Many anions are quite stable in the aqueous phase, but not so much in organic solvents where its necessary to perform some reaction (usually nucleophilic substitutions). I have heard that crown ethers are good phase transfer catalysts that bring ions to the organic phase. 18-crown-6 is used to coordinate to $\ce{K+}$ ions and bring them to organic phases.

enter image description here

While the cation can enter the organic phase, how does the anion enter it then? Does the anion simply "tag along" with the crown ether complex? The anion gains no solvation stability in organic phase, so the anion moving from aqueous to organic phase seems unlikely.

So my question is: How does the phase transfer catalyst ensure migration of anions to the organic phase?

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    $\begingroup$ I suspect the anion just tags along, forming a tight ion pair. In a sense, the anion does not need to be solvated by the solvent because it is largely "solvated" by the cation. Also, solutions do not necessarily need to be electroneutral, so in principle the organic layer could have a net positive charge from an excess of potassium ions, while the aqueous layer would have a net negative charge from an excess of anions, but this charge imbalance must be very small, otherwise an immense voltage difference would build up between the layers. $\endgroup$ – Nicolau Saker Neto May 17 '17 at 12:55
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    $\begingroup$ In addition, instead of the couple of crown ether + inorganic salt, you may use a couple of organic cation and inorganic anion to get your anion into the organic phase. Albeit not available as anhydrous salt, tetrabutylammonium fluoride (TBAF), used for desilylation in solvents like THF, comes to my mind as one example. $\endgroup$ – Buttonwood May 17 '17 at 14:02
  • $\begingroup$ @Buttonwood while that's true, that doesn't seem to imply how inorganic anions enter organic phases. $\endgroup$ – Pritt says Reinstate Monica May 17 '17 at 14:46
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    $\begingroup$ There's always some solvation and almost always some solubility. $\endgroup$ – Mithoron May 17 '17 at 21:33
  • $\begingroup$ @Mithoron Pretty sure that slight solvation isn't greater that what water provides. $\endgroup$ – Pritt says Reinstate Monica May 18 '17 at 1:33

Actually, anions are not unstable in organic phases per se. There is no intrinsic physical property of organic phases that would make anions inherently unstable: the main problem is that most heteroatoms in organic solvents are more electronegative than carbon and therefore carry a slightly negative charge which attracts cations more easily than anions.

Most organic phases are best classified as ionophobe, however. They will not like cations or anions in their vicinity. Remember that organic phases are typically mainly hydrocarbons with the odd heteroatom, so they have a low polarisablility. Water, on the other hand, is a highly polarised dipole and able to stabilise both cations and anions easily with the appropriate side of the water molecule.

Now if we add a phase transfer catalyst to a biphasic mixture of water and an organic solvent — typical examples would be $\ce{Bu4N+ I-}$ or crown ethers — then these will readily transfer themselves into the organic phase. In the case of crown ethers, it is because they are basically already like the organic solvent: a hydrocarbon with a few heteroatoms. Crown ethers can, however, piggyback a coordinated cation at practically no extra cost: the cation is directly solvated by the crown ether’s oxygens. In the case of the tetrabutylammonium cation, the charge of the tetravalent nitrogen is somewhat shielded by the four butyl residues which interact much better with other organic residues than with water.

This means that we have a general positive charge in the organic phase due to the crown-ether solvated cations or tetrabutylammonium cations present in there. This in turn draws anions towards the cationic charge due to electrostatic interactions.

We can now also look at some basic principles explaining London interactions: generally, the more disperse the orbitals of a species are, the easier this species can be polarised and thus the better London interactions can be. Cations are species in which there is an overall deficiency of electrons so orbitals are drawn closer to the nuclei. Anions, on the other hand, have a surplus of electrons, meaning that these will repel each other more and orbitals will be more diffuse. Compare neutral atom radii to ionic radii to confirm this. The more diffuse anions will therefore have an easier time forming London interactions with the hydrocarbon solvent than the less diffuse cations.

Thus, in summary, one typically needs the ion pair to cross the phase boundary. An anion might transfer by itself but the cation needs help; thankfully, cations can be transferred easily with crown ethers or tetrabutylammonium compounds because these are more able to interact well with the solvent.

  • $\begingroup$ I still don't understand how the anion moves into the organic phase though. It's not coordinated by a crown ether, then what's making it to abandon it's cozy aqueous phase to enter the organic one? $\endgroup$ – Pritt says Reinstate Monica Aug 19 '17 at 4:51
  • $\begingroup$ Because the organic phase has a positive charge and it is not that uncozy. $\endgroup$ – Jan Aug 19 '17 at 4:59
  • $\begingroup$ Is it like a "I would leave my 10 close friends to follow my girlfriend into a party I didn't want to go" kind of way? That the anion prefers to stay with the cation as opposed to being solvated in the aqueous phase? $\endgroup$ – Pritt says Reinstate Monica Aug 19 '17 at 6:18
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    $\begingroup$ @PrittBalagopal You’re comparison is invalid, it’s rather leaving one or two friends to follow your girlfriend to another somewhat chill party. And it doesn’t really work on a 1:1 level imho; rather, the cations are so attracted to the organic phase that there is a charge imbalance that somewhat draws the anions. $\endgroup$ – Jan Aug 19 '17 at 7:24
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    $\begingroup$ So maybe it’s more like ‘Wow, there are tons of single girls at that party, let’s go there, the music’s not all too bad.’ $\endgroup$ – Jan Aug 19 '17 at 7:24

The generally accepted mechanism by which phase transfer catalysts bring about the migration of anions is slightly different from that described by Jan. Phase transfer catalysts essentially help to solve the heterogeneity problem:

That is, if we have a mixture of a reactant that is only soluble in the organic phase and another reactant that is only water-soluble, how do we facilitate a reaction between the two?

Traditionally, this problem is solved with the use of a mutual solvent. We can possibly use a solvent in which both reactants have appreciable solubility in. This mutual solvent would then be the phase in which the reaction takes place in. An example of such a solvent is ethanol, which has both a hydrophilic hydroxyl group and a lipophilic ethyl group.

Phase transfer catalysis (PTC) offers another solution to this heterogeneity problem. Starks (1970) provides a good example to allow us to understand its working principle.

Consider a nucleophilic displacement reaction between 1-bromooctane and aqueous sodium cyanide. With a stirred heterogeneous mixture of the two reactants in separate phases, the only reaction is hydrolysis of $\ce {NaCN}$ to sodium formate after $\ce {2}$ weeks at $\ce {100}$ $^{\circ}$$\ce {C}$.

The use of a phase transfer catalyst helps to facilitate this nucleophilic displacement reaction. Reaction is brought about by the use of small quantities of an agent which transfers one reactant across the interface into the other phase so that reaction can proceed. The phase-transfer agent is not consumed but performs the transport function repeatedly. Thus, in the cyanide displacement on 1-bromooctane, a phase transfer catalyst may either transport the alkyl bromide into the aqueous phase for reaction, or transport cyanide ion into the organic phase. Organic-soluble quaternary ammonium or phosphonium cations, $\ce {Q+}$, were found to be excellent agents for the transport of anions from aqueous phase to an organic phase. Catalysis of the cyanide displacement on 1-bromooctane by quaternary salt is represented in eq 1. In this way a little organic soluble quaternary salt dramatically increases the displacement reaction rate.

enter image description here

The above image illustrates the general mechanism by which PTCs work. It primarily involves anion exchange and ion-pair migration.


Starks, C. M. Phase-transfer catalysis. I. Heterogeneous reactions involving anion transfer by quaternary ammonium and phosphonium salts. J. Am. Chem. Soc. 1971, 93, 195–199.


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