List the following equilibrium solutions in order of decreasing free Ag+ concentration in mixture: 0.1M AgNO3, saturated AgCl, saturated AgBr, saturated AgI, Ah(NH3)2+, and Ag(S2O3)2 3-.
For AgNO3 you have 0.1 M Ag^+ because the salt is completely soluble and completely ionized. For a saturated solution of AgI, AgCl, an AgBr, you must use Ksp to determine Ag^+ in solution. For the last two complex ions, you need a concn which isn't listd.
To determine the order of decreasing free Ag+ concentration in the mixture, we need to consider the solubility product constants (Ksp) of the compounds involved. The equation for the dissociation of each compound is as follows:
1. AgNO3 ↔ Ag+ + NO3-
2. AgCl ↔ Ag+ + Cl-
3. AgBr ↔ Ag+ + Br-
4. AgI ↔ Ag+ + I-
5. Ag(NH3)2+ ↔ Ag+ + 2NH3
6. Ag(S2O3)2 3- ↔ 2Ag+ + 3S2O3 2-
The solubility product constant (Ksp) expressions for these compounds are:
1. Ksp(AgNO3) = [Ag+][NO3-]
2. Ksp(AgCl) = [Ag+][Cl-]
3. Ksp(AgBr) = [Ag+][Br-]
4. Ksp(AgI) = [Ag+][I-]
5. Ksp(Ag(NH3)2+) = [Ag+][NH3]^2
6. Ksp(Ag(S2O3)2 3-) = [Ag+]^2[S2O3 2-]^3
To compare the equilibrium solutions, we need to determine which compound has the highest Ksp. The higher the Ksp value, the more soluble the compound, resulting in a higher free Ag+ concentration.
Let's examine the Ksp values for each compound:
1. Ksp(AgNO3) is not relevant in this case since it is already an ionic compound that fully dissociates into Ag+ and NO3- ions.
2. Ksp(AgCl) is a constant value, 1.8 x 10^-10.
3. Ksp(AgBr) is a constant value, 5.4 x 10^-13.
4. Ksp(AgI) is a constant value, 8.3 x 10^-17.
5. Ksp(Ag(NH3)2+) is not relevant since it involves coordination complex formation with ammonia (NH3), and its value is related to the concentration of ammonia.
6. Ksp(Ag(S2O3)2 3-) is a constant value, 1.5 x 10^-10.
From the available Ksp values, we find that AgNO3 will have the highest free Ag+ concentration since it is already fully dissociated. Among the remaining compounds, Ag(S2O3)2 3- (thiosulfate) has the next highest Ksp value.
Therefore, the order of decreasing free Ag+ concentration in the mixture would be:
1. AgNO3
2. Ag(S2O3)2 3-
3. AgCl
4. AgBr
5. AgI
6. Ag(NH3)2+
Please note that the specific concentrations depend on the conditions and the starting concentrations of the compounds.