We’re being asked to compare the osmotic pressure of 0.10 M solution of NaCl and 0.10 M solution of KBr.** **We are given the molarity which we can relate to osmotic pressure.

The ** osmotic pressure (Π)** of a solution is related to the molarity of the solution:

$\overline{){\mathbf{\Pi}}{\mathbf{=}}{\mathbf{iMRT}}}$

where:

**i** = van’t Hoff factor

**M** = molarity of the solution (in M or mol/L)

**R** = gas constant (0.08206 atm • L/mol • K)

T = temperature

Is the osmotic pressure of a 0.10 M solution of NaCl greater than, less than, or equal to that of a 0.10 M solution of KBr?

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