I performed a chemistry experiment where I had to determine the solubility of po
ID: 838661 • Letter: I
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 (KHT) 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 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 (potassium hydrogen tartrate) 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 (potassium hydrogen tartrate) in water increases with increasing temperature. What effect would an increase in temperature have on the experimentally determined Ksp (solubility product constant) of KHT?
Explanation / Answer
1) Yes, we would expect different results as Br are bigger atoms than Cl and will sterically hinder the solubility of KHT more.
2) KCl already has K atoms which on dissociation are released as K+ so solubility of KHT decreases as it also dissociates to give K+ when KCl is there. If we will use LiCl then solubility is bound to increase.
3) Just as I said in 2). If KHT does not dissociate then KCl addition will have no effect on KHT solubility.
4) Ksp increases with temperature so Ksp of KHT too will increase on increasing temperature.
Hope this helps. Thank You.