Can you help me find the osmolarity of this KNO3 solution?

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To find the osmolarity of a 0.500 liter solution containing 132g of KNO3, the calculation involves determining the number of moles of KNO3 first. The molar mass of KNO3 is approximately 101.1 g/mol, leading to about 1.306 moles in 132g. Since KNO3 dissociates into two ions (K+ and NO3-), the osmolarity is calculated by multiplying the moles by the number of particles, resulting in an osmolarity of 5.224 osmoles/L. The initial confusion stemmed from assuming a 1L volume instead of the correct 0.500L. The final osmolarity is confirmed to be 5.224 osmoles/L.
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Homework Statement



I tried to solve this question, but I'm not sure if my answer is correct.

What is the osmolarity of a 0.500 liter solution containing 132g of KNO3?

Homework Equations



N/A

The Attempt at a Solution



1.306 mol/0.500 L solution x 2 mol ions/1 mol KNO3 = 5.224
 
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oceanbreeze said:

Homework Statement



I tried to solve this question, but I'm not sure if my answer is correct.

What is the osmolarity of a 0.500 liter solution containing 132g of KNO3?

Homework Equations



N/A

The Attempt at a Solution



1.306 mol/1 L solution x 2 mol ions/1 mol KNO3 = 2.612

What is the volume of solution? You seem to have assumed it to be 1L.
 
It's 0.500L. I've reworked the equation, but I'm not sure how to proceed.
 
oceanbreeze said:
It's 0.500L. I've reworked the equation, but I'm not sure how to proceed.

What answer do you reach now?
 

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