# Affects of Adding Water to Cobalt Chloride Equilibrium

1. Feb 15, 2010

### tkahn6

Effects of Adding Water to Cobalt Chloride Equilibrium

1. The problem statement, all variables and given/known data

$$Co(H_{2}O)_{6} ^{2+} (aq) + 4Cl^{-} (aq) \Leftrightarrow CoCl_{4} ^{2-} (aq) + 6H_{2}O (l)$$
$$Pink \Leftrightarrow Blue$$

We're learning about Le Chatelier's Principal.

My question is:

Why does the reaction shift the left when adding $$H_{2}O$$?
2. Relevant equations

3. The attempt at a solution

My first thought was that stress is being added to the right side of the equation and so equilibrium shifts left. This is incorrect because $$H_{2}O$$ is a liquid and therefore is not part of the equilibrium reaction (it has no concentration).

The addition of water does however dilute both sides of the equation. This is the explanation my teacher gave but going back over it, diluting the concentrations of the products and reactants would give you a larger $$K_{c}$$ which would shift it to the right.

Thank you.

Last edited: Feb 15, 2010
2. Feb 16, 2010

### Mapes

At the molecular scale, the individual reactions don't stop just because the reaction is in equilibrium. They continue, but the rate going forward is the same as the rate going in reverse.

In other words, $\mathrm{Co(H_2O)_6^{2+}}$ ions get together and react with four chlorine ions each at the same rate that cobalt chloride ions get together and react with six water molecules.

If you had a lower $\mathrm{Co(H_2O)_6^{2+}}$ concentration, for example, the forward reaction would be less likely to occur because it would be harder to find a $\mathrm{Co(H_2O)_6^{2+}}$ ion to react.

So what happens when water is added?

3. Feb 17, 2010

### epenguin

Re: Effects of Adding Water to Cobalt Chloride Equilibrium

$$Co ^{2+} + 4Cl^{-} \Leftrightarrow CoCl_{4} ^{2-} (l)$$
$$Pink \Leftrightarrow Blue$$