A) calculate the osmolarity of a 0.70% (m/v) MgSO4 solution. B) is it safe to us

Question

A) calculate the osmolarity of a 0.70% (m/v) MgSO4 solution.
B) is it safe to use this solution in an IV?
C) if the MgSO4 solution is safe to use in an IV, enter the concentration from part A into the answer module below, if it is not safe, calculate what concentration (m/v%) of the MgSO4 solution would be safe. A) calculate the osmolarity of a 0.70% (m/v) MgSO4 solution.
B) is it safe to use this solution in an IV?
C) if the MgSO4 solution is safe to use in an IV, enter the concentration from part A into the answer module below, if it is not safe, calculate what concentration (m/v%) of the MgSO4 solution would be safe.
B) is it safe to use this solution in an IV?
C) if the MgSO4 solution is safe to use in an IV, enter the concentration from part A into the answer module below, if it is not safe, calculate what concentration (m/v%) of the MgSO4 solution would be safe.

Explanation / Answer

Osmolarity is product of the molarity and the number of osmoles that each solute produces.

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

MgSO4 dissociates in to 1 mole Mg2+ and 1 mole SO4^2-, no.of osmoles = 2

Molecular weight of MgSO4 = 120.37 g/mol

0.70 % MgSO4 means 0.70 g in 100 ml or 7.0 g in 1000 ml (1L).

7 g MgSO4 = 7 g /120.37 g/mol = 0.0581 mol

Osmolarity = 0.116 osmole / L = 116 mOsmole/ L

b)

It is too low in osmolarity and is not safe.

c)

The normal range of IV is 300 mOsmole /L - 310 mOsmole/ L.

For this approximately 0.1575 moles of MgSO4 is needed, so that

Osmolarity becomes = 0.152 x 2 = 0.304 Osmole/L = 304 mOsmole/L

0.152 moles = 0.152 x 120.37 = 18.30 g /L = 1.83 g /100 no

So MgSO4 concentration should be approximately = 1.83% (m/v)

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