What mass of chromium II chlroide (CrCl2) is dissolved in 150.0mL of solution to prepare .250M solution?
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How many mols do you need? That's M x L = mols.
Then mols = grams/molar mass. You knopw mols and molar mass, solve for grams.
g=.00461 ?
I don't think so. I think that is off by a factor of 1000. You can check yourself this way.
mols CrCl2 = 0.00461g/122.9.
Then M = mols/0.150 and that is not 0.25M.
To find the mass of chromium II chloride (CrCl2) dissolved in 150.0 mL of solution to prepare a 0.250 M solution, we need to use the formula:
Molarity (M) = (moles of solute) / (volume of solution in liters)
First, we need to convert the volume of solution from milliliters (mL) to liters (L):
150.0 mL = 150.0 mL * (1 L / 1000 mL) = 0.150 L
Next, we rearrange the formula to solve for moles of solute:
moles of solute = Molarity (M) * volume of solution (L)
moles of solute = 0.250 M * 0.150 L = 0.0375 moles
To find the mass of chromium II chloride (CrCl2), we need to use its molar mass. The molar mass of CrCl2 is:
Cr: 51.996 g/mol
Cl: 35.45 g/mol (x 2 since there are two chlorine atoms in CrCl2)
Molar mass of CrCl2 = (51.996 g/mol) + (35.45 g/mol * 2) = 85.890 g/mol
Now, we can calculate the mass of CrCl2:
mass of CrCl2 = moles of solute * molar mass of CrCl2
mass of CrCl2 = 0.0375 moles * 85.890 g/mol = 3.218 g
Therefore, the mass of chromium II chloride (CrCl2) dissolved in 150.0 mL of solution to prepare a 0.250 M solution is 3.218 grams.