Determine the volume (in mL) of a 0.184 M CaCl2 solution that would be required to obtain 73.4 g of CaCl2.

0.184 x molar mass = grams CaCl2/L = 20.42 grams. So if you have 20.42 g in 1000 mL, how many mL will it take to obtain 73.4g.

To determine the volume (in mL) of a 0.184 M CaCl2 solution that would be required to obtain 73.4 g of CaCl2, we need to use the formula:

Molarity (M) = moles of solute / volume of solution in liters

First, we need to calculate the number of moles of CaCl2.

The molar mass of CaCl2 is calculated by adding the atomic masses of calcium (Ca) and chlorine (Cl). The atomic mass of Ca is 40.08 g/mol, and the atomic mass of Cl is 35.45 g/mol.

Molar mass of CaCl2 = (1 x Ca atomic mass) + (2 x Cl atomic mass) = 40.08 + (2 x 35.45) = 110.98 g/mol

Now, we can calculate the number of moles of CaCl2:

moles = mass / molar mass = 73.4 g / 110.98 g/mol = 0.661 mol

Next, we need to use the molarity formula and rearrange it to solve for volume:

Volume (in liters) = moles of solute / Molarity

Since the molarity is given as 0.184 M, we can substitute the values into the equation:

Volume (in liters) = 0.661 mol / 0.184 M = 3.59 L

Finally, we need to convert the volume from liters to milliliters by multiplying it by 1000:

Volume (in mL) = 3.59 L x 1000 mL/L = 3590 mL

Therefore, the volume of a 0.184 M CaCl2 solution that would be required to obtain 73.4 g of CaCl2 is 3590 mL.