How many grams of CaCl2 would be required to produce a 3.5M(molar) solution with a volume of 2.0L?
mols needed = M x L = ?
Then mols = grams/molar mass. You know molar mass and mols, solve for grams.
To determine how many grams of CaCl2 are required to produce a 3.5M solution with a volume of 2.0L, we need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
First, let's rearrange the formula to solve for moles of solute:
moles of solute = Molarity (M) x volume of solution (L)
Now, let's plug in the values we know:
Molarity (M) = 3.5M
Volume of solution = 2.0L
moles of solute = 3.5M x 2.0L = 7.0 moles
To convert moles of CaCl2 to grams, we need to know the molar mass of CaCl2, which can be calculated by adding up the atomic masses of calcium (Ca) and chlorine (Cl):
Molar mass of CaCl2 = (1 mol of Ca) + (2 moles of Cl) = 40.08 g/mol + (2 x 35.45 g/mol) = 110.98 g/mol
Now that we know the molar mass of CaCl2, we can calculate the mass required using the formula:
mass (g) = moles x molar mass
mass (g) = 7.0 moles x 110.98 g/mol = 776.86 grams
Therefore, approximately 776.86 grams of CaCl2 would be required to produce a 3.5M solution with a volume of 2.0L.