chemistry/math solution stoichiometry

A 9.3 gram sample of chromium (III) nitrate is placed in 30.0 mL of a 0.100 M (molarity) barium hydroxide solution. What is the molarity of the chromium (III) nitrate solution before the reaction occurred?

I found the balanced equation to be:

2Cr(NO_{3})_{3} + 3BaOH_{2} --> 2CrOH_{3} + 3Ba(NO_{3})_{2}

After I do this am I suppose to convert 9.3 grams of chromium (III) nitrate into either volume or molarity so I can use the formula:

V_{1}xM_{1}=V_{2}xM_{2} ?????

If not, what should my next step be? Thanks so much for any help. :D