Commercially availiable concentrated hydrochloric acid contains `38% HCl` by mass. (a) What is the molarity of this solution? The density is `1.19g mL^(-1)` ?
(b) What volume of concentrated `HCl` is required to make `1.00 "litre"` of `0.10M HCl`?

Explanation

(a) `"Mass of" HCl= 38 g`,
`"density of solution"=1.19g//mL`,
`"Mass of solution" -100 g`
`"Molarity"=("Moles of"HCl)/("Volume of solution in litre")`
`=("Mass of "HCl)/("Molar mass of "HClxx("Weight of solution")/("density of solution"xx1000))`
`=(38)/(36.5xx(100)/(1.19xx1000))=12.4`
(b) MIlli-moles of solute does not change on dilution and this,
`{:(MxxV_(mL),=,MxxV_(mL),,),("(for conc.)",=,"(for dil)",,):}`
`12.4xxV= 0.1xx100 `
`V= 8.06mL`