What will happen if 50mL of 0.022M Na2S2O3, 50mL of 0.010M AgNO3, and 50mL of 0.097M KCl are mixed together? For AgCl, ksp=1.8x10^-10 ; for Ag(S2O3)2^3-, Kf= 2.9 x 10^13.

I would suggest you go about it this way.

First, you know Cl from KCl concn. Using Ksp for AgCl, and the KCl concentration, calculate (Ag^+) needed to ppt AgCl.
Then using Kf for Ag(S2O3)^3-, calculate the Ag^+ in that solution. Compare that with Ag^+ from the Ksp. Post your work if you get stuck.

precipitate will form

To determine what will happen when these solutions are mixed together, we need to consider the possible reactions that can occur based on the given information.

Let's analyze the potential reactions step by step:

1. Na2S2O3 (sodium thiosulfate) reacts with AgNO3 (silver nitrate):
Na2S2O3 + 2AgNO3 -> 2NaNO3 + Ag2S2O3

This reaction forms silver thiosulfate (Ag2S2O3) and sodium nitrate (NaNO3).

2. Ag2S2O3 (silver thiosulfate) further reacts with AgNO3:
Ag2S2O3 + 2AgNO3 -> AgCl + 2NaNO3 + Ag(S2O3)2^3-

Here, silver thiosulfate reacts with more silver nitrate to produce AgCl (silver chloride), sodium nitrate (NaNO3), and the complex ion Ag(S2O3)2^3-.

3. AgCl (silver chloride) can react with KCl (potassium chloride):
AgCl + KCl -> AgCl + K+

This reaction does not lead to any significant change in the solution because both AgCl and KCl are sparingly soluble salts.

Based on these reactions, we can predict that the following compounds will be present in the final solution after mixing:

- AgCl (silver chloride)
- Ag(S2O3)2^3- (silver thiosulfate complex ion)
- NaNO3 (sodium nitrate)
- K+ (potassium ion)

Now, let's consider the solubility product constant (Ksp) and the stability constant (Kf) provided:

The Ksp value of AgCl (silver chloride) is 1.8x10^-10. Since this value is very small, we can conclude that AgCl will remain largely insoluble and form a precipitate in the solution.

The Kf value of Ag(S2O3)2^3- (silver thiosulfate complex ion) is 2.9x10^13, which suggests that the complex is highly stable. Therefore, Ag(S2O3)2^3- will remain in solution.

In summary, when 50mL of 0.022M Na2S2O3, 50mL of 0.010M AgNO3, and 50mL of 0.097M KCl are mixed, a precipitate of AgCl will form due to its low solubility. Additionally, Ag(S2O3)2^3- will remain in solution along with NaNO3 and K+, being soluble in the solution.