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**QUESTION:**

You have an unknown triprotic acid, H

_{3}X, and have titrated it with 22.53mL of NaOH. The pH of the unknown solution is 2.04 and the concentration is 48.028g/2L. While the concentration of the NaOH is 0.251mol/L. What is the molar mass, as well as the first and second ionization constant (K

_{a1}) for the unknown triprotic acid H

_{3}X?

**WORK SO FAR:**

H

_{3}X + 3NaOH --------> Na3X + 3H

_{2}O

I know that if I solve for the concentration of the unknown by using the formula 3CaVa=CbVb I get 0.334 mol/L , but then what was the point of being given a concentration?

I really don't understand how to move forward from this point. So any help would be appreciated.

Thanks in advance :)