Question

A 3.56g sample of Fe is dissolved in 75.0 mL of 6.00 M HCl, forming H2(g) and FeCl2(aq). The Total volume of the resulting solution is 75.2 mL. What is the final concentration of H+ in the solution?

Answer 1

According to my professor, the final concentration is 0, but I'm not sure how to prove that numerically. I started with getting the moles of HCl from the molarity and volume given, but I don't know what to do from there.

Answer 2

Maybe ask him to do it on the board?

Answer 3

Balanced equation =

1 Fe(s) + 2 HCl (aq) --> 1 FeCl2(aq) + 1 H2(g)

Ideally, starting with 0.075 L of 6 M HCl -- Initially our concentration of H+ is [0.45 H+]

finding H+ per liter --> [0.45]/0.0752 = 6 H+/Liter initial...