Determining the pH Effect and Partition Coefficient of Diethyl Malonate in Water and Water - Pentane systems using Liquid-Liquid Extraction and Ultraviolet - Visible Spectroscopy. Chris Bilham Amanda Ranero Dr. Rainer Volkamer Dr. Molly Larsen Zachary Finewax Theodore Koenig University of Colorado Department of Chemistry and Biochemistry
This document is posted to help you gain knowledge. Please leave a comment to let me know what you think about it! Share it to your friends and learn new things together.
Transcript
Determining the pH Effect and Partition Coefficient of Diethyl Malonate in Water and Water - Pentane systems using Liquid-Liquid
Extraction and Ultraviolet - Visible Spectroscopy.
Chris BilhamAmanda Ranero
Dr. Rainer VolkamerDr. Molly LarsenZachary FinewaxTheodore Koenig
● All senior chemical engineer undergraduates are required to complete a design project for an assigned client.
● Our client DMC limited has produced an environmentally friendly way to produce DEM using engineered microbes and a sugar feedstock.
● However the majority of DEM produced is done in organic solvents and there was little to none literature on how to separate DEM from an aqueous solution.
● Our design team proposed two continuous separation methods: 1) Liquid-Liquid Extraction (LLE) with distillation using n-pentane. 2) Natural Phase Separation with decanting.
● Both the above methods were missing critical physical parameters in order to develop a successful process model. Mainly, the partition coefficient for our solvent n-pentane and the effect of pH on the solubility of DEM in water.
❖Motivation
Depiction of Separation Process Series Process of Phase Separation followed by LLE and Distillation
.
❖Motivation
Critical for these Units
❖Methodology
Choice of Method of Quantification
• It was determined (by recommendation of Theodore Koenig) that the best method of quantification would be to use Ultraviolet – Visible Spectroscopy (UV-VIS)
• Originally High Performance Liquid Chromatography coupled with UV-VIS spectroscopy and Attenuated Total Reflectance Fourier Transform Infrared Spectroscopy (ATR - FTIR) were considered, but subsequently discarded.
• It was found that DEM shows an absorbance peak at 212 nm, in the Ultraviolet region, using a Cary 5000 UV-VIS spectrometer.
• It was found that n-pentane and water had a cut off absorbance around 190 nm, preventing spectral interference
Figure 1: UV-VIS data from Cary 5000
❖Methodology
Instrumentation
Cary 5000 UV-VIS spectrometer • 1 cm path length quartz cells• 0.5 nm data interval• 1 nm slit width• 200nm – 350 nm scan range
• It was found that lowering the pH did decrease the solubility of DEM in water
• The scale was done as a relative solubility in order to standardize the ‘limit’ of solubility.
• Although the exact mechanism is not clear, we hypothesis that the increase in [H+] ions is acting to make the solution ‘more polar’ driving DEM out of solution.
• This effect would be similar to that of salting out, increasing hydrophobic interactions with DEM.
• Although terms are not known, equation is shown to demonstrate it is a non-linear affect.
% 𝑅𝑆=[𝐷𝐸𝑀 ]𝑝𝐻
[𝐷𝐸𝑀 ]𝑁𝑒𝑢𝑡𝑟𝑎𝑙×100
Figure 2: pH affect on relative solubility of DEM in water
❖Experiment – 2 Results & Analysis
Calibration Curves for DEM in Water and n-Pentane Respectively
Figure 3: Calibration Curve for DEM in water Figure 4: Calibration Curve for DEM in n-pentane
❖Experiment – 2 Results & Analysis
Molar Absorption Coefficient (σ)
Figure 3: Molar Absorption Coefficient Epsilon in inverse (Molarity*cm)
σ= 𝑨𝒄𝒍
Beer- Lambert Laws Solved for Molar Absorption Coefficient
Partition Coefficients Determined from Liquid-Liquid Extractions
Table 4: Partition Coefficients from Aqueous (Heavy Phase)
Table 5: Partition Coefficients from Pentane (Light Phase)
• A two sided t-test on the means concluded these values were statistically
different at the 95% confidence level• A 95% confidence interval for pentane and
water respectively are: 6 ± 6 & 2.6 ± 0.2
𝐾=𝑉 𝑎𝑞
𝑉 𝑜𝑟𝑔𝑞𝑎𝑞−𝑉 𝑎𝑞
𝑉 𝑜𝑟𝑔
𝐾=𝑉 𝑎𝑞
𝑉 𝑜𝑟𝑔( 1𝑞𝑎𝑞
−1)Ratios can ‘blow up’ results
❖Experiment – 2 Results & Analysis
So why did that happen?
• The main contribution is hypothesized to be the evaporation of pentane, causing a variable increase in concentration.
• This is further validated by the fact that pentane samples were not run on the same day as the LLE; K values for samples run the longest time after LLE were the highest.
• It is also hypothesized that a micro emulsion was forming with DEM saturated water. Pentane with the smallest LLE volume would be most susceptible to these effects while the large volume of aqueous phase could be sampled while ignoring this emulsion.
??
❖Experiment – 2 Results & Analysis
pH and Partition Coefficient Analysis
2.645𝐾 𝑝𝐻=
𝐾 [𝐻 ]𝐾 𝑎+[𝐻 ]
• The given equations below are used to describe the theoretical change in K based upon a known K and pH
• This data was graphed to the right as figure 5
• Looking at the pH range for this experiment it is expected that K did not change in our pH range. Our findings match the theoretical.
Figure 5: Theoretical effect of pH on K; pka = 12.9, Ko = 2.645
❖Conclusion
• pH does decrease the solubility of DEM in water, the effect is non-linear and most likely operates in the same manner as ‘salting out’.
• The partition coefficient was found to not be dependent on pH in our experimental range, this matches theoretical predictions.
• The partition coefficient of DEM in water-pentane systems was found at a 95% confidence interval to be 2.6 ± 0.2 from aqueous data and 6 ± 6 in the organic n-pentane phase. These results were found to be statistically different by a two sided t-test
• The pentane data is deemed to be precise but not accurate.
❖Recommendations
• A larger pH range should be investigated (1-14) with replicates to better examine effect of pH on DEM solubility in water.
• Additionally salt concentrations should be done in a similar manner to verify pH effect hypothesis and to further characterize DEM-water solubility
• A higher pH range should be investigated (7 - 14) with replicates to better examine effect of pH the partition coefficient
• Larger separatory funnels should be used, allowing for larger aqueous and pentane volumes to mitigate the effect of emulsion layers
• Pentane samples should be either be run immediately after or stored in a manner that prevents evaporation or can be accurately re-diluted
❖Acknowledgements
Professor Rainer Volkamer
Dr. Molly Larsen
Zachary Finewax Theodore Koenig
University of Colorado Department of Chemistry
and Biochemistry
❖References
Acid-Base Equilibria. (n.d.). Retrieved April 25, 2016, from http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch17/ph.php
Harris, Daniel C. "Fundamentals of Spectrophotometry." Quantitive Chemical Analysis. 8th ed. China Lake: W.H. Freeman, 2010. 505-565. Print.
Larsen, Molly, and Rainer Volkamer. "E6 Analysis of Vanillin in Vanilla Using High Performance Liquid Chromatography." Chem 4171/4181 Instrumental Analysis Laboratory. Fall 2015 ed. 75-79. Print.
Lipscomb, M., Dr. (2016). Client Meetings [Personal interview].
Dr. Matthew Lipscomb, PhD in Chemical Engineering from CU Boulder. Client for DMC limited.
S. J., Dr. (2005, April 11). MALONIC ACID DIESTERS Dimethylmalonate, 108-59-8 Diethylmalonate, 105-53-3. Retrieved March 15, 2016, from http://www.inchem.org/documents/sids/sids/malonates.pdf
Used, extensively throughout the report
Method for Producing Diethyl Malonate. (2013). Retrieved April 25, 2016, from https://xudaphne01.wordpress.com/2013/08/28/method-for-producing-diethyl-malonate/