If the molality of a CaCl2 solution is .100 mol/kg, and was made from 500.0 mL of water, how many grams of CaCl2 were needed to make the solution?
Step by step would be appreciated!
3 answers
DrBob222, do you know how to do this?
The density of H2O=1g/mL, solve for mass.
mass=density*volume=(1g/mL)*(500mL)=500g or 0.500 kg
m=moles of solute/kg of solvent, solve for moles
(0.100 mol/kg)*(0.500 kg)= moles of CaCl2
moles of CaCl2*(111.0g/mole)= mass of CaCl2
****I'm not Dr. Bob222, but I think this is correct.
mass=density*volume=(1g/mL)*(500mL)=500g or 0.500 kg
m=moles of solute/kg of solvent, solve for moles
(0.100 mol/kg)*(0.500 kg)= moles of CaCl2
moles of CaCl2*(111.0g/mole)= mass of CaCl2
****I'm not Dr. Bob222, but I think this is correct.
I'll buy all of that. Something like 5.55 g if I punched in the right numbers
2 answers