You are given a solution that contains one of the ions Ag+, Pb2+ or Ba2+. Develop a procedure to determine which ion is present. More than one reaction may be required to discover the ion’s identity. Explain how your procedure will determine the identity of the ion.

Well, let's play a little game with these ions to figure out who's who. First, let's add a little bit of hydrochloric acid (HCl) to the solution. If we see a white precipitate forming, then we know it's not Ag+ because silver chloride is insoluble and will show up as a precipitate.

Next, let's add some sodium sulfate (Na2SO4) to the solution. If a yellow precipitate forms, we can confidently eliminate barium (Ba2+) from the equation because barium sulfate is insoluble.

Finally, if none of the previous tests gave any precipitates, we can conclude that we're dealing with the lead ion (Pb2+). To confirm this, we can add some potassium iodide (KI) solution. If a bright yellow precipitate forms, then it's definitely lead (PbI2).

So, in summary, we're looking for the white precipitate of silver chloride for barium, the yellow precipitate of barium sulfate for barium, and the bright yellow precipitate of lead iodide for lead. It's just a chemical game of hide and seek, but we'll catch that sneaky ion eventually!

To determine the identity of the ion in the given solution (Ag+, Pb2+, or Ba2+), we can use a series of selective chemical reactions that produce distinct precipitates for each ion. Here's a step-by-step procedure:

1. Test for Ag+:
- Add a few drops of dilute nitric acid (HNO3) to the solution to remove any carbonates or sulfides that could interfere with the test.
- Add a few drops of sodium chloride (NaCl) solution to the solution containing the ions.
- If a white precipitate forms, it indicates the presence of Ag+ ions, as silver chloride (AgCl) is insoluble in water.

2. If there was no precipitate formed in step 1, we move on to test for Pb2+:
- Add a few drops of dilute sulfuric acid (H2SO4) to the solution to remove any carbonates or sulfides.
- Add a few drops of potassium iodide (KI) solution to the solution containing the ions.
- If a bright yellow precipitate forms, it indicates the presence of Pb2+ ions, as lead iodide (PbI2) is insoluble in water.

3. If there was no precipitate formed in step 2, we move on to test for Ba2+:
- Add a few drops of dilute sulfuric acid (H2SO4) to the solution to remove any carbonates or sulfides.
- Add a few drops of sodium sulfate (Na2SO4) solution to the solution containing the ions.
- If a white precipitate forms, it indicates the presence of Ba2+ ions, as barium sulfate (BaSO4) is insoluble in water.

By systematically performing these tests, we can identify the ion present in the solution based on the specific precipitate formed. If none of the tests result in a precipitate, it suggests the absence of Ag+, Pb2+, and Ba2+ ions in the solution.

To determine the identity of the ion present in the solution (Ag+, Pb2+, or Ba2+), you can follow a series of tests or reactions to narrow down the possible options. Here is a step-by-step procedure to determine the ion's identity:

1. Test for Ag+:
a. Add a few drops of dilute nitric acid (HNO3) to a small portion of the solution.
b. If a white precipitate forms, it indicates the presence of Ag+ ions. Proceed to confirm the presence of Ag+ ions using the next step.
c. Add a few drops of dilute ammonium hydroxide (NH4OH) to the solution from step 1b.
d. A dark brown precipitate (Ag2O) confirms the presence of Ag+ ions.

2. Test for Pb2+:
a. Add a few drops of dilute hydrochloric acid (HCl) to a small portion of the solution.
b. If a white precipitate is formed, it suggests the presence of Pb2+ ions. Proceed to confirm Pb2+ ions using the next step.
c. Add a few drops of dilute sulfuric acid (H2SO4) to the solution from step 2b.
d. A yellow precipitate (PbSO4) indicates the presence of Pb2+ ions.

3. Test for Ba2+:
a. Add a few drops of dilute sulfuric acid (H2SO4) to a small portion of the solution.
b. If a white precipitate forms, it suggests the presence of Ba2+ ions. Proceed to confirm Ba2+ ions using the next step.
c. Add a few drops of dilute hydrochloric acid (HCl) to the solution from step 3b.
d. A white precipitate (BaSO4) confirms the presence of Ba2+ ions.

By performing these tests sequentially, you can determine the identity of the ion present in the solution. If a precipitate forms and matches the expected compound for a particular ion, it confirms the presence of that ion. If none of the tests produce a precipitate, it means that none of the tested ions (Ag+, Pb2+, Ba2+) are present in the solution.

To write a procedure you really need to know the solubility tables. You can go to Google to find that table. Then you should memorize it. Here is a procedure that will work.

To the sample, add a few drops of AgNO3. No ppt means Ba ion is present. A white ppt means either Pb ion or Ag ion (or both) are present as AgCl or PbCl2. Let the ppt settle and decant the liquid. Divide the ppt into two parts. To one part add hot water. If the white ppt dissolves it is Pb^2+ because PbCl2 is soluble in hot water. To the other part add dilute aqueous NH3. If it dissolves it is Ag^+ because AgCl in the presence of NH3 form a complex ion of [Ag(NH3)2]^+ which is soluble. That, in summary, is the procedure for group I of an analytical procedure for qualitative analysis of an unknown. If you take much chemistry you should become familiar with that.