The osmotic pressure of a 0.010 M aqueous solution of CaCl 2 is found to be 0.674 atm at 25 °C. Calculate the van't Hoff factor, i, for the solution.

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

Ch.13 - Properties of Solutions

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Brown 14th Edition

Ch.13 - Properties of Solutions

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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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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Osmotic Pressure

Osmotic pressure is the pressure required to prevent the flow of solvent into a solution through a semipermeable membrane. It is directly proportional to the concentration of solute particles in the solution and can be calculated using the formula π = iCRT, where π is the osmotic pressure, i is the van't Hoff factor, C is the molarity of the solution, R is the ideal gas constant, and T is the temperature in Kelvin.

van't Hoff Factor (i)

The van't Hoff factor, denoted as i, represents the number of particles into which a solute dissociates in solution. For ionic compounds, i is greater than 1, as they separate into multiple ions. For example, CaCl2 dissociates into one calcium ion (Ca²⁺) and two chloride ions (Cl⁻), resulting in a van't Hoff factor of 3. This factor is crucial for calculating colligative properties like osmotic pressure.

Colligative Properties

Colligative properties are properties of solutions that depend on the number of solute particles rather than their identity. These properties include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure. Understanding colligative properties is essential for predicting how solute concentration affects the physical behavior of solutions, particularly in the context of osmotic pressure calculations.

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Colligative Properties

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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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Key Concepts

Osmotic Pressure

van't Hoff Factor (i)

Colligative Properties

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.