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. Assume that the molarity of the NaOH solution used to titrate the saturated solution was actually higher than reported. Would the calculated KHT solubility be incorrectly high or low? Briefly explain.
2.) Assume that the filter paper that was used in the experiment had a small hole in it which allowed some solid KHT to get into the saturated filtrate. If some of the solid were included in the portion of solution titrated with NaOH solution, what effect would the solid have on the calculated KHT solubility? Briefly explain.
Answer all three questions and provide required steps