1. The problem statement, all variables and given/known data A student added 50.0mL of an NaOH solution to 100.0 mL of 0.400 M HCL. The solution was then treated with an excess of aqueous chromium (III) nitrate, resulting in formation of 2.06g of precipitate. Determine the concentration of the NaOH solution. 2. Relevant equations pH=14-pOH 3. The attempt at a solution NaOH + HCL -> NaCL +H2O Cr(NO3)3 + HCL -> Cr(OH)3 + 3NaNO3 I'm not sure what to do after creating the equations. I tried to use the 2.06g and converting this to moles using the molar weight of 3NaNO3, but i think I'm not doing the right steps. Any help?