Lead metal is added to 0.100M Cr3+(aq)

Pb(s) + 2Cr3+(aq) -> Pb2+(aq) + Cr2+(aq)

What is [Pb3+] when equilibrium is reached?
What is [Cr2+] when equilibrium is reached?
What is [Cr3+] when equilibrium is reached?

any help is appreciated

Do an ICE chart.

Let me know what you don't understand if you get stuck on that.

To determine the concentrations of ions at equilibrium, we need to use the balanced chemical equation and the concept of stoichiometry. Here's how you can approach each question:

1. What is [Pb3+] when equilibrium is reached?
Given the balanced equation: Pb(s) + 2Cr3+(aq) -> Pb2+(aq) + Cr2+(aq), we can see that for every 1 mole of Pb(s) that reacts, 1 mole of Pb2+(aq) is formed. Therefore, at equilibrium, the concentration of [Pb2+] will be equal to the concentration of [Pb3+]. To find the concentration of [Pb3+], you need to determine the equilibrium concentration of [Pb2+] or assume it is the same as the concentration of Pb(s) added.

2. What is [Cr2+] when equilibrium is reached?
Since 1 mole of Pb(s) reacts with 2 moles of Cr3+(aq), the concentration of [Cr2+] will depend on the concentration of [Cr3+]. However, the problem does not provide the initial concentration of Cr3+(aq) or any information about the reaction progress. Hence, it is not possible to determine the concentration of [Cr2+] at equilibrium without further information.

3. What is [Cr3+] when equilibrium is reached?
Again, the given information does not provide the concentration of Cr3+(aq) initially or any information about the reaction progress. Without additional data, it is not possible to determine the concentration of [Cr3+] at equilibrium.

In summary, without information regarding the initial concentration or the progress of the reaction, it is not possible to determine the concentrations of [Cr2+] and [Cr3+] at equilibrium. However, you can assume the concentration of [Pb3+] is equal to the concentration of Pb(s) added.