Final answer:
To make a 0.300 M CaCl2 solution with a volume of 5.5 L, a chemist should use 1821.39 grams of CaCl2.
Step-by-step explanation:
To calculate the mass of CaCl2 needed to make a 0.300 M solution, we can use the formula:
Mass = Molarity x Volume x Molar mass.
To determine the mass of CaCl2 (in g) a chemist should use to make 5.5 L of a 0.300 M CaCl2 solution, we'll use the molarity equation: Molarity (M) = moles of solute / volume of solution in liters (L).
First, we need to calculate the number of moles of CaCl2 needed for this concentration and volume:
Moles of CaCl2 = 0.300 M × 5.5 L = 1.65 moles of CaCl2.
Next, we find the mass using te molar mass of CaCl2 (110.98 g/mol):
First, we need to convert the volume of the solution from liters to milliliters, since the molar mass of CaCl2 is given in grams per mole. 5.5 liters is equal to 5500 milliliters.
Then, we can substitute the values into the formula:
Mass = 0.300 mol/L x 5500 mL x 110.98 g/mol = 1821.39 grams.