Determine the correlation factor k value for 56% ethyl acetate (EA) in ethyl propionate (EP) (volume/volume%). Given the area ratio obtained by GC analysis, AEA/AEP- 1.19 for the standard mixture of 56% EA in EP, what is the value of k? Use the equations shown below. You do need to show all your calculations. AEA/AEP = NEA/NEP * C NEA/NEP = AEA/AEP*1/C = AEA/AEP*k

Determine the correlation factor k value for 56% ethyl acetate (EA) in ethyl propionate (EP) (volume/volume%). Given the area ratio obtained by GC analysis, AEA/AEP- 1.19 for the standard mixture of 56% EA in EP, what is the value of k? Use the equations shown below. You do need to show all your calculations. AEA/AEP = NEA/NEP * C NEA/NEP = AEA/AEP1/C = AEA/AEPk

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...

See similar textbooks

Similar questions

Hexanoic acid was added to an immiscible biphasic solvent system, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D2) of hexanoic acid in water with respect to CCl4.
If an instrument gives a response of 1240 for a standard containing 8 ppm of a substance, how much if this substance is in a sample that gives a response of 1705? Are any assumptions needed?
Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.
Following titration analysis, a sample of a fruit juice was found to contain 8.9 mg cm-3 ascorbic acid. Given that the Mr value for ascorbic acid is 176.1 Da, calculate the value of the ascorbic acid concentration expressed in units of mmols dm-3 then enter it
A chemist is asked to separate the components of a mixture composed of 1.00 g each of the two compounds shown below. The chemist has access to the following bases: 10% aqueous NaHCO3 and 10% aqueous NaOH. Which base and how many mLs of the base (i.e., the minimum amount) are needed to completely separate these compounds from each other by liquid-liquid extraction?
The separation and purification processes given below and the method used against them are given. Which or which of these pairings are correct? Brewing the tea - Extraction Purification of water from impurities-Chromatography Separating olive pomace from oil while olive oil is being produced - Decantation Obtaining oil fractions - Ordinary distillation Obtaining essential oils and using them in perfume making - Water-steam distillation A. I, IV, V B. I, II, III, IV, V C. I, II, V D. I, II, III, V E. I, II, III, IV
Sheet 5 From the following data determine the following: Define outlier and then identify the outlier in the data. Determine if the outlier should be kept of discarded from the data. Trial 1 2 3 4 HCl (mL) 22.3 28.4 29.8 29.3 NaOH (mL) 35.2 35.1 34.9 35.0
25 ml of pickled brine was taken from an apple pickled with vinegar and diluted to 500 ml, 25 ml of this was taken and acidity was determined with 0.2 N (Factor: 1.05) NaOH. In the main trials, 6.3 ml - 6.5 ml - 6.9 ml, respectively, 0.1 ml base was used in the analysis without using the sample.For example, how many ppm is its acidity?
Calculate the mass percent of the ascorbic acid in the same show full solution Situation: The pounded Vitamin C tablet was half into two below are the calculated data in the experiment. Each of the half are transfered in a 250ml erlen meyer flask and added 75ml of deionized water for the vitamin C to dissolve. Then it was prepared for titration where the burette was filled with 0.09794M standardize NaOH solution then a total of with 3 drops 2% phenolphthalein indicator was added to each erlen meyer flask l, swrill it and begin the titration. below are the following data gathered: Vitamins used: Nature Made vitamin C 500mg tablet Trial 1 Mass: 0.3108g of Vitamin C tablet Initial volume: 1.6mL Final volume: 15.4mL Trial 2 Mass: 0.3349g Initial volume: 15.4 mL Final volume: 30.2 mL
(Concentration) You are tasked to prepare 300.000 ppb of a sodium carbonate standard for a titrimetric analysis. If you need to prepare 1000.00 (±0.06) mL of this solution, how much (in grams) solid, pure Na2CO3 are you supposed to dissolve? What absolute uncertainty is associated with your mass measurement if the prepared solution has a 0.1% percent relative uncertainty? Write your answer using the appropriate number of digits. Note that the formula mass of Na2CO3 is 105.9888 g/mol with negligible error. Assume that instrument precision is not a limitation in your lab. g (absolute error) How many significant figures does your reported mass have? (number of sig. figs.)
A 15.00 g sample containing mixed alkali and other inert components was dissolved and diluted to 300 mL with water. A 20 mL aliquot was titrated with 5.02 mL of 0.5352 M HCl to reach PHP endpoint. Another 20 mL aliquot was titrated to the BCG endpoint, using up 18.87 mL of titrant in the process. Note: Answer in two decimal places only. If there is no answer, type in 0.00. Use the molar masses 105.989 ?/??l ??2cO3 and 84.007 g/mol NaHCO3 indicated. The volume of titrant needed to neutralize NaOH is _________ mL.The volume of titrant needed to neutralize Na2CO3 is _____________ mL.The volume of titrant needed to neutralize NaHCO3 is _____________ mL. The mass of NaOH is ___________ g.The mass of Na2CO3 is __________ g.The mass of NaHCO3 is __________ g. The percent weight of NaOH is __________ %.The percent weight of Na2CO3 is __________ %.The percent weight of NaHCO3 is __________ %.
For a 22.16 mg sample of MgC2O4•H2O (Mwt = 130.35 g/mol) shows two steps:a loss of 3.06 mg from 100–250 oC and a loss of 12.24 mg from 350–550oC. For each step, identify the volatilization product and the solidresidue that remains. In second step, two volatile products are formed.(Mwt C = 12 g/mol; O = 16 g/mol; H = 1 g/mol)