We are being asked to calculate the osmotic pressure of a 9.3×10^{−2} M potassium sulfate solution at 306K using the van’t Hoff factor in the table

Osmotic pressure (**Π)** is given by the equation:

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

where

i = van't Hoff factor

M = molarity

R = gas constant

T = temperature

Use the van't Hoff factors in the table below to calculate each colligative property:

Van't Hoff Factors at 0.05 m Concentration in Aqueous Solution

Solute | /Expected | /Measured |

Nonelectrolyte | 1 | 1 |

NaCl | 2 | 1.9 |

MgSO_{4} | 2 | 1.3 |

MgCl_{2} | 3 | 2.7 |

K_{2}SO_{4} | 3 | 2.6 |

FeCl_{3} | 4 | 3.4 |

Calculate the osmotic pressure of a 9.3×10^{−2} M potassium sulfate solution at 306K.

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Our tutors have indicated that to solve this problem you will need to apply the The Colligative Properties concept. You can view video lessons to learn The Colligative Properties. Or if you need more The Colligative Properties practice, you can also practice The Colligative Properties practice problems.

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