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

Jul 24, 2017

Well, by definition, $\text{Concentration"="Moles of stuff"/"Volume of solution}$. I gets a mass of approx. $5 \cdot g$.

#### Explanation:

And thus, $\text{moles of stuff"="concentration"xx"volume of solution}$.

And in turn, $\text{moles of stuff"="Mass of stuff"/"Molar mass of stuff}$.

We have a $100 \cdot c {m}^{3}$ volume of a $0.250 \cdot m o l \cdot {L}^{-} 1$ solution of $B a C {l}_{2}$. And $1 \cdot c {m}^{3} = 1 \cdot m L = {10}^{-} 3 \cdot L$.

And so .................$\text{moles of barium chloride} = 100 \times {10}^{-} 3 \cdot \cancel{L} \times 0.250 \cdot m o l \cdot \cancel{{L}^{-} 1}$

$\equiv 100 \times {10}^{-} 3 \times 0.250 \cdot m o l \equiv 0.0250 \cdot m o l$.

The molar mass of barium chloride is $208.23 \cdot g \cdot m o {l}^{-} 1$.

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