A barium chloride solution is prepared by transferring 20 g of barium chloride to 1.0 liters of water. Calculate the chloride concentration in milliequivalents per liter of this solution.
A) 1.92 mEq Cl/L
B) 19.2 mEq Cl/L
C) 192.0 mEq Cl/L
D) 384 mEq Cl/L

Question

Quizplus · Accepted Answer

The molecular weight of barium chloride (BaCl2) is approximately 137.33 g/mol for barium and 35.45 g/mol for each chlorine atom, totaling approximately 208.23 g/mol. Since each molecule of BaCl2 releases two chloride ions upon dissolution, the number of moles of chloride ions will be twice the number of moles of BaCl2. $$ \text{Moles of BaCl2} = \frac{20 \text{ g}}{208.23 \text{ g/mol}} \approx 0.096 \text{ mol} $$$$ \text{Moles of Cl}^- = 0.096 \text{ mol} \times 2 = 0.192 \text{ mol} $$Since 1 equivalent (Eq) of chloride ion equals 1 mole of chloride ion (because the valency of chloride is 1), the concentration of chloride ions in milliequivalents per liter (mEq/L) is:$$ 0.192 \text{ mol/L} \times 1000 = 192.0 \text{ mEq/L} $$

A Barium Chloride Solution Is Prepared by Transferring 20 G