text: Why are you messing with this if you cant do simple stoichiometry?\n\nAre you sure this stuff is pure?... and not at a different Molarity?\nif so... \n(Molarity X Volume)concentrated = (M X Vol) dilute\n\nYou need to find the # moles... so since you have a the volume of pure Trifloroacetic acid you need its density and molar mass.\n\nDensity = 1.531 g/ml\nMM = 114.03 g/mol\n\ndensity X Volume = Mass =   153.1 grams\n\nMass / Molar mass = moles =   1.342629 moles\n\nMolarity = moles/Liter = 2...... Liters are the unknown here\n\n2= 1.342629/X\n\nX= .67131 L\nYou need a total volume of the solution to be 671.31 ml... to be 2M\n\nSo add acid to Deionized H2O to get the total volume of 671.31\n\nHave fun!\n\nP.S. Nearly forgot since your inexperienced with lab techniques... safety first!  Add acid to water... not water to acid!  \n\nhttp://antoine.frostburg.edu/chem/senese/101/safety/faq/always-add-acid.shtml