Now this is concentrated sulfuric acid...and to find its molarity we interrogate the quotient....
#"Moles of sulfuric acid"/"Volume of solution"#
And we can assess its concentration by taking a #1*mL# volume and thus....
#((98%xx1.80*cancelg)/(98.08*cancelg*mol^-1))/(1xx10^-3*L)=??*mol*L^-1#.....
Of course this is consistent dimensionally, in that #1/(mol^-1)=1/(1/(mol))=mol# as required.........
Sometimes in the lab when you lift Winchesters (i.e. glass bottles of #2.5*L# volumes) of say sulfuric acid, from the cabinet to a basket, you are surprised at its weight....as you are not surprised by the mass of Winchesters of organic solvent, whose densities are often less than #1*g*mL^-1#. In the same way, you might pick up a bottle of mercury with a small volume of #10*mL# to #20*mL# of metal, and be impressed by the mass of the bottle; #rho_"Hg"=13.6*g*mL^-1#...
