1. The problem statement, all variables and given/known data In a lab, 40.3 mL Mn2+ is mixed with 5 mL H3PO4. 0.4g of potassium periodate is added. The flask is heated and then diluted to 100mL. The final solution prepared is a permanganate solution. Calculate the final molarity of the solution. C Mn2+ = 0.06061 M (60.61 micrograms/ mL) C H3PO4 = 15 M V Mn2+ = 40.3 mL V H3PO4 = 5 mL M (Mn2+) = 54.94 g/mol V final = 100mL 2. Relevant equations C1V1=C2V2 2Mn2+ + 5IO4- + 3H2O ---> 2MnO4- + 5IO3- + 6H+ 3. The attempt at a solution (60.62 * 40.3 *10^-6) / (54.94 *0.100) = 4.45 *10^-4 M The 10^-6 was used as a conversion factor from micrograms to grams. I'm not sure if this is right, as it is not taking into account the H3PO4 added.