Answer :

To find the volume of a 1.00 M (molar) LiF (Lithium Fluoride) solution needed to provide 1.50 moles of LiF, we can use the formula relating moles, molarity, and volume:

[tex]\[ \text{Moles} = \text{Molarity} \times \text{Volume} \][/tex]

We need to calculate the volume in liters. Rearranging the formula for volume, we get:

[tex]\[ \text{Volume} = \frac{\text{Moles}}{\text{Molarity}} \][/tex]

Given:
- The moles of LiF needed ([tex]\( \text{n} \)[/tex]) = 1.50 moles
- The molarity of the solution ([tex]\( \text{C} \)[/tex]) = 1.00 M

Plugging the values into the formula:

[tex]\[ \text{Volume} = \frac{1.50 \text{ moles}}{1.00 \text{ M}} = 1.50 \text{ L} \][/tex]

Next, we convert the volume from liters to milliliters. Since 1 liter (L) = 1000 milliliters (mL):

[tex]\[ 1.50 \text{ L} \times 1000 \text{ mL/L} = 1500 \text{ mL} \][/tex]

Therefore, the volume of a 1.00 M LiF solution needed to provide 1.50 moles of LiF is 1500 mL.

So, the correct answer is:

D. 1500 mL