Answer:
6.0 moles.
Explanation:
To solve this problem, we have to use the molarity formula. Remember that the molarity (M) of a solution is the number of moles of solute dissolved in one liter of solution:
[tex]Molarity\text{ \lparen M\rparen=}\frac{moles\text{ of solute}}{liter\text{s of solution}}=\frac{mol}{L}.[/tex]We want to find 'moles of solute', so we have to solve for this unknown value and replace the given data (molarity = 2.0 M, liters of solution = 3.0 L):
[tex]\begin{gathered} Moles\text{ of solute=molarity}\cdot liters\text{ of solution,} \\ \\ Moles\text{ of solute=2.0 M}\cdot3.0\text{ L,} \\ \\ Moles\text{ of solute= 6.0 moles.} \end{gathered}[/tex]The answer would be that we require 6.0 moles to prepare the wanted solution.
