According to the IUPAC Goldbook a solution is:
A liquid or solid phase containing more than one substance, when for convenience one (or more) substance, which is called the solvent, is treated differently from the other substances, which are called solutes. When, as is often but not necessarily the case, the sum of the mole fractions of solutes is small compared with unity, the solution is called a dilute solution. A superscript attached to the ∞ symbol for a property of a solution denotes the property in the limit of infinite dilution.
There is no mentioning of that the solute may not react with the solvent. If you investigate a few common solutions, you will also find that it is indeed quite common, that the solvent reacts with the solution. Take for example the dissolution of hydrochloride in water, which is often expressed with the following equation:
$$\ce{HCl (g) + H2O (l) <=> Cl- (aq) + H3O+ (aq)}$$
You can see here, that the proton is transferred onto a water molecule and from one point of view this is a displacement reaction; the chloride is displaced by water.
Another example is the dissolution of acetic acid. It is often described with the following equation:
$$\ce{H3C-COOH (s) + H2O (l) <=> H3C-COO- (aq) + H3O+ (aq)}$$
The same happens here. We hide the fact that the dissolution process includes getting the solvent into a highly flexible network of hydrogen bonds in the addendum of $\ce{(aq)}$.
When you look at common salts that get dissolved, it is often that the metal ion reacts as a weak acid, co-coordinating the solvent molecules. In many cases this is so flexible, like for the alkaline metals, that we cannot describe even the first solvation sphere approximately.
For other salts this is quite possible. Take for example the dissolution of copper sulfate. We often write for short
$$\ce{CuSO4 (s) <=> Cu^2+ (aq) + SO4^2- (aq)}$$
when we actually mean the formation of a complex
$$\ce{CuSO4.5H2O (s) + H2O (l) <=> [Cu(H2O)6]^2+ (aq) + SO4^2- (aq)}.$$
A chemical reaction actually takes place. And since everything is in equilibrium, there are many chemical reactions happening in solutions all the time.
Now the dissolution of bromine in water is no different. In fact the disproportionation
$$\ce{Br2 (l) + 2 H2O <=> BrOH (aq) + Br- (aq) + H3O+ (aq)}$$
is quite necessary to dissolve bromine in the first place. While I do not even slightly agree to the causality of having a dipole means being a polar molecule, I can still see, that the bromine molecule is less polar than water. It is however quite well polarizable; it has a quadrupole moment.[1] This is what also leads to the above equation.
The bromine hydrolysis has been investigated a couple of times.
$$\begin{align}
\ce{Br2 + H2O &<=>[K_1] HBrO + H+ + Br- }&
K_1 &= \ce{\frac{[HBrO][H+][Br- ]}{[Br2]}}
\end{align}$$
The temperature dependency of $K_1$ has been studied by Liebhafsky as early as 1934.[2] In their studies they also considered the effects of the tribromide equilibrium
$$\begin{align}
\ce{Br3^- &<=>[K_3] Br- + Br2}
K_3 &= \ce{\frac{[Br- ][Br2]}{[Br3^- ]}}.
\end{align}$$
And later continue to state that the existence of the pentabromide ion is highly probable.
$$\begin{align}
\ce{Br5^- &<=>[K_5] Br- + 2 Br2}
K_5 &= \ce{\frac{[Br- ][Br2]^2}{[Br5^- ]}}
\end{align}$$
From the equilibrium constants you can see, that the main dissolved species is still $\ce{Br2}$.
$$\begin{array}{lrrrrr}
T/~\mathrm{^\circ C} & 0 & 10 & 25 & 30 & 35 \\\hline
K_1\times10^{-9} & 0.70 & 1.78 & 5.8 & 8.3 & 11.3\\
\end{array}$$
Conclusion
Solutions do not exist without chemical reactions. There are often multiple different species in solution, that have very low concentration, so for various purposes a valid approximation is to neglect those species' concentrations.
- Jacek Bieroń, Pekka Pyykkö, Dage Sundholm, Vladimir Kellö, and Andrzej J. Sadlej; Phys. Rev. A 2001, 64, 052507.
- Herman A. Liebhafsky; J. Am. Chem. Soc. 1934, 56 (7), 1500–1505.
