A commercially sold conc. HCl is 35 % HCl by mass. If the density of this commercial acid is 1.46 g / mL, the molarity of this solution is: (Atomic mass: Cl =35.5 amu , H =1 amu )

Question

A commercially sold conc. HCl is 35 % HCl by mass. If the density of this commercial acid is 1.46 g / mL, the molarity of this solution is: (Atomic mass: Cl =35.5 amu , H =1 amu ) (A) 10.2 M (B) 12.5 M (C) 14.0 M (D) 18.2 M

Tardigrade Admin · Accepted Answer

Let total volume =1000 mL =1 L total mass of solution =1460 g mass of HCl =(35/100) × 1460 moles of HCl =(35 × 1460/100 × 36.5) So molarity =(35 × 1460/100 × 36.5)=14 M

Q. A commercially sold conc. $H Cl$ is $35% H Cl$ by mass. If the density of this commercial acid is $1.46 g / m L$ , the molarity of this solution is :
(Atomic mass : $Cl = 35.5 am u, H = 1 am u$ )

10.2 M

12.5 M

14.0 M

18.2 M

Let total volume $= 1000 m L = 1 L$
total mass of solution $= 1460 g$
mass of $H Cl = \frac{35}{100} \times 1460$
moles of $H Cl = \frac{35 \times 1460}{100 \times 36.5}$
So molarity $= \frac{35 \times 1460}{100 \times 36.5} = 14 M$

Q. A commercially sold conc. HCl is 35%HCl by mass. If the density of this commercial acid is 1.46g/mL, the molarity of this solution is : (Atomic mass : Cl=35.5amu,H=1amu )