2HNO3+2Ag=2AgNO3+h2 the pecipitate AgNO3 is white in colour like yoghurt or curd
Ag is going to exist in nature as Ag2--no doubt about it. The actual reaction with carbonate is 2AgNO3 (silver nitrate) + Na2CO3 (sodium carbonate) = Ag2CO3 (silver carbonate) plus NaNO3. For some reason you get elemental silver out of this too--which you shouldn't because it's a balanced equation, but Ag2CO3 is yellowish and it's normally got gray flecks in it when you get it.
Silver = Ag+1 Carbonate = CO3-2 Formula is: Ag2(CO3)
Chloride ion (Cl-) will not precipitate silver ion (Ag+) because silver chloride (AgCl) is insoluble and will not form a precipitate.
Yes, a precipitate will form when silver ions (Ag^+) react with oxalate ions (C2O4^2-) to form silver oxalate (Ag2C2O4), which is insoluble in water. This insoluble compound will precipitate out of solution.
The formula for silver carbonate is Ag2CO3. It consists of two silver (Ag) ions and one carbonate (CO3) ion.
Silver = Ag+1 Carbonate = CO3-2 Formula is: Ag2(CO3)
The combination of ions least likely to produce a precipitate is those that form a soluble salt when combined. For example, ions like Na+ and Cl- are unlikely to produce a precipitate when combined because NaCl is soluble in water and remains in solution. Conversely, ions that form insoluble salts when combined, like Ag+ and Cl-, are more likely to produce a precipitate.
The ionic equation between halides and silver nitrate involves the cation from silver nitrate combining with the anion from the halide compound to form a precipitate. For example, with chloride ions, Ag^+ from silver nitrate reacts with Cl^- from the chloride compound to form solid silver chloride (AgCl) precipitate. The net ionic equation would show the formation of the silver halide precipitate.
Ag is going to exist in nature as Ag2--no doubt about it. The actual reaction with carbonate is 2AgNO3 (silver nitrate) + Na2CO3 (sodium carbonate) = Ag2CO3 (silver carbonate) plus NaNO3. For some reason you get elemental silver out of this too--which you shouldn't because it's a balanced equation, but Ag2CO3 is yellowish and it's normally got gray flecks in it when you get it.
Silver = Ag+1 Carbonate = CO3-2 Formula is: Ag2(CO3)
Chloride ion (Cl-) will not precipitate silver ion (Ag+) because silver chloride (AgCl) is insoluble and will not form a precipitate.
It's called a 'precipitate'Example:(solution of) Ag+ + (solution of) Cl- ==> (precipitate) AgCl This is a white, cloudy suspension of tiny particles, called 'precipitate'
Yes, a precipitate will form when silver ions (Ag^+) react with oxalate ions (C2O4^2-) to form silver oxalate (Ag2C2O4), which is insoluble in water. This insoluble compound will precipitate out of solution.
One mole of chloride (Cl-) to one mole of Ag+ ions: Cl- + Ag+ --> AgCl(s)
Of course; the reaction is: Ag+ + NO-3 + Na+ + Cl- = Na+ + NO-3 + AgCl Silver chloride is a white precipitate, very insoluble in water.
Since silver carbonate dissociates into two silver ions for each carbonate ion, by definition its solubility product constant is the product of [Ag+1]2 and [CO3-2], and (assuming that there is no other source of carbonate ions present], [CO3-2] = [Ag+1]/2. Therefore, in this instance, Ksp = (2.6 X 10-4)3/2 = 8.8 X 10-12.
The reaction is:Ag+ + Cl- = AgCl(s)Silver chloride is an insoluble, white, photosensitive precipitate.