What mass of barium chloride is present in a #100*mL# of barium chloride solution of #0.250*mol*L^-1# concentration?

1 Answer
Jul 24, 2017

Answer:

Well, by definition, #"Concentration"="Moles of stuff"/"Volume of solution"#. I gets a mass of approx. #5*g#.

Explanation:

And thus, #"moles of stuff"="concentration"xx"volume of solution"#.

And in turn, #"moles of stuff"="Mass of stuff"/"Molar mass of stuff"#.

We have a #100*cm^3# volume of a #0.250*mol*L^-1# solution of #BaCl_2#. And #1*cm^3=1*mL=10^-3*L#.

And so .................#"moles of barium chloride"=100xx10^-3*cancelLxx0.250*mol*cancel(L^-1)#

#-=100xx10^-3xx0.250*mol-=0.0250*mol#.

The molar mass of barium chloride is #208.23*g*mol^-1#.

And thus #"mass"=0.0250*molxx208.23*g*mol^-1=??*g#.