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Ch.13 - Properties of Solutions
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All textbooksBrown 14th EditionCh.13 - Properties of SolutionsProblem 83

Chapter 13, Problem 83

The osmotic pressure of a 0.010 M aqueous solution of CaCl2 is found to be 0.674 atm at 25 °C. Calculate the van't Hoff factor, i, for the solution.

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Hi everyone here we have a question telling us that a 0.150 molar solution of cobalt chloride has an osmotic pressure of 11.0 atmospheres at 25°C. What is the value of the band hall factor for the solution? To calculate the Van Hoff factor, we will first calculate the osmotic pressure for the solution. Using osmotic pressure equals more clarity. Times are constant times temperature. So our polarity equals zero .150 A constant equals 0. leaders Times atmospheres divided by moles times kelvin. Our temperature Equals 25.0°C plus 273.15, Which equals 298 . Kelvin. So our osmotic pressure equals 0.150 polarity times 0. Leaders Times atmospheres divided by moles times kelvin times 298.15 kelvin, So that equals three .67 Atmospheres. Now the actual osmotic pressure is 11 atmospheres. So our van Hoff factor is going to equal actual osmotic pressure divided by our calculated osmotic pressure. So I Is going to equal atmospheres Divided by 3. Atmospheres, which equals three. And that is our final answer. Thank you for watching. Bye
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