An **osmole** (Osmol) is 1 mol of particles that contribute to the osmotic pressure of a solution.

For example, dextrose is a nonelectrolyte.

1 mol of dextrose gives 1 mol of particles in solution. So.

#"1 mol dextrose = 1 Osmol dextrose"#

Thus, the osmolarity of the dextrose in your solution is

#"Osmolarity" = (20 color(red)(cancel(color(black)("mmol"))))/(100 color(red)(cancel(color(black)("mL")))) × (1000 color(red)(cancel(color(black)("mL"))))/"1 L" × "1 mOsmol"/(1 color(red)(cancel(color(black)("mmol")))) = "200 mOsmol/L"#

#"KCl"# dissociates completely in water to form #"K"^+# ions and #"Cl"^"-"# ions.

Thus, each mole of #"KCl"# becomes two osmoles in solution: one of #"K"^+# and one of #"Cl"^"-"#.

The osmolarity of #"KCl"# in your solution is

#"Osmolarity" = (4 color(red)(cancel(color(black)("mmol"))))/(100 color(red)(cancel(color(black)("mL")))) × (1000 color(red)(cancel(color(black)("mL"))))/"1 L" × "2 mOsmol"/(1 color(red)(cancel(color(black)("mmol")))) = "80 mOsmol/L"#

The total osmolarity of the solution is the sum of the individual osmolarities.

#"Total osmolarity" = "(200 + 80) mOsmol/L" = "280 mOsmol/L"#