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/sci/ - Science & Math

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12556735 No.12556735 [Reply] [Original]

Would this reaction also work in dilute solutions? Because I'm thinking of just dumping aqueous ammonia into an Ammonium Bicarbonate solution

>> No.12556876
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12556876

>>12556735
>by bubbling ammonia through an aqueous solution
>aqueous solution
Probably yes, just try it. You may want to use a more concentrated ammonia solution, but it still must be an aqueous solution to allow ions to move and for collisions and stuff to happen.

>> No.12556889

>>12556735
Why the fuck do you want to synthesize baking soda? You know its like a dollar a pound at the grocery store.

>> No.12556895

>>12556889
Baking soda uses sodium for the cation

>> No.12556900
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12556900

>>12556889

>> No.12556932

>>12556876
Yeah I was unsure about it because other sources said to use a strong solution, and I dont entirely understand how this reaction works.
Maybe they just noted that it should be a strong solution to make getting the salt out of solution easier, which im not really interested in I just need a solution of ammonium carbonate

>> No.12556981

>>12556932
Looks like the basic ammonia may attack the H+ in the (NH4)HCO3, which forms another ammonium ion (NH4+) which forms the final product with the NH4CO3- that lost the proton. So in other words, it really doesn't matter too much the strength of your ammonia solution, but it is somewhat soluble in water, so to separate it from the solution once the reaction is completed it will be more convenient to use a solution with less water so the water can be evaporated much faster (this will especially take longer since trying to speed up the evaporation via heating can decompose your product). You just need enough water to completely dissolve your ammonium bicarbonate, and then add a strong(ish, doesn't really matter too much) ammonia solution, and then evaporate the water to isolate the product (without heating). Should work fine.

>> No.12557001

>>12556981
Thanks!

>> No.12557011

>>12557001
no problem anon