83 -- 200 grams of a 2.22 percent by mass solution of calcium chloride is mixed with a sufficient amount of solid sodium phosphate. The solution formed is 1800 mL. After the reaction is complete, the chloride ion concentration at the end of the reaction, after separating the precipitate, the balanced equation of the reaction is taken into account, from the change in mass of the solution, what is the concentration in ppm? $$\mathrm{CaCl_2(aq) + Na_3PO_4(s) \rightarrow Ca_3(PO_4)_2(s) + NaCl(aq)} \qquad (\mathrm{Cl = 35.5,\ Ca = 40 : g.mol^{-1}})$$ (1) 2840 (2) 1420 (3) 4260 (4) 5680
\textbf{83 --} 200 grams of a 2.22 percent by mass solution of calcium chloride is mixed with a sufficient amount of solid sodium phosphate. The solution formed is 1800 mL. After the reaction is complete, the chloride ion concentration at the end of the reaction, after separating the precipitate, the balanced equation of the reaction is taken into account, from the change in mass of the solution, what is the concentration in \textbf{ppm}?
$$\mathrm{CaCl_2(aq) + Na_3PO_4(s) \rightarrow Ca_3(PO_4)_2(s) + NaCl(aq)} \qquad (\mathrm{Cl = 35.5,\ Ca = 40 : g.mol^{-1}})$$
(1) 2840 \hfill (2) 1420 \hfill (3) 4260 \hfill (4) 5680
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