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Ammonium Chloride sublimes when heated whereas Barium Sulfate does not. Another method would be to add de-ionized water to the mixture. The solids left over will be the Barium Sulfate whereas the the Ammonium Chloride will be mixed with the de-ionized water. Weigh everything first, including the water because the Ammonium Chloride will sublime when dry if you try to evaporate the de-ionized water from the mixture.
BaF2 - Barium fluoride
Barium sulphate to barium sulphate is NO CHANGE!
Barium sulfate is thermally decomposed in barium oxide and sulfur trioxide.
since both substance will dissolve, the barium and the sulfate will come together and barium sulfate does not dissolve in water so barium sulfate will be the precipitate.
Ammonium sulfate reacts with barium nitrate to form ammonium nitrate and barium sulfate. (NH4)2SO4 + Ba(NO3)2 ==> 2NH4NO3 + BaSO4 It is a double replacement reaction. that is the correct answer
(NH4)2SO4(aq) + BaCl2(aq) → 2NH4Cl(aq) + BaSO4(s). Barium sulfate is the precipitate.
Barium fluoride is BaF2.Sodium oxides are Na2O, Na2O2, NaO2.
Ba2+ + CO32- >> BaSO4
Add water and pass it though a filter. Ammonium sulfate will dissolve in water, barium sulfate will not.
The equation is:Ba+ + (SO4)2- = BaSO4(s)
(NH4)2SO4 + Ba(NO3)2 -> BaSO4 + 2NH4NO3
Ammonium Chloride sublimes when heated whereas Barium Sulfate does not. Another method would be to add de-ionized water to the mixture. The solids left over will be the Barium Sulfate whereas the the Ammonium Chloride will be mixed with the de-ionized water. Weigh everything first, including the water because the Ammonium Chloride will sublime when dry if you try to evaporate the de-ionized water from the mixture.
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BaF2 - Barium fluoride
Salts: sodium chloride, barium nitrate, uranyl acetate, plutonium sulfate, ammonium phosphate etc.
If you treat an unknown sample with ammonium sulfate (or any other soluble sulfate) and get a precipitate, you can conclude that there's a metal ion which forms insoluble sulfates in it. (Pretty much all ammonium salts are soluble, so you don't need to worry about the anion.)