Experimental Study on Reactive Extraction of Malonic Acid with Validation by Fourier Transform Infrared Spectroscopy

Abstract

Malonic acid is an essential carboxylic acid that is used as a backbone reactant in deriving multiple higher-order carboxylic compounds. The successful attempt of producing malonic acid from a biological route has attracted the scientific community to extract malonic acid from a fermentation broth or dilute aqueous stream. Experimental study on the recovery of malonic acid by reactive extraction was performed, and the effects of TBP concentration, diluents (alkane, ketone, and alcohol), and malonic acid concentration were investigated. The equilibrium models (relative basicity and mass action law models) and the number of theoretical units (NTU) were also evaluated. Fourier transform infrared spectroscopy provided evidence for the formation of significant bonds among extractant–diluent–acid complexation systems which support the experimental outcomes. The results of extraction equilibrium are discussed regarding dimerization constant (D MA), partition coefficient (P MA), extraction efficiency (E MA%), distribution coefficient (K D(MA)), overall extraction complexation equilibrium (K E(MA)), and loading factor (Z MA). The highest reactive extraction efficiency was 73.5% with 0.5962 mol·kg–1 TBP used in MIBK. The distribution coefficient (K D(MA)) of malonic acid in various diluents exhibited the trend MIBK > octanol > heptane. The comparison between values predicted by the equilibrium model and experimental outcomes shows that the relative basicity models predicted better results than the mass action law for reactive extraction of malonic acid. The NTU was calculated to be 2, which was estimated by the modified Kremser equation for designing a countercurrent reactive extraction column.

Ruthenium Nitrosyl Structure in Solvent Extraction Systems: A Comparison of Tributyl Phosphate, Tetrabutyl Urea, N-Methyl, N-Octyl Ethylhexanamide, and N,N,N′,N′-Tetraoctyl Diglycolamide

“…These initial solutions are contacted with organic phases (TBP, TBU, MOEHA, and TODGA-diluent). The composition of the organic solutions are close to optimized concentrations proposed for an industrial solvent extraction application. ,,, The extractions from 4 M nitric acid represent conditions typical of the extraction cycles of the PUREX process at very simplified conditions. , Organic phases after ruthenium extraction from 4 M nitric acid are analyzed by FTIR and EXAFS spectroscopy. − FTIR is used to determine the vibrations which are attributed to ruthenium extraction. EXAFS spectroscopy is used to analyze and compare the local coordination of ruthenium in the different solvents.…”

The recovery of Gallic acid with Triphenylphosphine Oxide and modelling with Artificial Intelligence

“…The solvent properties like dielectric constant, boiling point, density, molecular weight, Dimroth-Reichardt E T parameter, and dipole moment (μ) have been attempted to correlate with K D [37]. E T parameter gives information about the ionization power of the solvent.…”

“…The loading factors were calculated and written in Table 3. As seen, the higher extractant concentrations were used in the solvents, the less were the loading factor values, which can be expressed by the definition of Z [37]. The loading factor values were calculated to be less than 0.5, showing that there was no overload on the extractant molecule.…”

“…If loading factors are less than 0.5, complexation constant values are calculated as in the below Eq. ( 5) [37,38]: (5) where K E is the experimental complexation constant of 1:1 acid-extractant complex formation, and it is found from the slope when Z 1−Z is plotted versus [HGA] aq [39]. Mass Action Law Model explains the nature and type of the formed complex.…”

Reactive liquid–liquid extraction of bio-based 3-hydroxypropionic acid using a biocompatible organic phase containing a tertiary amine: A model-based approach to elucidate dominant mechanisms

“…Recently, Chemarin et al [35] proposed this mechanism for 3-HP extraction based on FT-IR data obtained using TOA in 1-decanol. Ion-pair formation has been widely studied for several organic acids using different tertiary amines [36][37][38].…”