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

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Answer 1 · 2017-07-24T07:51:21

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

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#.

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