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

Question

4066 views around the world

You can reuse this answer
Creative Commons License

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*mL100*mL of barium chloride solution of 0.250*mol*L^-10.250*mol*L^-1 concentration?