November 16, 2019, 05:34:48 PM
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Topic: Amonium hydroxide solution  (Read 601 times)

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Offline pdhrati

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Amonium hydroxide solution
« on: March 12, 2019, 12:21:39 PM »
Hello, I need to make ammonium hydroxide solution (1M). Can anyone help me with what would be the best way of doing that (Any method other than using gas!)? Can I make it using ammonia (Powder form)? If yes how?
Thanks in advance

Offline AWK

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Re: Amonium hydroxide solution
« Reply #1 on: March 12, 2019, 01:03:41 PM »
Concentrated (~28 %) aqueous ammonia solution is a common cheap chemical reagent.
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Offline chenbeier

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Re: Amonium hydroxide solution
« Reply #2 on: March 12, 2019, 02:05:03 PM »
Hello, I need to make ammonium hydroxide solution (1M). Can anyone help me with what would be the best way of doing that (Any method other than using gas!)? Can I make it using ammonia (Powder form)? If yes how?
Thanks in advance

If you dont aware other ions in the solution then dissolve 1 mol ammonium chloride and 1 mol sodium hydroxide  per liter.

Offline mjc123

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Re: Amonium hydroxide solution
« Reply #3 on: March 13, 2019, 05:53:08 AM »
That will give you sodium chloride solution and generate ammonia gas.

Offline AWK

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Re: Amonium hydroxide solution
« Reply #4 on: March 13, 2019, 07:01:34 AM »
That will give you sodium chloride solution and generate ammonia gas.
Solutions of NH4Cl and NaOH when they react with each other, practically do not evolve heat. Ammonia is good soluble even in highly concentrated NaCl (see Solvay process) so Chenbeier method will not produce the gaseous ammonia without warming. But this form mixture of NaCl and ammonia in water.
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Offline Babcock_Hall

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Re: Amonium hydroxide solution
« Reply #5 on: March 13, 2019, 11:01:04 AM »
Wouldn't the easiest way be to dilute the commercial reagent?  I am old enough to remember a convenient table in The Chemist's Companion.  Or is there a reason not to do so?  After reading the OP, I am not sure.

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