Questions regarding the role of chloride ions in the decomposition of nitroammonium
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This post was last edited by carlcjb on 2010-5-21 16:37. I want to design an experiment: Use about 60% nitric acid along with solid ammonium chloride for vacuum distillation, in order to evaporate the hydrochloric acid from the system and leave behind an aqueous solution of ammonium nitrate. This aqueous solution can then be concentrated and cooled to induce crystallization, thereby obtaining solid ammonium nitrate! However, while researching, I found that chloride ions accelerate the decomposition of ammonium nitrate, and it may even explode. I am not very familiar with this industry, so I would like to ask for advice from those who are more knowledgeable! 1. Can this experiment be carried out? Why? 2. If it can be done, what is the maximum temperature allowed? 3. Are there any similar production devices in industrial manufacturing? Or is there any feasibility for industrialization?
If you want to conduct this experiment, you need to determine whether there are heavy metal ions in your solution.
My friend, what’s still a bit unclear is this: heavy metal ions will definitely be present to some extent! But to what level should heavy metals be controlled? Furthermore, which heavy metal ion has the greatest impact on this reaction?