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viridianlocust958Lv1

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5. Assume that the partition coefficient, K, for partitioning of compound Abetweendiethyl ether and water is 3; that is, A preferentially partitions into ether.a. Given 400 mL of an aqueous solution containing 12 g of compound A, howmany grams of A could be removed from the solution by a single extractionwith 200 mL of diethyl ether?b. How many total grams of A can be removed from the aqueous solution withthree successive extractions of 67 mL each?*if given the equation can you please explain how you got it and what the numbers mean in it (if some numbers or standard or the plug in's you took from the question I asked you )-thanks :)

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Bunny GreenfelderLv2

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Related questions

1. Compound Y with a partition coefficient of 0.4 (K) between solvents A and B (as shown in the formula below) is dissolved in 100 mL of A. Which will be more effective for extracting compound Y one extraction using 80 mL of solvent B or two successive extractions using 40 mL of solvent B at the time? Show your calculations.

Partition Coefficient: K={Y}A/{Y}B

2. A mixture containing 1,3,5-trimethoxybenzene (A), phenol (B), aniline (C) and 1- naphthoic acid (D) was dissolved in dichloromethane. Next two extractions were performed first using HCl then with NaOH. Which of the compounds could not be separated in this procedure. Explain and show the pertinent reaction equation/s. (4 pts)

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4. Acetanilide and aniline were dissolved in diethyl ether and extracted with 5% NaOH. Which of the two compounds would you expect to find in the aqueous layer? Explain your answer. (2 pts)

Why did you only titrate the aqueous layer during the experiment? (my experiment about the extraction)

Could you have titrated the organic layer to figure out the distribution coefficients and other data? Why or why not?

Show all work please for points

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i have the right answers just need help with the work

Calculate the pH of a solution made by mixing 1 L each of 0.30 M acetic acid and 0.10 M sodium hydroxide. [pKa of acetic acid = 4.74] Calculate the pH change that occurs when 30 mL of 0.1 M NaOH are added to 200 mL of the solution in (a). Do you expect the pH change in (b) to be equal to the pH change when 30 mL of 0.1 M NaOH are added to 200 mL of 3.5 times 10-5M HC1? EXPLAIN. Calculate the pH change in (c). Is this what you expected? If not, can you find an explanation (i.e., do you think your prediction in (c) is wrong or do you think you "messed up" in your calculation)? Given that quantitative extraction should be at least 99.9%, answer the following: If the partition coefficient for a metal chelate partitioning between water and chloroform is 6.4, will quantitative extraction be achieved if a 25.0 mL solution of 4.3 times 10-2M ML (metal-ligand complex) is shaken with One 20-mL portion of chloroform Two 10-mL portions of chloroform Can you find the number of extractions needed to achieve quantitative extraction from the general formula? Suppose that a solute has a partition coefficient of 8.8 between water and chloroform. What volume of chloroform will be needed for a single extraction if the fraction of solute remaining in 25.0 mL of water is to be the same as the fraction remaining after three successive extractions with 10.0 mL portions of chloroform? How many grams of C^COONa should be added to one liter of 0.100 M HC1 to obtain an acid buffer with pH = 4.4. [You are given that pKa of acetic acid is 4.74] Using examples, explain how masking, de-masking, and pH control are used in EDTA titrations Explain how sulfate ion (as an example of an anion) can be analyzed via EDTA titration Ni2+ can be analyzed by back titration using standard Zn2+ at pH 5.5 with xylenoi orange indicator. A solution containing 25.00 mL of Ni2+ in dilute HC1 is treated with 25.00 mL of 0.05283 M Na2EDTA. The solution is neutralized with NaOH, and the pH is adjusted to 5.5 with acetate buffer. The solution turns yellow when a few drops of indicator are added. Titration with 0.02299 M Zn2+ requires 17.61 mL to reach the red end point. What is the molarity of Ni2+ in the unknown? In nature, hardwater tends to contain appreciable concentrations of Fe3+ and Cu2+. Explain how EDTA titration is used to determine hardness as Ca2+ and Mg2+ in the presence of these other metal ions.

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