Now, by definition, "molarity"="moles of solute (mol)"/"volume of solution (L)"molarity=moles of solute (mol)volume of solution (L).
Now the wording of your problem gave us that 2.25*mol2.25⋅mol sulfuric acid were dissolved in water to give us 725*mL725⋅mL of solution. Had it said that 2.25*mol2.25⋅mol sulfuric acid were dissolved in 725*mL725⋅mL of water, we would be uncertain as to the volume of the sulfuric acid solution. Do you appreciate the distinction I make here?
And thus, we simply have to address the quotient:
(2.25*mol)/(725*mLxx10^-3L*mL^-1)=3.10*mol*L^-12.25⋅mol725⋅mL×10−3L⋅mL−1=3.10⋅mol⋅L−1 WITH RESPECT TO SULFURIC ACID.
Again, I am trying to be cautious in my wording, and chemists often speak of a "formal concentration"formal concentration to indicate that of course in solution, the solute might speciate, and certainly sulfuric acid does, to H_3O^+H3O+, and HSO_4^(-)HSO−4, and SO_4^(2-)SO2−4. As a practical chemist, you would treat this solution as [SO_4^(2-)]=3.10*mol*L^-1[SO2−4]=3.10⋅mol⋅L−1, and [H_3O^+]=6.20*mol*L^-1[H3O+]=6.20⋅mol⋅L−1. Capisce?
