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Preparation & properties of Ammonium phosphates (ammonium salts of orthophosphoric acid)
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- Опубликовано: 14 сен 2015
- Music: Hypnothis by Kevin MacLeod is licensed under a Creative Commons Attribution license (creativecommon...)
Source: incompetech.com...
Artist: incompetech.com/
good demonstration. simple, clear, professional.
I am interested in making Triammonium phosphate to combine with MgO to make Magnesium Phospate cement. I can access phosphoric acid and ammonia so this might be the go but if i mix in larger quantities, say 10 liters at a time, how much would i be able to dilute the reagants by and still get the reaction without the risk of blowing myself up? Your video was very clear and helpful, thankyou.
Please make a video diammonium phospate . Please
Hi Shiva Chemist i have a question,
Is this the same as smelling salts they are selling on amazon these days?
Thanks in advance for the answer.
please i have a question, on this preparation do you need drying to get the crystal?
Sir do you have any related studies or literature that I can use for this
Shiva chemist, could you please explain the stoichiometry. As per my understanding in the formation of MAP, the molar ratio of the two reactants should be 1:1. Could you please show if the molar ratio of the reagents you used (ie, 1.9 mL of ammonium hydroxide for every 1 mL of phosphoric acid) accounts to 1:1?
thanks
Yes, in this case both reactants are liquids. So, density will come into play. Also, the concentration of each liquid is different as well.
To find out the stoichiometric ratio for these reactants, you have to calculate 1M for both separately.
1M NH4OH = Molecular mass/density = 35/0.9 = 38.88
38.88/concentration (30%)*100 = 129.62
Similarly to prepare 1M Phosphoric acid = 98/1.68 = 58.33/85*100 = 68.62
Now to find out the ratio: = 129.62/68.62 = ~1.9
So, they are in the ratio = 1:1.9
Hope this is clear.
thanks alot
As you explained here, in the first step you divide mass/density which give you units of volume.
In the second step you divide volume/concentration(which is volume/(mass/volume)) which gives you units of sq. volume per mass
How is this dimensionally correct?
kindly explain
Well, there is a difference between density and concentration. Density concerns both solute and solvent whereas concentration is about how much solute dissolved in a solvent. Different substances with same concentration have different densities. What we are doing here is molar concentration of a substance. Here it gives you an amount of substance needs to be added to prepare a molar solution of desired quantity. More the concentration lesser the substance you need to dissolve and vice versa. Here we know the mass of a substance when it is in 100% concentration and we are making a molar solution of a liquid with available concentration. Hope this is clear.
+Shiva Chemist Do you have any idea about how quick does triammonium phosphate release all of its ammonia to form diammonium phosphate?
+ChemicalMaster
Definitely the conversion is not fast. It will take a while. If you store it properly in a tightly sealed container, sure, it will be fine for some months.
Shiva Chemist Alright, but if leave it outside how many time does it take to be completely converted? More or less, one week?
+Shiva Chemist And by the way, does triammonium phosphate solution also decompose into ammonia and diammonium phosphate?
Hi Shiva Chemist. This reaction that you shown MAP fertilizer - monoammonium phosphate - NH4H2PO4 + H2SO4 = (NH4)HSO4 + H3PO4 is it possible to distill this solution to get phosphoric acid?
I need K2HPO4 ( Dipotassium phosphate ) so i was thinking to react H3PO4 + 2 KOH → K2HPO4 + 2 H2O. Or is another way to prepare K2HPO4?
Thanks.
hello did you find it?
@@khadijachouni7973 Yes I did.
I used KOH + MAP . You will get lot of ammonium gas that need to be boiled off and then you get K2HPO4. You first react MAP with KOH stoichiometric ratio to get mono potassium phosphate and then heat slowly to boil of all ammonium gas
(do not boil of liquid, just heat it until all start to boil) and then react with more KOH to get dipotassium Phosphate.
Do it all outside because of ammonium gas.
Both KOH and MAP are first dissolved in water, than you slowly adding KOH solution into MAP solution (all cold). Try first on small scale.
I am amateur, that's how I did it.
I prepared KH2PO4 with simple reaction of KOH and H3PO4 , I want to know if it can also prepared by 2 KOH + H3PO4 ?!
@@khadijachouni7973 Yes, when you react 2KOH you get DI potassium phosphate and with 1KOH monopotassium phosphate
en.wikipedia.org/wiki/Dipotassium_phosphate
From that page you have also reaction with KCl
H3PO4 + 2 KCl → K2HPO4 + 2 HCl
Also Monopotassium phosphate is produced by the action of phosphoric acid on potassium carbonate.
@@klokoloko2114 Bonsoir, j'ai effectuée la synthèse de KOH+ H3PO4 et j'ai obtenu le KH2PO4 , mais lorsque j'ai réagi 2KOH avec H3PO4 j'ai pas obtenu le précipité et je ne sais pas pourquoi?
+Shiva Chemist By the way, are the 3 ammonium phosphates hygroscopic or deliquescent?
+ChemicalMaster
Not sure. But Ammonium dihydrogen phosphate is neither hygroscopic nor deliquescent. Because, the crystals of it are still sitting fine in a watch glass.
hi.shiva chemist ,tank's for this can I do that reaction from phosphoric acid green (not pure) ?
Of course, you can. But, the resulting compound will not be pure.
Hi shiva chemist , I want convert (NH4)2HPO4 to NH4H2PO4 .What I do
How to make H2PO4 or (NH4)H2PO4? or how to convert phosphoric acid to ammonium phosphate, diammonoum phosphate or Monoammonium phosphate? plz help with this. Thanks
+Ahsan Khan
You mean H3PO4? I've explained all these in this video. Didn't you watch it? If not, please do.
+Ahsan Khan
You are welcome. Fine, but you didn't get me I think. Orthophosphates or phosphates are salts of Phosphoric acid. Orthophosphoric acid is just the other name of phosphoric acid (H3PO4). You asked me how to prepare ammonium phosphate (triammonium phosphate - (NH4)3PO4), diammonoum phosphate (diammonium hydrogen phosphate -(NH4)2HPO4 or Monoammonium phosphate (ammonium dihydrogen phosphate-NH4H2PO4). I've shown how to prepare all these three in this video. Hope this is clear. Please let me know otherwise.
+Shiva Chemist Can we get H2PO4 from Phosphoric acid without reaction with ammonia? any easy and less riskful way to do it on large scale? for example making a solution of 100 litre or 100kg?
+Ahsan Khan
You can use ammonium carbonate solution but it will give off so much carbon dioxide. CO2 can be expelled by heating up the solution but you will lose some ammonia by that way. The neutralization reaction between phosphoric acid and ammonia is highly exothermic, so you should dilute both reagents before mixing them carefully. It will mitigate the danger.
+Shiva Chemist can we also get H2PO4 by adding 5% hydrogen per oxide in phosphoric acid? Thanks once again for answering all that questions.
how fucking acidic too because i got some in my eye, is the burning just in my head ?
Most chemicals will cause mild to severe irritation when they come in contact with your eyes, in worst cases, you may even lose your eye sight. But, do not worry, ammonium phosphate is not that dangerous. Wash your eyes with copious amount of water. Check with the nearby doctor if this problem persists.
Shiva Chemist thanks im ok now
how dangerous is this ammonium phosphate shit because im covered in it.
***** thank you for the info. i did survive and have moved on too more dangerous substances.