Assume you are running a forensic laboratory. Using the table of Rf values below, determine which solvent you would use to analyze a sample seized by the police in a drug smuggling case. Justify your solvent choice. Rf Values of Drugs in Various Solvent Systems Drug Solvent 1 Solvent 2 Solvent 3 Morphine 0.20 0.15 0.10 Cocaine 0.45 0.76 0.73 Reserpine 0.75 0.80 0.72

Assume you are running a forensic laboratory. Using the table of Rf values below, determine which solvent you would use to analyze a sample seized by the police in a drug smuggling case. Justify your solvent choice. Rf Values of Drugs in Various Solvent Systems Drug Solvent 1 Solvent 2 Solvent 3 Morphine 0.20 0.15 0.10 Cocaine 0.45 0.76 0.73 Reserpine 0.75 0.80 0.72

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter29: Mass Spectrometry

Section: Chapter Questions

Problem 29.12QAP

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Assume you are running a forensic laboratory. Use the table of Rf values below to determine the answer to the following question. Rf Values of Drugs in Various Solvent Systems Drug Solvent 1 Solvent 2 Solvent 3 Morphine 0.10 0.08 0.10 Quinine 0.07 0.26 0.19 Codeine 0.16 0.53 0.38 Cocaine 0.65 0.90 0.73 Strychnine 0.28 0.76 0.53 Aconitine 0.35 0.90 0.68 Reserpine 0.75 0.80 0.72 A sample seized by the police in a drug smuggling case and suspected to contain Morphine, Cocaine and Aconitine. Which solvent (1, 2 or 3) should be used as the developing solvent? Justify your answer.
1) How does IR radiation affect absorbing molecules? Name an example molecule that does not absorb IR and briefly explain why. 2) Suppose you are able to figure out, correctly, all of the functional groups for an unknown organic molecule using FTIR. Explain why this might not be sufficient to pin down the exact structure of the molecule. What additional information could be useful? 3) Explain the basic operating principle of an ATR based sampling system? Give the advantages of an ATR-based sampling system compared to one based on direct transmittance of IR radiation in terms of sample thickness and preparation techniques?
For TLC analysis, another student calculates the following Rf values for her samples: 1.45=aspirin; 1.25=Ibuprofen; 1.35=acetaminophen; 1.15=naproxen; 1.05=caffeine. 1.40=over-the-counter drug (unknown) Are these values reasonable? Why or why not? Explain what the student may have done incorrectly.
The Rf values for several dyes in an ink are listed below. Which dye has the greatest affinity for the stationary phase? Dye #1: Rf = 0.263 Dye #2: Rf = 0.551 Dye #3: Rf = 0.737 Dye #4: Rf = 0.882
A C¬D (carbon–deuterium) bond is electronically much like a C¬H bond, and it has a similar stiffness, measured by the spring constant, k. The deuterium atom has twice the mass (m) of a hydrogen atom, however. A chemist dissolves a sample in deuterochloroform (CDCl3) and then decides to take the IR spectrum and simply evaporates most of the CDCl3. What functional group will appear to be present in this IR spectrum as a result of theCDCl3 impurity?
It's important to mark the solvent front with a pencil after the plate is finished being developed in order to calculate an Rf. Group of answer choices True False
explain why sp2 chemistry was far easier than sp3 when inputting molecules into early synthetic libraries?
The manager of an organic chemistry stockroom prepared unknowns for a ‘Ketone and Aldehyde’ experiment by placing two drops of the liquid unknowns in test tubes labelled A and B. He then stored the test tubes for several days until they were needed. On the day of the experiment, the students complained the IR spectrum measured for test tube A is different from the spectrum shown by the stockroom manager at the end of the class (refer the picture below). Obviously something has happen to the solution while being left for a few days. a) Identify the functional group revealed by the IR spectrum of i)The stockroom manager ii)The students b)Explain the reason of discrepancy between the stockroom manager’s spectrum and the student’s results. c) Suggest how this misunderstanding might be prevented.1710 cm-1 1725 cm-1
Consider a sample that is a mixture composed of biphenyl, benzoic acid, and benzyl alcohol. The sample is spotted on a TLC plate and developed in a CH2C12-cyclohexane solvent mixture. Predict the relative Rf values for the three components in the sample. Would biphenyl be closest to the blotted line, then benzyl alcohol, then benzoic acid because these others are increasing in polarity to the non-polar solvent? Thanks!
When testing the absorbance of paracetamol with a uv spectrophotometer the following are the abosorbance levels with the concentration associated, what would this mean in terms of the aim of determining the amount of the analgesic paracetamol in commercial tablets using ultraviolet spectroscopy? Concentration (mg/L) Absorbance 0.75 0.032 1.5 0.075 2.25 0.125 4.5 0.181
1. a compound has an Rf value of 0.97 diethyl ether but an Rf value of 0.045 in cyclohexane. Suggest a couple (at least three) solvent (solvents), or solvent system (systems), that might be better suited for this particular compound. 2. suppose your TLC plate shows only one spot at an Rf value of 0.015 (essentially it does not move). Does this mean that your sample is 100% pure? Explain your answer. 3. suppose your TLC plate shows only one spot at an Rf value of 0.98 (essentially with the solvent front). Does this mean that your sample is 100% pure? Explain your answer.
From your results, which component had the highest Rf value and which had the lowest? Based on your answer from the previous question, what could be the reason behind some components having an Rf value higher than the others? Compare the qualities of the two components that rendered the highest and lowest Rf After performing the simulation, what do you think are the possible practical applications of chromatographic techniques that are relevant to your program NURSING?