How many mL of a 2.50 M K2SO4 solution are required to obtain 1.20 moles of K2SO4?

• A. 480 mL
• B. 600 mL
• C. 240 mL
• D. 300 mL

Answer: (A)

Verified step by step guidance

1. Start by understanding the relationship between molarity, moles, and volume. Molarity (M) is defined as moles of solute per liter of solution. The formula to use here is: \( M = \frac{n}{V} \), where \( M \) is molarity, \( n \) is the number of moles, and \( V \) is the volume in liters.
2. Rearrange the formula to solve for volume: \( V = \frac{n}{M} \). This will allow you to find the volume of the solution needed to obtain the desired number of moles.
3. Substitute the given values into the rearranged formula. You have \( n = 1.20 \) moles and \( M = 2.50 \) M. So, \( V = \frac{1.20}{2.50} \).
4. Calculate the volume in liters using the formula. This will give you the volume in liters required to obtain 1.20 moles of \( K_2SO_4 \).
5. Convert the volume from liters to milliliters. Since 1 liter is equal to 1000 milliliters, multiply the volume in liters by 1000 to get the volume in milliliters.