# Acid catalysed mechanism of the addition of alcohols to alkenes

I believe that this mechanism is false. The protonated ether would in my opinion give a proton to methanol rather than $\ce{H2SO4}$ because the protonated $\ce{CH3OH}$ is more stable than $\ce{H2SO4}$. Can someone confirm my thought?

• pKa of H2SO4 is -9 pKa of CH3OH2+ is -2.5 – yolo123 Aug 16 '14 at 1:50
• Dissenter's analysis is pretty much on target. The one thing I'd add, you are correct that the proton is probably given to back to methanol rather than bisulfate because there is probably a drop of acid and a lot of methanol. But thermodynamics will win out and eventually the proton will be transferred from protonated methanol to the bisulfate anion to regenerate the acid which, as Dissenter noted, is a catalyst - not to be consumed. – ron Aug 16 '14 at 2:11
• Protonating HSO4- in the presence of methanol is thermodynamically favorable? – Dissenter Aug 16 '14 at 2:16
• Ron, which thermodynamic property are you stating? From my current perception of things, I think the protonated methanol would NOT transfer the proton to make H2SO4. – yolo123 Aug 16 '14 at 2:17
• It is important to realize, that $\ce{H2SO4}$ is not the catalytically active species. It is also important to know that sulfuric acid always comes with water. The catalytic species is therefore either $\ce{H3+O}$ or $\ce{H2+OMe}$ as these are present in equilibrium. The scheme is only a sequence of reaction steps, it is no reaction mechanism as it completely lacks transition sates. (It is also omitted that the product has to be reprocessed in aqueous solution.) – Martin - マーチン Aug 16 '14 at 5:09

The protonated ether would in my opinion give a proton to methanol rather than H2SO4

I don't think sulfuric acid is gaining any protons here. You mean hydrogen sulfate ion, correct?

Can someone confirm my thought?

The mechanism is acid-catalyzed dehydration, so the acid must be regenerated. Catalysts are by definition not consumed over the course of a reaction. Now, whether the acid is actually sulfuric acid is debatable, and in my mind, unlikely, given the leveling effect and that the solvent is methanol.

The leveling effect states that the strongest acid that can exist in high concentration in a particular solvent is the conjugate acid of the solvent. The conjugate acid of methanol has a pKa of ~ -2.5, while the pKa of sulfuric acid is ~ -9. Thus, sulfuric acid can't exist in high concentration in methanol. Sulfuric acid would immediately protonate the strongest base in the system. Therefore, it appears to me that the acting acid is not sulfuric acid. Perhaps it is protonated methanol ion.

Or perhaps it is the case that sulfuric acid reacts directly with the alkene. Whether sulfuric acid would be regenerated in this particular solvent, however, is questionable at best, given sulfuric acid's extreme thermodynamic instability in methanol. If it were regenerated, then the sulfuric acid would again protonate the strongest base in the system.

Of course, thermodynamic considerations are important, but so are kinetic considerations. Do remember that there is likely a lot more solvent than there is sulfuric acid and substrate (the alkene). So it seems most likely that the acting acid is protonated methanol - it is a lot more likely for sulfuric acid to bump into a methanol molecule rather than an alkene molecule.

• Sorry for the mistake. Yes, I meant HSO4- – yolo123 Aug 16 '14 at 1:50
• Can you explain why the hydrogen sulfate ion would attack instead of methanol? – yolo123 Aug 16 '14 at 1:52
• imgur.com/fn2yxyU Solomon's, not Wade's. – yolo123 Aug 16 '14 at 1:56
• The three lines just means "equivalent" in chemistry. The triple lines are not indicating a hydride shift; it is just indicating that the two pentagons are the same (one is just purposely distorted as to make clear the hydride shift; the other has been adjusted to look pretty when printed). – Dissenter Aug 16 '14 at 2:20
• @yolo123 When it comes to reaction mechanisms you have to understand, that these are only the most likely steps that are going to happen. Also the depiction of most reaction mechanisms is only a reaction sequence. A mechanism has always to include the transition states. At the same time, there are many reactions happening simultaneously, and there are also quite many equilibria involved. A mechanism is never as simple as it is depicted in most organic chemistry textbooks. It is only a guideline to reactivity of certain species. – Martin - マーチン Aug 16 '14 at 5:20

The short version: You are correct, the schematic drawing is not the correct mechanism and it does also not provide the most likely path. For a training exercise it is close enough though. It shows the most important steps and it conserves stoichiometry.

The depicted scheme does not show a reaction mechanism in the sense of the definition given in the goldbook. A reaction mechanism always also has to include transition states, that lead to the respective products. It is rather a reaction sequence, that shows the most important steps. In this sense, the stoichiometry has to be conserved and in this sense it is as correct as it could be.

Noteworthy is, that the catalytically active species is not sulfuric acid, but instead a mixture of hydronium and protonated methanol, $\ce{H3+O/H2+OCH3}$. Sulfuric acid is such a strong acid, that it is capable of protonating any solvent that has a lone pair, even itself via autoprotolysis (in concentrated $98\%$ solution). $$\ce{2H2SO4 <=> [H3SO4]+ + [HSO4]- <=> H3+O + [HS2O7]- <=> H2O + H2S2O7}$$ The use of concentrated sulfuric in organic synthesis is usually not advisable, since its dehydration property can quickly decompose many organic compounds that contain hydroxyl groups. The use of diluted sulfuric acid (either in water or alcohols) is therefore much more common.

It is only logical, that sulfuric acid will protonate methanol, which can be considered a preceding equilibrium. $$\ce{H2SO4 + HOCH3 <=> H2+OCH3 + [HSO4]- }$$ Since methanol is also the solvent and the acid is only available in catalytic amounts, it is feasible to assume, that the equilibrium lies entirely on the right.

It is also important, that the last step must be also in equilibrium, since it is only the protonation/deprotonation of an ether. Here again we have much more methanol than product, so that the equilibrium will most likely be entirely on the product side.

A more descriptive mechanism would be the following:

For simplicity and sufficiently accurate bond formation and breaking is indicated by arrows, omitting the transition states. Resulting a slightly simplified picture. However, the preceding equilibrium - as you noted - should not be omitted. This formulation of the mechanism is particularly important for many simple organic reactions, as it focusses entirely on the reactants and products (and to a minor extent on the reactive intermediates).

When it comes to more complex reactions, e.g. with asymmetric catalysts it is often much better to include the transition states.

From this it can also be seen, that the choice of sulfuric acid is somewhat arbitrary, as most acids would do the same. However, sulfuric acid is often used, since bisulfate and sulfate are very weak nucleophiles.

• @Dissenter, even assuming the reagents were classified as anhydrous, the autoprotolysis and related self-ionization equilibria (which Martin described) of sulfuric acid would result in a hodgepodge of species. Greenwood & Earnshaw note the following species present in pure sulfuric acid (in order of decreasing abundance, with $\ce{H2SO4}$ itself being the solvent): $\ce{HSO4^{-}, H3SO4^{+}, H3O^{+}, HS2O7^{-}, H2S2O7, H2O}$. Of course, when added in catalytic quantities, they won't be the dominant species. – Greg E. Aug 19 '14 at 23:30