17.9 mL of 0.290 M HBr is mixed with 38.1 mL of 0.74 M HCl. What is the molarity of the H+

So Im on my last attempt on the Homework problem and I wanna make sure i got this right.
Please tell me if what i calculated is correct. Please correct me if I totally messed up.

HBr
.0179 x .290 = .005191
HCl
.0381 x .74 = .028194

.005191 + .028194 = .033385

.033385/(.01791 + .0381) = .60 M H+

So .60 H+ is the Molarity?

Since both HBr and HCl are strong acids and completely ionized, your calculations are correct, but watch your significant figures. Your answer should have 3 significant figures and be 0.600 M. Also remember to include units in your calculations.