What is osmolarity of a 0.20M MgSO4 solution, which is 50% dissociated?
What is osmolarity of a 0.20M MgSO4 solution, which is 50% dissociated?
To determine the osmolarity of a solution, we need to consider the number of solute particles that are present in the solution.
In this case, we have a 0.20 M (molarity) MgSO4 solution that is 50% dissociated. This means that for every 1 mole of MgSO4, only 0.5 moles of it will dissociate into ions.
MgSO4 dissociates into one Mg2+ ion and one SO4 2- ion. Therefore, for every mole of MgSO4, we will have 1 + 1 = 2 moles of solute particles.
Since the solution is 0.20 M in MgSO4, it means that there are 0.20 moles of MgSO4 present in 1 liter of the solution.
Now, to determine the osmolarity, we need to calculate the total number of moles of solute particles present in the solution:
Osmolarity = Molarity × Number of particles
In this case, the molarity is 0.20 M and the number of particles is 2 moles per mole of MgSO4.
Osmolarity = 0.20 M × 2 = 0.40 osmoles (or osmol/L)
So, the osmolarity of the 0.20 M MgSO4 solution, which is 50% dissociated, is 0.40 osmoles or 0.40 osmol/L.