What is the concentration of potassium sulfate when a 0.65*mol quantity is dissolved in 2.5*L of aqueous solution?

Jul 30, 2017

$\left[{K}_{2} S {O}_{4}\right] = 0.26 \cdot m o l \cdot {L}^{-} 1$
By definition, $\text{molarity"="Moles of solute"/"Volume of solution}$
And thus $\left[{K}_{2} S {O}_{4} \left(a q\right)\right] = \frac{0.65 \cdot m o l}{2.5 \cdot L} = 0.26 \cdot m o l \cdot {L}^{-} 1$; what are the concentrations of this solution with respect to (i) $S {O}_{4}^{2 -}$ ion, and (ii) ${K}^{+}$ ions?
What is the concentration with respect to potassium sulfate in $g \cdot {L}^{-} 1$?