A chemist wants to make 5.5 L of a 0.250 M CaCl2 solution, what mass of CaCl2 (in g) should the chemist use?
massCaCL2=molarity*volume*molmassCaCl2
Wha??
M = 0.250 mols/L * (111g CaCl2/1 mols CaCl2)= 27.7g/L
n = M*L
n = (27.7g/L)*(5.5L)= 153g of CaCl2
Why did the chemist become a magician? Because they wanted to make some "CaCl2-abra" solution!
To calculate the mass of CaCl2 needed, we can use the formula:
Mass (g) = molarity (mol/L) x volume (L) x molar mass (g/mol)
First, let's find the moles of CaCl2 needed:
Moles = molarity x volume
= 0.250 mol/L x 5.5 L
= 1.375 mol
The molar mass of CaCl2 is 110.98 g/mol.
Now, let's calculate the mass of CaCl2:
Mass (g) = 1.375 mol x 110.98 g/mol
= 152.45 g
So, the chemist should use approximately 152.45 grams of CaCl2 for the 5.5 L 0.250 M solution.
To determine the mass of CaCl2 needed to make the solution, you need to use the relationship between moles, concentration, and volume. Here are the steps to solve the problem:
1. Start by determining the number of moles needed for the desired concentration. The formula to calculate moles is:
Moles = Molarity x Volume
Moles = 0.250 mol/L x 5.5 L
Moles = 1.375 mol
2. Next, find the molar mass of CaCl2. The molar mass of Ca is 40.08 g/mol, and Cl is 35.45 g/mol (there are two Cl atoms in CaCl2).
Molar mass of CaCl2 = 40.08 g/mol + 2(35.45 g/mol)
Molar mass of CaCl2 = 110.98 g/mol
3. Calculate the mass of CaCl2 by multiplying the moles obtained in step 1 by the molar mass from step 2:
Mass = Moles x Molar mass of CaCl2
Mass = 1.375 mol x 110.98 g/mol
Mass = 151.47 g
Therefore, the chemist should use 151.47 grams of CaCl2 to make 5.5 L of a 0.250 M CaCl2 solution.