NH4NO3+NaOH solution=NaNO3?

cool ,thanks!

Quote: Originally posted by AndersHoveland

I do not think there really is any minimal concentration if the solution is heated or boiled.

As long as your stoichiometry is correct, the reaction should carry to completion, as with most inorganic ion exchange reactions. Keep in mind however, that ammonia is soluble in water, meaning that if there is too much water, the ammonia will not gas off, and you'll have to heat the solution to get rid of the ammonia. Ammonia reacts with water to form NH4OH, if there is too much water, the ammonia will stay in solution as NH4+ and OH-, and your reaction will go nowhere.

If you hate the smell of ammonia as much as I do, this is not a reaction you will look forward to doing

When a dry, stoichiometric mixture of finely ground table salt and ammonium nitrate is heated slowly, NH₄Cl will slowly sublime and may be collected on a cooled receiver!
Temperature should be controlled to prevent fusion and when sublimation ceases the residue will consist of NaNO₃ plus whatever small amounts of anti-caking agent were used.
The NH₄Cl collected though, will be of fairly high purity!
Another route would be to boil a solution of NH₄NO₃/NaCO₃!
(NH₄₂CO₃ will be driven off and can be condensed as a concentrated solution.
You could use the sal volatile to revive your partner if, during energetic copulation, she should slip into unconsciousness, as they're sometimes wont to do!


[Edited on 28-12-2011 by hissingnoise]

Quote: Originally posted by hissingnoise

Another route would be to boil a solution of NH<sub>4</sub>NO<sub>3</sub>/Na[<sub>2</sub>]CO<sub>3</sub>! (NH<sub>4</sub><sub>2</sub>CO<sub>3</sub> will be driven off and can be condensed as a concentrated solution.

Quote:

Quote: Originally posted by hissingnoise   Another route would be to boil a solution of NH<sub>4</sub>NO<sub>3</sub>/Na[<sub>2</sub>]CO<sub>3</sub>! (NH<sub>4</sub><sub>2</sub>CO<sub>3</sub> will be driven off and can be condensed as a concentrated solution. What are you talking about?! Ammonium carbonate and bicarbonate (in case nerdalert226 would want to use NaHCO3 instead of Na2CO3) both decompose in hot water, never mind condensing and using them for who knows what.

Ooooh, you are, er, um, abominable, Mr Yeti, but thanks for correcting my wee error.
Washing soda is cheaper and more available than the hydroxide, in case you didn't know?
And 'sal volatile' does indeed decompose by heat; ((NH₄₂CO₃∙H₂O ---> 2NH₃ + CO₂ + 2H₂O).
You do understand the equation?
Distillation from solution should be carried out at ~80°C for best results . . .
BTW, White Yeti, have you lived a, how should I say, an 'unusually cloistered life', by any chance?

Quote: Originally posted by hissingnoise

Ooooh, you are, er, um, abominable, Mr Yeti, but thanks for correcting my wee error. Washing soda is cheaper and more available than the hydroxide, in case you didn't know?

Yes, I know washing soda is cheaper than hydroxide, not to mention more available. I didn't have sodium hydroxide until yesterday, when I made it from chalk and baking soda, I never thought I'd see the day, but it worked

Quote: Originally posted by hissingnoise

BTW, White Yeti, have you lived a, how should I say, an 'unusually cloistered life', by any chance?

It's all ahead of you - do you know how lucky you are?

Quote: Originally posted by hissingnoise

Another quick aside; since sal volatile (smelling salts) produces only small quantities of free ammonia, and the gas being toxic in quantity, sniffing smelling salts can improve performance in certain 'strenuous sports'!

Believe it or not, I've been trying to make NH₄HCO₃ for a while, and I haven't succeeded yet. It must have something to do with the salt's volatility. I neutralised household ammonia with unflavoured seltzer until the solution was mildly acidic. IIRC, I tested the solution for bicarbonate ions with a concentrated solution of CaCl₂ and the test was positive (turned cloudy).

I didn't try to mix carbonated water with CaCl₂ as a control (silly me) and I'm all out of seltzer

Anyway, I left the solution to evaporate over a heating vent and a few days later, I was left with a dull white powder that doesn't smell like anything, not even of ammonia when heated. The powder was probably the impurities in both the water and ammonia :\ Better luck next time.

If you were wondering what I was going to use it for, I was hoping to use it as fuel for hydrogen fuel cells. Since the salt releases ammonia when heated (apparently it also releases ammonia spontaneously), the salt could be used to store ammonia at room temperature, and the ammonia could be split to yield hydrogen.

I just came across this.
If you have a strong stomach you could try it!
And the 'working material' is something there'll never be a shortage of.

Quote: Originally posted by hissingnoise

I just came across this. If you have a strong stomach you could try it! And the 'working material' is something there'll never be a shortage of.

Some people think I'm crazy, but I'm not crazy enough to make compounds by using urine as a starting material I don't think I have the dedication to do such a thing, or the stomach for that matter.

Quote: Originally posted by White Yeti

......If you have a strong stomach you could try it! ......Some people think I'm crazy, but I'm not crazy enough............ I don't think I have the dedication to do such a thing, or the stomach for that matter.

Quote: Originally posted by dann2

Quote: Originally posted by White Yeti   ......If you have a strong stomach you could try it! ......Some people think I'm crazy, but I'm not crazy enough............ I don't think I have the dedication to do such a thing, or the stomach for that matter. It's a great big bladder you need, no need for a stomach (strong or otherwish) at all.

You need a strong stomach not to throw up when dealing with the fumes emanating from stale urine