Help?
How many moles of LiF would be required to produce a 2.5 M solution with a volume of 10.5 L?
10.5L/(2.5moles/L) = 4.2 moles
To find the number of moles of LiF required to produce a 2.5 M solution with a volume of 10.5 L, we can use the formula:
Molarity (M) = Moles (mol) / Volume (L)
Rearranging the formula, we get:
Moles (mol) = Molarity (M) × Volume (L)
Given that the molarity is 2.5 M and the volume is 10.5 L, we can substitute these values into the formula:
Moles (mol) = 2.5 M × 10.5 L
Multiplying the molarity and the volume, we get:
Moles (mol) = 26.25 mol
Therefore, 26.25 moles of LiF would be required to produce a 2.5 M solution with a volume of 10.5 L.