An acidic solute, HA, has a Ka of 1.00 X 10-5 and a partition coefficient, Kp, between water and hexane of 5.00. Calculate the extraction efficiency if we extract a 50.00 mL sample of a 0.025 M aqueous solution of HA, buffered to a pH of 8.00, with 100.00 mL of hexane.
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- (b) Suppose the laboratory Technician carried out the same titration experiment in which he/she recorded an average volume of 20 cm³ of the dilute hydrochloric acid (HC) by titrating with 0.05 mol dm³ and 25 cm³ of potassium hydroxide (KOH). Calculate the concentration of hydrochloric acid from the Technician's experiment.Calculate the ionic strength (u) of a solution containing silver chromate Ag2CrO4 in 0.100 M sodium nitrate NaNo3. The thermodynamic solubility product of Ag2CrO4 is 1.2 x 10-12.In carbonate mixtures, Vpth > ½Vpcg for an NaOH, Na2CO; mixture. Try to explain why the relationship inverts and Vpth < ½Vbcg for an Na;CO3, NaHCO3 mixture.
- grammarly-G X * Content oard.odu.edu/ultra/courses/_393452_1/cl/outline F2 Question Completion Status: X GA student wan X 1 QUESTION 3 A student wants to determine the solubility of water and copper (1) bromide (a green solid) in ethyl acetate (a colorless organic liquid). She places 1 mL of ethyl acetate into each of two test tubes. To one, she adds 5 drops of water to it. To the other, she adds a small scoop of copper(1) bromide. 8.0 F3 2 - Which test tube represents the ethyl acetate and A. Test tube 1 copper(1) bromide if the copper(1) bromide is insoluble in ethyl B. Test tube 2 acetate? C. Test tube 3 D. Test tube 4 - Which test tube represents the mixture of the ethyl acetate and water if the water is insoluble in ethyl acetate? $ Question Com X C Chegg Search x 3 Which test tube represents the mixture of the ethyl acetate and water if the water is soluble in ethyl acetate? - Which test tube represents the ethyl acetate and copper(1) bromide if the copper(1) bromide is soluble…In an experiment to determine the concentration of H2SO4 in a brand of toilet cleanser, 10.0 cm3 of the cleanser was first diluted to 250.0 cm3 with distilled water. 25.0 cm3 of the diluted cleanser were titrated with 0.320 mol dm–3 NaOH solution, using methyl orange as indicator.If 29.2 cm3 of NaOH solution is used, what is the concentration of H2SO4 in the undiluted toilet cleanser?a. 2.30 mol dm–3b. 4.60 mol dm–3 c. 9.20 mol dm–3 d. 11.50 mol dm–3Use the expression of the activity coefficient to calculate the coefficient of activity of cobalt in the equilibrium solubility of Co (OH) 2 (Ksp = 1.3 x 10-15) in the presence of a solution containing 0.0333M NaCl. ions α: αCo 2+ = 0.45nm, αOH- = 0.30nm, -log γx = 0.51 zx2 √µ 1 + 3.3 αx√µ Select one:to. 0.51b. 0.91c. 0.75d. 0.83
- 3.) The following Beer's Law calibration plot was collected at 391.9 nm using the five mixtures listed above. The trendline equation was y = 4617.1x. A saturated solution of lead(II) chromate had an absorbance of 0.0025. Calculate its solubility, in molarity. Molar Solubility of PbCrO4: x 107 M ABSORBANCE VS CHROMATE CONCENTRATION AT 391.9 NM 1.40 1.20 y = 4617.1x R-0.9972 1.00 0.80 0.60 0.40 0.20 0.00 C 0.00005 0.0001 0.00015 0.0002 0.00025 0.0003 Chromate concentration (mol.L)Q3/ Calculate the solubility of barium carbonate BaSO4 in a solution containing MgSO4 0.04M taking into consideration the activities. Compare the result if the effectiveness is not taken into consideration, KSP BaSO4 = 1.08 x 10 -10Q: 1: The distribution constant for iodine between an organic solvent and HO is 85. Find the concentration of I, remaining in the aqueous layer after extraction of 50.0mL of 1.00 X 103 M I2 with the following quantities of the organic solvent: (a) 50.0 mL; (b) two 25.0 mL portions; (c) five 10.0 mL portions.
- Calculate the values expected for the total alkalinity and for the phenol- phthalein alkalinity of a 25°C saturated solution of calcium carbonate in water, and compare them to the values for a solution that also is in equilib- rium with atmospheric carbon dioxide. Use the concentrations quoted in the last column of Table 10-4.Calculate solubility in the presence of a common ion. Calculate the solubility of PbCrO4 (a) in pure water and (b) in a solution in which [CrO42-] = 0.298 M. Solubility in pure water = 2- Solubility in 0.298 M CrO4²- = ΣΣThe KSp of PbBr2 is 4.6 x 10-6. WWhat would be the solubility of this compound in a solution that was already 0.074M in KBr? mhen done