First, I know that strong acids are assumed to dissociate completely in water, so that the concentration of $\ce{H+}$ which they provide equals their concentration.
What I am asking for is not the concentration of $\ce{H+}$ which they provide, but $\ce{[H+]}$ for the solution, since the $\ce{H+}$ ions that they provide will not stay aloof, but rather will react with water and with $\ce{OH-}$ ions that are produced in the self-ionization of water.
Won't the reaction of $\ce{H+}$ ions with water shift the self-ionization of water $$\ce{H2O <=> H+ + OH-}$$ to the left and won't their reaction with $\ce{OH-}$ shift it to the right according to Le Châtelier’s principle?
So, what will $\ce{[H+]}$ be for the solution?