Pb(NO3)2(aq) 2 x 10-3 M and Na2SO4(aq) 2 x 10-3 M
Identify the ions that are present in each solution, and calculate their concentrations.
If 1 L of each solution are mixed, will a precipitate be formed? Why?
That's ion product.
To identify the ions present in each solution and calculate their concentrations, we need to break down the given compounds into their respective ions.
1. Pb(NO3)2:
- This compound dissociates into the Pb2+ ion and two NO3- ions.
- Therefore, in solution, we have 1 Pb2+ ion and 2 NO3- ions.
2. Na2SO4:
- This compound dissociates into two Na+ ions and one SO42- ion.
- So, in solution, we have 2 Na+ ions and 1 SO42- ion.
To calculate the concentration of each ion, we need to know the total volume of the solution.
Assuming the total volume of the combined solution is 1 liter, we can calculate the concentration of each ion using their initial molarity:
Concentration of Pb2+ ion = (initial molarity of Pb(NO3)2) x (volume of solution)
Concentration of Pb2+ ion = 2 x 10^-3 M x 1 L = 2 x 10^-3 mol/L
Concentration of NO3- ion = (initial molarity of Pb(NO3)2) x (volume of solution)
Concentration of NO3- ion = 2 x 10^-3 M x 2 L = 4 x 10^-3 mol/L
Concentration of Na+ ion = (initial molarity of Na2SO4) x (volume of solution)
Concentration of Na+ ion = 2 x 10^-3 M x 1 L = 2 x 10^-3 mol/L
Concentration of SO42- ion = (initial molarity of Na2SO4) x (volume of solution)
Concentration of SO42- ion = 2 x 10^-3 M x 1 L = 2 x 10^-3 mol/L
Now, let's analyze if a precipitate will be formed when these solutions are mixed.
To determine if a precipitate will form, we need to consider whether a reaction will occur between the ions present. In this case, when Pb2+ and SO42- ions are mixed, they can react to form a precipitate called lead(II) sulfate (PbSO4).
The solubility rules state that most sulfates are soluble, but there are exceptions. Lead sulfate (PbSO4) is one of those exceptions; it is insoluble and forms a precipitate.
Since the concentrations of Pb2+ and SO42- ions in the combined solution are both 2 x 10^-3 M, which is higher than the solubility product constant (Ksp) for PbSO4, a precipitate of PbSO4 will form. Therefore, when these solutions are mixed, a precipitate will indeed be formed.
Calculate the ion prouct (Qsp) and compare with Ksp to determine if a ppt will form.
For (ion), it'sw mols/L soln except for a ppt. If a ppt forms, the concn of those ions is determined as a Ksp problem.