# A 5.95*g mass of potassium bromide were dissolved in 400*cm^3 water ... what was the concentration of the solution in mol*L^-1?

Approx. $0.1 \cdot m o l \cdot {L}^{-} 1$......................
We use the quotient.....$\text{Molarity"-="Moles of solute"/"Volume of solution}$, and we know that $1 \cdot c {m}^{3} \equiv 1 \cdot m L \equiv {10}^{-} 3 \cdot L$......
And thus $\text{Molarity} = \frac{\frac{5.95 \cdot g}{119.0 \cdot g \cdot m o {l}^{-} 1}}{400 \cdot c {m}^{3} \times {10}^{-} 3 \cdot L \cdot c {m}^{-} 3}$
$= 0.125 \cdot m o l \cdot {L}^{-} 1$ with respect to $K B r$. What are the concentrations with respect to ${K}^{+}$ and $B {r}^{-}$? Are the units I use correct?