed salt?The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
