Question

An aqueous 2.00 M hydrochloric acid solution is prepared with a total volume of 0.350 L. The molecular

Answer 1

Answer : The mass of hydrochloric acid (in grams) needed for the solution is, 25.5 grams.

Explanation : Given,

Molarity of $HCl$ = 2.00 M

Volume of solution = 0.350 L

Molar mass of $HCl$ = 36.468 g/mole

Molarity : It is defined as the number of moles of solute present in one liter of volume of solution.

Formula used :

$\text{Molarity}=\frac{\text{Mass of }HCl}{\text{Molar mass of }HCl\times \text{Volume of solution (in L)}}$

Now put all the given values in this formula, we get:

$2.00M=\frac{\text{Mass of }HCl}{36.468g/mole\times 0.350L}$

$\text{Mass of }HCl=25.5g$

Therefore, the mass of hydrochloric acid (in grams) needed for the solution is, 25.5 grams.