Part 2. A solution of 6.00g of substance B in 100.0mL of aqueous solution is in equilibrium, at room temperature,wl a solution of B in diethyl ether (ethoxyethane) containing 25.0 g of B in 50.0 mL9) what is the distribution coefficient of substance Bb) what isthe mass of B extracted by shaking 200 ml of an aqueous solution containing10g of B with call at room temp):i) 100 mL ofdiethyl etherii) 50ml of diethyl ether twiceiii) 25ml of diethyl ether four times

Answered: Image /qna-images/answer/eb28913b-3cdd-42bf-b9e0-51cec959fc52.jpg

Answered: Part 2. A solution of 6.00g of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3.A sample is known to contain NaOH, Na2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCl ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample? ww ww
A 0.3172 g sample containing only KCl (MM: 74.55)and NaBr (MM: 102.89) is dissolved in 50 mL water and titrated with 0.1120 M AgNO3, requiring 36.14 mL to reach the endpoint. What is the % NaBr in the sample?Note: Send to me your solution for perfect points with proper name and label. a. 17.40% b. None of the given choices c. 78.39% d. 15.22% e. 82.41%
(3). Write short notes on displacement titration with suitable example.
simple steps Find the % of sodium carbonate in a sample if 5.002 g of the sample required 29.10 cm³ of 0.7344 mol dm-³ HCl for complete neutralisation. Make sure to solve the problem using the balanced equation. Solution (a) Determine moles of HC1 (titrant, known) (b) Use a balanced equation relate moles of analyte to moles of titrant (reaction ratio) (c) Determine mass of analyte (determine unknown) and % in sample
Provide full complete solution do not round off numbers and show proper labelling and cancellations
Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. This step was repeated using 0.400, 0.300, 0.200, 0.100 mLs of the standard solution Questions: A.) determine the concentration of the acetylsalicylic acid in the 100.00 mL volumetric flask containing the solution from which the standards were made. B.)determine the concentration of the acetylsalicylic acid in each of the 10.00 mL calibration solutions. I only need the work for 0.400 mLs C.)Make a scatter plot (on the computer again) of absorbance versus concentration for the calibration samples. On the plot, add a linear trendline, and display the equation and the R2 value on the chart. Take your time to label the axes
Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. Number of moles of NaOH = 0.005 moles Since the reaction between acetylsalicylic acid and NaOH is a 1:1 reaction, the number of moles of acetylsalicylic acid used in the reaction is also 0.005 moles. the concentration from analysis question 5: acetylsalicylic acid in the 100.00 mL volumetric flask is 0.050 M. From your plot, what is the value of εb? From the Beer- Lambert law For the aspirin sample, calculate the concentration of acetylsalicylic acid present using the value of εb that you found The concentration from analysis question 5 represents the concentration in the 10.00 mL sample that was prepared in the volumetric flask using an aliquot of the solution in the…
H.W 1) Calculate the number of meq. of H2C204.2H2O (fw= 126.1) in 0.5 gm of the pure compound assuming that two hydrogen ions to titrated with standard base?
3. Analysis of a mixture consisting of NaOH + Na2CO3 + inert matter gives the following data: 10.00 g. Its aqueous solution is diluted to 250.0 mL and two separate 25.00 mL sample portions are titrated. With one portion, an end point with phenolphthalein is obtained in cold solution, with 44.52 mL of 0.5000 N HCI. The other portion requires 46.53 mL of the acid for an end point with methyl orange. Calculate the percentage composition of the original sample.
A mixture was known to contain three of the four compounds in the table. After the mixture of the three solids was extracted with hot water and filtered, Compound A was obtained by evaporating the filtrate to dryness. When 3M HCl was added to the solid residue, a clear solution resulted. After adding excess 3M NaOH solution to the acid solution, a precipitate was formed. After filtration, the insoluble solid was found to be Compound B. Compound C was recovered by evaporation of the filtrate. None of the compounds (A, B, or C) was soluble in all of the solvents; water, 3M HCl, and 3M NaOH. Identify Compounds A, B, and C. Justify your answer.
2. a 10.00ml diluted chloride sample required 13.89 ml of 0.02014 M AgNo3 to reach the fajans endpoint. a. how many moles of Cl- ion were present in the sample b. what was the concentration of chloride in the diluted solution?
ghing out an accurate amount of solid sodium hydroxide and dissolving it in a known volume of water? 5. If magnesium hydroxide were used instead of NaOH, how many moles would it take to combine with three moles of KHP? Explain. 6. A 0.4622-g sample of potassium hydrogen phthalate was dissolved in 50 mL of deionized water and titrated to a phenolphthalein end-point with 19.48 mL of NaOH solution. What is the molarity of the NaOH? o 7. Assuming that the density of vinegar is 1.012 g/mL, calculate the weight percent of acetic acid in vinegar if 23.85 mL of 0.1311 M NaOH was required to titrate 5.00 mL of vinegar. noit reaction and dissociat rs bios olisos to dne hsq 2sm oq etb s sbubni A.2nileblu lnbotsrds nidslw .29ituoibidnembeqxins bns 2 e lo asS o (E. 4) uph nolto n 92 rt onithsie sted qid ierud srdt i asiddud tis svome of ballst ine dno 6 2 slddud his edd cnolienird douon t Vsi sbbeakc ut asw ql erd brs oldoloe HOs bluoW ed dnslom HO O oisiqxB 1ipid ood 1o wo 9U2MGE 6.AB breb 1UOY .S…

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