text: how would i prepare 2 m tri fluoro acetic acid? how would i prepare 2 m tri fluoro acetic acid?  i have 100 ml of it. why are you messing with this if you cant do simple stoichiometry?  are you sure this stuff is pure?... and not at a different molarity? if so...  (molarity x volume)concentrated = (m x vol) dilute  you need to find the # moles... so since you have a the volume of pure trifloroacetic acid you need its density and molar mass.  density = 1.531 g/ml mm = 114.03 g/mol  density x volume = mass =   153.1 grams  mass / molar mass = moles =   1.342629 moles  molarity = moles/liter = 2...... liters are the unknown here  2= 1.342629/x  x= .67131 l you need a total volume of the solution to be 671.31 ml... to be 2m  so add acid to deionized h2o to get the total volume of 671.31  have fun!  p.s. nearly forgot since your inexperienced with lab techniques... safety first!  add acid to water... not water to acid!    http://antoine.frostburg.edu/chem/senese/101/safety/faq/always-add-acid.shtml