1. The problem statement, all variables and given/known data Determine [K+] and [HT-] in this solution. If the temperature is Tp, a trace of solid is present and reaction is at equilibrium. Determine Ksp at this temperature. There is 0.950 g of KHT dissolved in 25.00 mL of solution. 2. Relevant equations KHT(s) ⇔ K+(aq) + HT-(aq) Ksp = [K+][HT-] 3. The attempt at a solution I originally thought to set up an ICE table to find the concentrations of K+ and HT- at equilibrium. With the concentrations, I figured I could then multiply them to get my Ksp value. I realized, however, I do not have a Kc value to use to solve for x. Is there any other way to find Ksp that I'm just missing?