Question- I performed a chemistry experiment where I had to determine the solubility of potassium hydrogen tartrate (KHT) in a set of aqueous solutions containing various amounts of sodium chloride(NaCl) and potassium chloride(KCl). I also calculated the average solubility product constant for potassium hydrogen tartrate in these solutions.

I came up with the result that the more KCl there is, the lower the average solubility of KHT.

I have these following short questions to answer:

1) Suppose this experiment were performed using NaBr-KBr solutions instead of the NaCl-KCl solutions. Would you expect different results?

2) Would the results be different if NaCl-LiCl solutions were used in this experiment, instead of the NaCl-KCl solutions? Briefly explain.

3) If KHT did not dissociate when dissolved in aqueous solution, what effect would added KCl solution have on KHT solubility? Briefly explain.

4) The solubility of KHT in water increases with increasing temperature. What effect would an increase in temperature have on the experimentally determined Ksp (solubility product constant) of KHT?

I want you to explain the chemistry in this problem