Question

A solution contains AgNO3 and Ba(NO3)2. What substance could be added to the solution to precipitate Ag+ ions, but leave Ba2+ ions in solution? NaNO3 Na2SO4 NaCl After removal of the Ag+ compound, what could then be added to the solution to precipitate the Ba2+ ions? NaNO3 Na2SO4 NaCl

Answer 1

To precipitate Ag+ ions and leave Ba2+ ions in solution, NaCl should be added to form AgCl. Subsequently, to precipitate Ba2+ ions, Na2SO4 is used to form BaSO4.

Step-by-step explanation:

To precipitate Ag+ ions while keeping Ba2+ ions in solution, a compound that forms an insoluble salt with Ag+ but not with Ba2+ needs to be added. The suitable substance from the given options is NaCl, which will form AgCl, a precipitate, while leaving the Ba2+ ions in solution.

After the removal of the Ag+ precipitate, to precipitate Ba2+ ions, a solution that forms an insoluble salt with Ba2+ should be added. Na2SO4 would be added to the remaining solution to form BaSO4 as a precipitate. Therefore, the correct choices to precipitate these ions are NaCl first for Ag+ and Na2SO4 next for Ba2+.

Answer 2

It uses sodium nitrate, so that the nitrate group reacts with silver and precipitates as a salt, thus forming silver nitrate

And as for the precipitation of barium, I would use sodium sulfate, since we would use the nitrate group, barium nitrate would form, which is very dangerous and is considered high risk.

Step-by-step explanation:

All the compounds that we name are reactions where as a product they give salts that are highly complex, where they are solid at room temperature, precipitate and are whitish in color.

These salts so that they precipitate it is important that they are in supersaturation since otherwise they will be in constant dynamism dissolving with the water, since they are soluble in them and the decantation will not be perceived at the naked eye of the human eye.