Liquid-liquid extraction: Wikis


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Concepts in
Chemical Equilibria
Acid dissociation constant
Binding constant
Buffer solution
Chemical equilibrium
Chemical stability
Complex dissociation constant
Dissociation constant
Distribution coefficient
Distribution ratio
Equilibrium constant
Equilibrium unfolding
Equilibrium stage
Liquid-liquid extraction
Phase diagram
Predominance diagram
Phase rule
Reaction quotient
Relative volatility
Solubility equilibrium

Molar solubility

Stability constant
Stability constants of complexes
Thermodynamic equilibrium
Theoretical plate
Vapor-liquid equilibrium

Liquid-liquid extraction, also known as solvent extraction and partitioning, is a method to separate compounds based on their relative solubilities in two different immiscible liquids, usually water and an organic solvent. It is an extraction of a substance from one liquid phase into another liquid phase. Liquid-liquid extraction is a basic technique in chemical laboratories, where it is performed using a separatory funnel. This type of process is commonly performed after a chemical reaction as part of the work-up.

In other words, this is the separation of a substance from a mixture by preferentially dissolving that substance in a suitable solvent. By this process a soluble compound is usually separated from an insoluble compound. Solvent extraction is used in nuclear reprocessing, ore processing, the production of fine organic compounds, the processing of perfumes and other industries.

Liquid-liquid extraction is possible in non-aqueous systems: in a system consisting of a molten metal in contact with molten salt, metals can be extracted from one phase to the other. This is related to a mercury electrode where a metal can be reduced, the metal will often then dissolve in the mercury to form an amalgam which modifies its electrochemistry greatly. For example it is possible for sodium cations to be reduced at a mercury cathode to form sodium amalgam, while at an inert electrode (such as platinum) the sodium cations are not reduced. Instead water is reduced to hydrogen. A detergent or fine solid can be used to stabilize an emulsion, or third phase.


Measures of effectiveness

Distribution ratio

In solvent extraction, a distribution ratio is often quoted as a measure of how well-extracted a species is. The distribution ratio (D) is equal to the concentration of a solute in the organic phase divided by its concentration in the aqueous phase. Depending on the system, the distribution ratio can be a function of temperature, the concentration of chemical species in the system, and a large number of other parameters.

Note that D is related to the ΔG of the extraction process.

Sometimes the distribution ratio is referred to as the partition coefficient, which is often expressed as the logarithm. See partition coefficient for more details. Note that a distribution ratio for uranium and neptunium between two inorganic solids (zirconolite and perovskite) has been reported.[1] In solvent extraction, two immiscible liquids are shaken together. The more polar solutes dissolve preferentially in the more polar solvent, and the less polar solutes in the less polar solvent. In this experiment the nonpolar halogens preferentially dissolve in the nonpolar mineral oil.

Separation factors

The separation factor is one distribution ratio divided by another, it is a measure of the ability of the system to separate two solutes. For instance, if the distribution ratio for nickel (DNi) is 10 and the distribution ratio for silver (DAg) is 100, then the silver/nickel separation factor (SFAg/Ni) is equal to DAg/DNi = SFAg/Ni = 10.

Decontamination factor

This is used to express the ability of a process to remove a contaminant from a product. For instance, if a process is fed with a mixture of 1:9 cadmium to indium, and the product is a 1:99 mixture of cadmium and indium then the decontamination factor (for the removal of cadmium) of the process is 0.1 / 0.01 = 10.

Slopes of graphs

The easy way to work out the extraction mechanism is to draw graphs and measure the slopes. If for an extraction system the D value is proportional to the square of the concentration of a reagent (Z) then the slope of the graph of log10(D) against log10([[Z]]) will be two.


Batchwise single stage extractions

This is commonly used on the small scale in chemical labs. It is normal to use a separating funnel. For instance, if a chemist was to extract anisole from a mixture of water and 5% acetic acid using ether, then the anisole will enter the organic phase. The two phases would then be separated.

The acetic acid can then be scrubbed (removed) from the organic phase by shaking the organic extract with sodium bicarbonate. The acetic acid reacts with the sodium bicarbonate to form sodium acetate, carbon dioxide, and water.

Multistage countercurrent continuous processes

Coflore Continuous Counter Current Extractor

These are commonly used in industry for the processing of metals such as the lanthanides, because the separation factors between the lanthanides are so small many extraction stages are needed. In the multistage processes, the aqueous raffinate from one extraction unit is fed to the next unit as the aqueous feed, while the organic phase is moved in the opposite direction. Hence in this way even if the separation between two metals in each stage is small, the overall system can have a higher decontamination factor.

Multistage countercurrent arrays have been used for the separation of lanthanides. For the design of a good process the distribution ratio should be not too high (>100) or too low (<0.1) in the extraction portion of the process. It is often the case that the process will have a section for scrubbing unwanted metals from the organic phase, and finally a stripping section to obtain the metal back from the organic phase.

Extraction without chemical change

Some solutes such as noble gases can be extracted from one phase to another without the need for a chemical reaction (See Absorption (chemistry)). This is the simplest type of solvent extraction. When a solvent is extracted, two immiscible liquids are shaken together. The more polar solutes dissolve preferentially in the more polar solvent, and the less polar solutes in the less polar solvent. Some solutes which do not at first sight appear to undergo a reaction during the extraction process do not have distribution ratio which is independent of concentration. A classic example is the extraction of carboxylic acids (HA) into non polar media such as benzene. Here it is often the case that the carboxylic acid will form a dimer in the organic layer so the distribution ratio will change as a function of the acid concentration (measured in either phase).

For this case the extraction constant k is described by k = [[HAorganic]]2/[[HA aqueous]]

Solvation mechanism

Using solvent extraction it is possible to extract uranium, plutonium, or thorium from acid solutions. One solvent used for this purpose is the organophosphate tri-n-butyl phosphate. The PUREX process is commonly used in nuclear reprocessing uses a mixture of tri-n-butyl phosphate and an inert hydrocarbon (kerosene), the uranium(VI) are extracted from strong nitric acid and are back-extracted (stripped) using weak nitric acid. An organic soluble uranium complex [UO2(TBP)2(NO3)2] is formed, then the organic layer bearing the uranium is brought into contact with a dilute nitric acid solution the equilibrium is shifted away from the organic soluble uranium complex and towards the free TBP and uranyl nitrate in dilute nitric acid. The plutonium(IV) forms a similar complex to the uranium(VI) but it is possible to strip the plutonium in more than one way, a reducing agent can be added which converts the plutonium to the trivalent oxidation state. This oxidation state does not form a stable complex with TBP and nitrate unless the nitrate concentration is very high (circa 10 mol/L nitrate is required in the aqueous phase). Another method is to simply use dilute nitric acid as a stripping agent for the plutonium. This PUREX chemistry is a classic example of a solvation extraction.

Here in this case DU = k TBP2[[NO3]]2

Ion exchange mechanism

Another extraction mechanism is known as the ion exchange mechanism. Here when an ion is transferred from the aqueous phase to the organic phase, another ion is transferred in the other direction to maintain the charge balance. This additional ion is often a hydrogen ion, for ion exchange mechanisms the distribution ratio is often a function of pH. An example of an ion exchange extraction would be the extraction of americium by a combination of terpyridine and a carboxylic acid in tert-butyl benzene. In this case

DAm = k terpyridine1carboxylic acid3H+-3

Another example would be the extraction of zinc, cadmium or lead by a dialkyl phosphinic acid (R2PO2H) into a non polar diluent such as an alkane. A non-polar diluent favours the formation of uncharged non-polar metal complexes.

Some extraction systems are able to extract metals by both the solvation and ion exchange mechanisms, an example of such a system is the americium (and lanthanide) extraction from nitric acid by a combination of 6,6'-bis-(5,6-dipentyl-1,2,4-triazin-3-yl)-2,2'-bipyridine and 2-bromohexanoic acid in tert-butyl benzene. At both high and low nitric acid concentrations the metal distribution ratio is higher than it is for an intermidate nitric acid concentration.

Ion pair extraction

It is possible by careful choice of counterion to extract a metal. For instance, if the nitrate concentration is high it is possible to extract americium as an anionic nitrate complex if the mixture contains a lipophilic quaternary ammonium salt.

An example which is more likely to be encountered by the 'average' chemist is the use of a phase transfer catalyst. These are charged species which transfer another ion to the organic phase. The ion reacts and then forms another ion which is then transferred back to the aqueous phase.

For instance, the 31.1 kJ mol-1 is required to transfer an acetate anion into nitrobenzene,[1] while the energy required to transfer a chloride anion from an aqueous phase to nitrobenzene is 43.8 kJ mol-1.[2] Hence if the aqueous phase in a reaction is a solution of sodium acetate while the organic phase is a nitrobenzene solution of benzyl chloride, then when a phase transfer catalyst the acetate anions can be transferred from the aqueous layer where they react with the benzyl chloride to form benzyl acetate and a chloride anion. The chloride anion is then transferred to the aqueous phase. The transfer energies of the anions contribute to the given out by the reaction.

A 43.8 to 31.1 kJ mol-1 = 12.7 kJ mol-1 of additional energy is given out by the reaction when compared with energy if the reaction had been done in nitrobenzene using one equivalent weight of a tetraalkylammonium acetate.

Aqueous two phase extraction

Using an Aqueous two phase system, it is possible to generate two immiscible water phases. This can then be used to extract proteins, which would denature if exposed to organic solvents.

Kinetics of extraction

It is important to investigate the rate at which the solute is transferred between the two phases, in some cases by an alteration of the contact time it is possible to alter the selectivity of the extraction. For instance, the extraction of palladium or nickel can be very slow because the rate of ligand exchange at these metal centres is much lower than the rates for iron or silver complexes.

Aqueous complexing agents

If a complexing agent is present in the aqueous phase then it can lower the distribution ratio. For instance, in the case of iodine being distributed between water and an inert organic solvent such as carbon tetrachloride then the presence of iodide in the aqueous phase can alter the extraction chemistry.

Instead of D_{\mathrm{I}^{+2}} being a constant it becomes D_{\mathrm{I}^{+2}} = k[[I2.Organic]]/[I2.Aqueous] [[I-.Aqueous]]

This is because the iodine reacts with the iodide to form I3-. The I3- anion is an example of a polyhalide anion which is quite common.

Industrial process design

Typically an industrial process will use an extraction step in which solutes are transferred from the aqueous phase to the organic phase, this is often followed by a scrubbing stage in which unwanted solutes are removed from the organic phase, then a stripping stage in which the wanted solutes are removed from the organic phase. The organic phase may then be treated to make it ready for use again.

After use the organic phase may be subjected to a cleaning step to remove any degradation products, for instance in PUREX plants, the used organic phase is washed with sodium carbonate solution to remove any dibutyl hydrogen phosphate or butyl dihydrogen phosphate which might be present.


Two layers separating during a liquid-liquid extraction.

An organic MTBE solution is extracted with aqueous sodium bicarbonate solution. This base removes benzoic acid as benzoate but leaves non-acidic benzil (yellow) behind in the upper organic phase.

While solvent extraction is often done on a small scale by synthetic lab chemists using a separatory funnel, it is normally done on the industrial scale using machines which bring the two liquid phases into contact with each other. Such machines include centrifugal contactors, Thin Layer Extraction#Thin layer extractors,spray columns, pulsed columns and mixer-settlers.

Extraction of metals

The extraction methods for a range of metals include:[3]

  • Cobalt - The extraction of cobalt from hydrochloric acid using alamine 336 in meta-xylene.[4] Cobalt can be extracted also using Cyanex 272 {bis-(2,4,4-trimethylpentyl) phosphinic acid}.
  • Copper - Copper can be extracted using hydroxyoximes as extractants, a recent paper describes an extractant which has a good selectivity for copper over cobalt and nickel.[5]
  • Neodymium - This rare earth is extracted by di(2-ethyl-hexyl)phosphoric acid into hexane by an ion exchange mechanism.[6]
  • Nickel - Nickel can be extracted using di(2-ethyl-hexyl)phosphoric acid and tributyl phosphate in a hydrocarbon diluent (Shellsol).[7]
  • Palladium and platinum - Dialkyl sulfides, tributyl phosphate and alkyl amines have been used for extracting these metals.[8][9]
  • Zinc and cadmium - The zinc and cadmium are both extracted by an ion exchange process, the N,N,N′,N′-tetrakis(2-pyridylmethyl)ethylenediamine (TPEN) acts as a masking agent for the zinc and an extractant for the cadmium.[10] In the modified Zincex process, zinc is separated from most divalent ions by solvent extraction. D2EHPA (Di (2) ethyl hexyl phosphoric acid) is used for this. A zinc ion replaces the proton from two D2EHPA molecules. To strip the zinc from the D2EHPA, sulfuric acid is used, at a concentration of above 170g/l (typically 240-265g/l).

See also


  1. ^ Scholz, F.; S. Komorsky-Lovric, M. Lovric (February 2000). "A new access to Gibbs energies of transfer of ions across liquid". Electrochemistry Communications (Elsevier) 2 (2): 112–118. doi:10.1016/S1388-2481(99)00156-3.  
  2. ^ Danil de Namor, A.F.; T. Hill (1983). Journal of the Chemical Society, Faraday Transactions: 2713.  
  3. ^ Mackenzie, Murdoch. "The Solvent Extraction of Some Major Metals". Cognis GmbH. Retrieved 2008-11-18.  
  4. ^ M. Filiz, N.A. Sayar and A.A. Sayar, Hydrometallurgy, 2006, 81, 167-173.
  5. ^ Yoshinari Baba, Minako Iwakuma and Hideto Nagami, Ind. Eng. Chem. Res, 2002, 41, 5835-5841.
  6. ^ J. M. Sánchez, M. Hidalgo, M. Valiente and V. Salvadó, Solvent Extraction and Ion Exchange, 1999, 17, 455-474.
  7. ^ Lee W. John. "A Potential Nickel / Cobalt Recovery Process". BioMetallurgical Pty Ltd.  
  8. ^ "Precious Metals Refining By Solvent Extraction". Halwachs Edelmetallchemie und Verfahrenstechnik. Retrieved 2008-11-18.  
  9. ^ P. Giridhar, K.A. Venkatesan, T.G. Srinivasan and P.R. Vasudeva Rao, Hydrometallurgy, 2006, 81, 30-39.
  10. ^ K. Takeshita, K. Watanabe, Y. Nakano, M. Watanabe (2003). "Solvent extraction separation of Cd(II) and Zn(II) with the organophosphorus extractant D2EHPA and the aqueous nitrogen-donor ligand TPEN". Hydrometallurgy 70: 63–71.  

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