StudyGPT Just Leveled Up – Say Hello to Knowee! 🚀
Knowee
Questions
Features
Study Tools

At 300K, what is the relation between the osmotic pressure of two equimolar solutions, onewhose Van’t Hoff factor is 2 and for the other is ½?

Question

🧐 Not the exact question you are looking for?Go ask a question

Solution

To determine the relation between the osmotic pressure of two equimolar solutions at 300K, one with a Van't Hoff factor of 2 and the other with a Van't Hoff factor of 1/2, we can use the formula for osmotic pressure:

π = iMRT

Where: π is the osmotic pressure, i is the Van't Hoff factor, M is the molarity of the solution, R is the ideal gas constant, and T is the temperature in Kelvin.

For the solution with a Van't Hoff factor of 2, the osmotic pressure can be calculated as:

π1 = (2)(M)(R)(T)

For the solution with a Van't Hoff factor of 1/2, the osmotic pressure can be calculated as:

π2 = (1/2)(M)(R)(T)

To find the relation between the two osmotic pressures, we can divide π1 by π2:

π1/π2 = [(2)(M)(R)(T)] / [(1/2)(M)(R)(T)]

Simplifying the equation, we can cancel out the common factors:

π1/π2 = 4

Therefore, the relation between the osmotic pressure of the two equimolar solutions is that the osmotic pressure of the solution with a Van't Hoff factor of 2 is four times greater than the osmotic pressure of the solution with a Van't Hoff factor of 1/2.

This problem has been solved

Upgrade your grade with Knowee

Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.