Posted by Emily on .
I need help with this question!!
a sample of pure KHP weighing .8097g dissolved in water and titrated with 40.25 mL of NaOH solution. The same NaOH solution was used to titrate a solution of a weak diprotic acid H2X. A sample of 0.18694g of the weak acid was first dissolved in water in a 100 mL volumetric flask creating a solution of 100.00 mL. A 25.00 mL portion of this solution was tuitrated with the sodium hydroxide solution. The titration required 28.02 mL of the basic solution. What is the molar mass of the weak acid H2X?
I know that the KHP and the NaOH have a 1:1 mole ratio, and then using that you can substitute it to the formula H2X+NaOh=Na2X+H2O, and then make a IRF table...? PLEASE help!!!
College Chemistry -
the species of H3o+ can be called which of the following?