What products are formed when aluminum nitrate is mixed with ammonium hydroxide?
341863
ammonium nitrate and aluminum hydroxide\n\nNH4NO3 + Al(OH)3\n\nThe aluminum hydroxide is insoluble when formed and will precipitate out of the solution as a solid powder.
864694
Tin floride\nAmmonium sulfate\nMagnesium hydroxide\nBarium carbonate\nSodium sulfate\nCarbon chloride
572470
a.  4H20 + 4NO2 + 02--------->4HNO3 + 2 H2O\n      Al(OH)3+ 3HCl------------> AlCl3+ 3H2O\nb. not sufficient as Al(OH)3 is 12/78 moles which is able to react with .462 moles of HCl and here we have .9444 moles of HCl\n\n9. it is done by equilliberium reaction\n and u written Na reaction with H2 to form hydride
314441
The chemical compound ammonium nitrate\nNH4 NO3
290908
http://www.eacochem.com/lc_aluminumcleaning.shtml
860022
Here are the formulas:\n\nAluminum Hydroxide = Al(OH)_3\nSulfuric Acid = H_2SO_4\nWater = H_2O\nAluminum Sulfate = Al_2(SO_4)_3\n\nThe correct balanced equation is:\n\n2[Al(OH)_3] + 3[H_2SO_4] + → Al2(SO_4)_3 + 6[H_2O]
105132
3 Sn(NO3)4 + 4 AlCl3 --> 4 Al(NO3)3 + 3 SnCl4
168132
Making of Fertilizers:\nBasically, fertilizers are made from ammonia..I will take you through four stages that are basically followed in order to make ammonia..mind it that I am talking about artificial fertilizers not natural ones like cow dung which is not man-made...Alright then,\n\nSTAGE 1: Haber Process\n\nThis is a reversible reaction and an exothermic reaction thats used to make Nitrogen and Hydrogen under low temperatures (about 750 degrees celcius) and high pressures (about 30 atmospheres with a catalyst of nickel)..The reaction for this equation is:\n\nN2 + 3H2 <---> 2NH3  (-92kJmol -1)\nNitrogen + Hydrogen <---> Ammonia\n\nNow we have got our ammoina..which is the raw material in the production of fertilizers..Lets move on to the 2nd step...\n\nSTAGE 2: Ammonia being converted into Nitrogen Monoxide..\n\nIn this stage, we are going to let ammonia (which we got from the Haber process) react with oxygen to form nitrogen monoxide and water..\nFor this reaction to take place..we need to apply heat and catalyst (not so sure of which catalyst). We need to apply 230 degrees celcius of heat for heating air and ammonia). So, here's the reaction equation for that:\n\n4NH3(g)  +  5O2(g)  --->  4NO(g)  +  6H20(l)\n\nWe've got our Nitrogen monoxide now..so let's move on..\n\n\nSTAGE 3: Converting Nitrogen Monoxide into Nitric Acid\n\nIn this reaction we are going to react Nitrogen Monoxide with Oxygen and Steam to obtain Nitric Acid like this:\n\n4NO(g) + 3O2(g) + 2H2O(g) ---> 4NO3(aq)\n\nSTAGE 4: Converting this Nitric Acid into Ammonium Nitrate\n\nSo, Now nitric acid is going to be reacted with Ammonia (from Haber Process again..) in an addition reaction. Ammonium Nitrate in this case, will be our fertilizer..So, this is the final stage.. <Phweks!!> Here we go:\n\nNH2(g)  +  HNO3(aq)  --->  NH4NO3(aq)\nAmmonia gas + Nitric Acid ---> Ammonium Nitrate!!!\n\n\nUses:\nThe ions these fertilizers contain enrichen the soil very much..Ions like the nitrates and phosphates are absorbed by the plants through osmosis from the soil..These ions then help the plant in various stuff like synthesising the chlorophyll molecule..some like nitrates are converted into plant proteins...\n\nOk, I guess I have exhausted everything I know about fertilizers...\n\nI really hope it was of some help for u...   :)
799604
If the ionic compound is soluble, no precipitate is formed.\n\nOn the other-hand, if an ionic compound is not very soluble in the solvent, then it will precipitate out of solution.\n\nFor example, Sodium chloride is soluble and Silver nitrate is soluble, but if these solutions are mixed, some of the Silver ions will react with chloride ions and form solid Silver chloride precipitate.
823469
All nitrates are soluble.  You would need to consult a table of solubilities to see what other ions you could use to precipitate out the cations.\n\nEx:  If you had silver nitrate in a solution you could add something with a halide ion such as sodium chloride.  The silver ion would precipitate out with the chloride ion.  If no ppt forms with the sodium chloride you know it was not silver ions.\n\nThen look for other ions that you could test for.
625685
Aluminium has a valanly of 3 Oxgygen has 2\nSo\n4Al + 3O2   -> 2Al2O3
971239
When the two solutions are mixed, you'll get a bright yellow precipitant.\n\nPb(NO3)2 + 2 NaI ---> PbI2 + 2 NaNO3
471526
I suspect that the product is AlSO4.\n\nI'm thinking that the Al swaps with the Cu.  That would leave a free Cu+ which might displace the H from H20 and form either CuOH or CuO, either one of which would probably produce H2.  \n\nSo, I guess you would first get CuOH and AlOH, as intermediate reactions.\n\nI think the equation is:\n\n                          NaCl (goes over the arrow)\n6CuSO4 + 4Al + 12H2O ---------------> 2Al2(SO4)3 + 6Cu(OH)2 + 6H2
890642
Al + Fe(NO3)3 ---> Al(NO3)3 + Fe.\n\n2K + 2H2O ---> 2KOH + H2\n\n2KOH + CuSO4 ---> Cu(OH)2 + K2SO4\n\n3NaOH + H3PO4 ---> 3H2O + Na3PO4\n\nBest?
838903
This is just an acid-base reaction.  The nitrogen lone pair acts as a Lewis base and takes the HCl proton.  You then have a quaternary ammonium cation and a chloride anion.  This will form the salt shown as answer b.
604455
Mix solution of (phosphoric acid/nitric acid/acetic acid) can be used to clean the settlement on aluminium composite surface.
216099
Yes if you react NH4NO3(aq) with something SO4 you can make it.