Determine the concentrations of BaBr2, Ba2, and Br - in a solution prepared by dissolving 1.18 * 10-4 g BaBr2 in 1.00 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm).

Supposing complete ionization:

BaBr2 → Ba{2+} + 2 Br{-}

(2.23 * 10^-4 g BaBr2) / (297.135 g BaBr2/mol) / (2.00 L) = 3.75 * 10^-7 mol/L BaBr2

(3.75 * 10^-7 mol/L BaBr2) x (1 mol Ba{2+} / 1 mol BaBr2) = 3.75 * 10^-7 mol/L Ba{2+}

(3.75 * 10^-7 mol/L BaBr2) x (2 mol Br (-} / 1 mol BaBr2) = 7.50 * 10^-7 mol/L Br{-}