How is the molarity of a 0.50 * M * KBr solution changed when water is added to double its volume?

We’re asked to** determine how the molarity of a 0.50 M KBr solution changes** when **water is added** to **double its volume.**

Recall that when we are **adding water (or solvent) to a solution**, we are **diluting **the solution.

When dealing with **dilution **we will use the following equation:

$\overline{){{\mathbf{M}}}_{{\mathbf{1}}}{{\mathbf{V}}}_{{\mathbf{1}}}{\mathbf{=}}{{\mathbf{M}}}_{{\mathbf{2}}}{{\mathbf{V}}}_{{\mathbf{2}}}}$

M_{1} = initial concentration

V_{1} = initial volume

M_{2} = final concentration

V_{2} = final volume

**Calculate the ****Molarity of KBr ***when its volume is doubled.*

Dilution