Answer:
[tex]Ca^{2+}[/tex]= 4.0959 ppm
[tex]Mg^{2+}[/tex]= 0.3296 ppm
Explanation:
ppm means milligram of solute per kilogram of solution.
[tex]ppm= \frac{mg of solute}{Kg of solution}[/tex]
Solutes: [tex]Ca^{2+} y Mg^{2+}[/tex]
Mass [tex]Ca^{2+}[/tex] = 0.410g
Mass [tex]Mg^{2+}[/tex] = 0.0330g
Solution: 100.0 L, whose density is 1.001 g/mL
First, let us to calculate mass of solution:
[tex]100.0 L * \frac{1.001 g }{1 mL } * \frac{1000 mL}{1 L} * \frac{1 kg}{1000 g} =[/tex]= 100.1 kg
Now, we have to calculate ppm [tex]Ca^{2+} y Mg^{2+}[/tex]
ppm [tex]Ca^{2+}= \frac{0.410 g * (1000 mg/1g)}{100.1 Kg} =4.0959 mg/Kg[/tex]
ppm [tex]Mg^{2+}= \frac{0.0330 g * (1000 mg/1g)}{100.1 Kg} =0.3296 mg/Kg[/tex]
