Discussion Overview
The discussion revolves around calculating the number of moles of solute particles in a solution of Na3PO4, specifically focusing on the distinction between moles of solute and moles of solute particles, which involves osmolarity. The context is primarily homework-related, with participants exploring the implications of molarity versus osmolarity.
Discussion Character
- Homework-related
- Debate/contested
- Mathematical reasoning
Main Points Raised
- One participant calculates the moles of solute using molarity and finds 3.49E-3 moles for 5.07 mL of 0.688 M Na3PO4.
- Another participant suggests that the calculation should consider osmolarity, which accounts for the total number of particles in solution, proposing that the moles of solute particles should be 1.40E-2.
- A participant expresses uncertainty about the correct approach, noting that their textbook did not cover osmolarity, and questions whether finding moles of solute would simply involve using molarity.
- Another participant clarifies that "moles of solute" refers to molarity, while "moles of solute particles" refers to osmolarity.
- One participant challenges the earlier calculations, suggesting that the actual concentration of dissolved entities is approximately 2.804 M due to the behavior of phosphate in solution, leading to a different estimate of moles.
Areas of Agreement / Disagreement
Participants do not reach a consensus on the correct method for calculating the moles of solute particles, with multiple competing views on the interpretation of osmolarity and the effects of chemical behavior in solution.
Contextual Notes
There are unresolved assumptions regarding the behavior of ions in solution and the definitions of molarity versus osmolarity, which may affect the calculations presented.
