Cu (I): CN-

Pb2+: CN-, SO3^2-, PO3^3-,MnO4-
Ca2+: CN-
Al3+: CN-, SO3^2-, PO3^3-,MnO4-
Cr5+: CN-, SO3^2-, PO3^3-,MnO4-
Pb4+: CN-
Sn2+: CN-
Mn2+:MnO4-
Ag+:CN-, SO3^2-, PO3^3-
H+: CN-, SO3^2-, PO3^3-,MnO4-

Doesn't tell me a thing.

molarity of 474 mL solution containing 21.1 g of potassium iodide

In this question, you have been given a list of ions and their corresponding possible ligands. Your task is to determine which ligands can form stable complexes with each ion.

To determine the stable complexes, we need to consider the charge and the size of the ions. Here are the steps to figure out the stable complexes for each ion:

1. Cu2+ (Copper): The Cu2+ ion has a charge of +2. CN- (cyanide) has a charge of -1. Since the charges are opposite and equal in magnitude, Cu2+ can form a stable complex with CN-.

2. Pb2+ (Lead): Pb2+ has a charge of +2. CN- has a charge of -1, SO3^2- (sulfite) has a charge of -2, PO3^3- (phosphite) has a charge of -3, and MnO4- (permanganate) has a charge of -1. Out of these ligands, only CN- can form a stable complex with Pb2+ due to the matching charge.

3. Ca2+ (Calcium): Ca2+ has a charge of +2. CN- has a charge of -1. Just like with Cu2+, Ca2+ can also form a stable complex with CN-.

4. Al3+ (Aluminum): Al3+ has a charge of +3. Similar to Pb2+, CN- has a charge of -1, SO3^2- has a charge of -2, PO3^3- has a charge of -3, and MnO4- has a charge of -1. Again, only CN- can form a stable complex with Al3+ due to the matching charge.

5. Cr5+ (Chromium): Cr5+ has a charge of +5. CN- has a charge of -1, SO3^2- has a charge of -2, PO3^3- has a charge of -3, and MnO4- has a charge of -1. None of these ligands have charges that can match the charge of Cr5+, so there would be no stable complex formed.

6. Pb4+ (Lead): Pb4+ has a charge of +4. Only CN- has a charge of -1, so it can form a stable complex with Pb4+.

7. Sn2+ (Tin): Sn2+ has a charge of +2. As we have established earlier, CN- can form a stable complex with ions having a charge of +2, so it can form a stable complex with Sn2+.

8. Mn2+ (Manganese): Mn2+ has a charge of +2. Among the provided ligands, only MnO4- has a charge of -1. Hence, Mn2+ can form a stable complex with MnO4-.

9. Ag+ (Silver): Ag+ has a charge of +1. CN- has a charge of -1, SO3^2- has a charge of -2, and PO3^3- has a charge of -3. Among these, only CN- has a matching charge, making a stable complex with Ag+.

10. H+ (Hydrogen): H+ has a charge of +1. Similar to Cu2+, Ca2+, and Ag+, CN- can form a stable complex with H+ due to the matching charge.

In summary, the stable complexes for each ion are as follows:
- Cu2+: CN-
- Pb2+: CN-
- Ca2+: CN-
- Al3+: CN-
- Cr5+: None
- Pb4+: CN-
- Sn2+: CN-
- Mn2+: MnO4-
- Ag+: CN-
- H+: CN-

Remember that this explanation is based on the provided information and may vary depending on the specific chemical properties and conditions involved.