Question

How can we prepare $0.1$ N HCl solution?

Answer 1

Step1: Molar mass for HCl = $36.4611$g/mol

The volume will be in $1$ litre and the specific gravity of HCl is $1.189$

Step 2: Volume= Mass/Density

Step3:Compound required in grams = ($0.1$ N)($36.4611$)($1$Litre) = $3.3461$

Volume of concentrated acid required = ($3.3461$)/l$0.375\times 1.189)=8.1774$ml

Therefore,$8.1774$ ml of $37.5\%$ concentrated HCl is required to prepare $0.1$ M HCl