Commercially available $HCl$ contains $38\%$ $HCl$ by mass. Calculate molality of the solution.

Q. Commercially available concentrated hydrochloric acid contains $38$ $HCl$ by mass.
$\left(i\right)$ What is the molarity of the solution (density of solution = $1.19gm{L}^{-1}$)?
$\left(ii\right)$ What volume of concentrated $HCl$ is required to make $1.0L$ of an $0.10MHCl?$

Q. Commercially available conc. HCl contains 38% HCl by mass, what is the molarity of the solution, density of solution = 1.19 g/ml. What volume of conc. HCl is required to make 10. L of an 0.10 M HCl

Q.

Commercialy available concentrated HCl contains 38% HCl by mass ?

1) What is the molarity of the solution ? ( d = 1.19 g/mL)

2) What volume of concentrated HCl is required to make 1 L of 0.1 M of HCL ?

Q.

Comercially available concentrated HCL contains 38% HCL by mass.

i . What is molarity of the solution.(d=1.19ml).

ii . What volume of conc. HCL is required to make 1L of 0.1 M HCL.

Q.

Commercial available concentrate HCl contain 38percent HCl by mass. What is the molarity of this solution. Density is 1.19g per cm3