Recall:

$\overline{){\mathbf{Molarity}}{\mathbf{\left(}}{\mathbf{M}}{\mathbf{\right)}}{\mathbf{=}}\frac{\mathbf{moles}\mathbf{}\mathbf{solute}\mathbf{}\mathbf{\left(}\mathbf{mol}\mathbf{\right)}}{\mathbf{liter}\mathbf{}\mathbf{solution}\mathbf{}\mathbf{\left(}\mathbf{L}\mathbf{\right)}}}$

**Total volume of the solution = 50.0 mL + 25.0 mL = 75.0 mL**

The concentration of each of the ions in solution is:

Suppose 50.0 mL of 0.250 M CoCl_{2} solution is added to 25.0 mL of 0.350 M NiCl_{2} solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive.

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