`20 mg` of `K^(o+)` ions are present in `1 L` of aqueous solution. Density of the solution is `0.8 mL^(-1)`. What is the concentration of `K^(o+)` ions in ppm?

Explanation

Mass of `K^(o+)` ions `(W_(2)) = 20 mg = 20 xx 10^(-3) g`
Mass of solution `= V_(sol) xx d_(sol) = 100 mL xx 0.8 g mL^(-1) = 800 g`
`ppm = (W_(2) xx 10^(6))/(W_(sol)) = (20 xx 10^(-3) xx 10^(6))/(800) = 25 ppm`