Solubility-Pressure graph of Ammonia

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Discussion Overview

The discussion revolves around the solubility of ammonia (NH3) in water as it relates to pressure, with participants exploring how pressure influences this solubility compared to temperature effects. The conversation includes references to relevant laws and empirical data.

Discussion Character

  • Exploratory
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant notes difficulty in finding information on how ammonia's solubility changes with pressure, despite available data on temperature effects.
  • Another participant questions the assumption that ammonia, being a gas, would have significant solubility variation with pressure, suggesting a review of Henry's law for clarity.
  • A participant provides data indicating that at 0°C, ammonia's solubility in water is 90% by mass, while at 72°C, it becomes almost insoluble, linking solubility to temperature rather than pressure.
  • One participant emphasizes that while ammonia is a gas at room temperature, its behavior under varying pressures is uncertain, particularly due to its reaction with water.
  • A later reply references Henry's Law, indicating that while ammonia's solubility does change with pressure, the extent of this change is reportedly low according to an expert consulted by the participant.

Areas of Agreement / Disagreement

Participants express differing views on the extent to which pressure affects ammonia's solubility, with some suggesting minimal impact while others propose that it could vary significantly. The discussion remains unresolved regarding the precise relationship between pressure and solubility.

Contextual Notes

Participants reference empirical data and theoretical frameworks, but there are limitations in the assumptions made about gas behavior and the specific conditions under which solubility is measured.

pranj5
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I have searched to find out how the solubility of Ammonia changes with pressure, but haven't been able to find out. Though data about solubility change with temperature is available. One have told me that solubility of Ammonia varies little with pressure. But, I want to be assured about that. Can anybody help me?
 
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Isn't NH3 a gas normally? If so, I would imagine the solubility to vary wildly with pressure, but I don't know.

Maybe take a look at Henry's law and see if that helps: https://en.wikipedia.org/wiki/Henry's_law, http://www.henrys-law.org/henry-3.0.pdf
 
Last edited:
The critical temperature of Ammonia is 132.4°C and that means at ambient temperature and pressure it wouldn't act like a gas. At 0°C, the solubility of Ammonia in water (by mass) is 90% while at 72°C, it's almost insoluble.
 
pranj5 said:
The critical temperature of Ammonia is 132.4°C and that means at ambient temperature and pressure it wouldn't act like a gas. At 0°C, the solubility of Ammonia in water (by mass) is 90% while at 72°C, it's almost insoluble.

Okay? The boiling point is -30 something C. It's a gas at room temperature. Do you mean it doesn't behave like an ideal gas? No gases do. Solubility of gases decrease with increased temperature, so that sounds legit.

Because NH3 reacts with water, I'm not sure if differing gas pressures would cause solubility to change... but it might. I'll let the others here answer.
 
As per Henry's Law, solubility of different gases to water is different. I don't want to mean that solubility of Ammonia to water at different pressure doesn't change at all. But, as per an expert with whom I have talked about it a few days ago, told me that it's very low.
 

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