Question

You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO₃, BaCl₂, or MgSO₄. a friend suggests that you test a portion of the solution with Ba(NO₃)₂ and then with nacl solutions. part a according to your friend’s logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle?

O silver chloride could precipitate.
O silver sulfate could precipitate.
O barium sulfate could precipitate.
O more than one, but not all, of the reactions described above could occur.
O all three reactions described above could occur.

Answer 1

Only the precipitation of silver chloride (AgCl) is guaranteed when adding Ba(NO3)2 and NaCl to the solution. Precipitation of barium sulfate (BaSO4) is not possible with given reagents,

Step-by-step explanation:

According to your friend's logic, when testing the unlabeled aqueous solution with Ba(NO3)2 and then with NaCl solutions, the following reactions could occur:

• If the solution contains AgNO3, then AgCl could precipitate when NaCl is added because AgCl is insoluble.
• If the solution contains BaCl2, then AgCl could precipitate when AgNO3 is added for similar reasons.
• If the solution contains MgSO4, no reaction will occur with the addition of Ba(NO3)2 because both barium and magnesium sulfates are soluble.

Therefore, the chemical reactions described above that could occur and help identify the solution are the precipitation of silver chloride (AgCl) and potentially, but not necessarily, barium sulfate (BaSO4) depending on the various combinations of reagents.

This indicates that "more than one, but not all, of the reactions described above could occur" is the correct response.