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

(i) 38% IIC1 by mass means that 38 g of IIC1 is present in 100 g of solution.
Volume of solution `=("Mass")/("Density") = 100/(1.19) = 84.03` mL
Moles of HCl =`38/36.5 = 1.04`
Molarity `=(1.04 xx 1000)/(84.03) = 12.38` M
(ii) The volume of this solution required to make 1.0 L of 0.10 M HC1 can be calculated by applying molarity equation as:
`underset("acid"_(1))(M_(1)V_(1)) = underset("acid2")(M_(2)V_(2))`
`12.28 M xx V_(1) = 0.10 M xx 1.0 L`
`therefore V_(1) = (0.10 xx 1.0)/12.38 = 0.00808 L` or `=8.08 cm^(3)`