The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H406 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6 (aq) + OH (aq) + C4H406² (aq) + H2Ou) The table below shows the data gathered from the experiment. Initial buret reading, mL Final buret reading, mL Volume of KHC4H4O6 solution, mL 11.25 32.30 15.00 1. Write the dissociation reaction for KHC4H4O6 + and the Ksp expression KHC4H406(s) – K^1+(aq) + HC4H406^1-(aq) KHC4H406(aq) → K^1+(aq) + HC4H406^1-(aq) HC4H406^1-(aq) H^1+(aq) + C4H406^2-(aq) HC4H406^1-(s) H^1+(aq) + C4H406^2-(aq) 2. What is the molar solubility of KHC4H4O6? Ksp expression Ksp = [H^1+][C4H406^2-] Ksp = [K^1+][HC4H406^1-] 2. What is the m Ksp = [H^1+][C4H406^2-J/[HC4H406^1-] Ksn = IKA1+1THCAHA06^1-1/[ KHCAHA061.

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