Determination of the Solubility Product Constant of a Salt

3 March 2017

When no KHC4H4O6 dissolves, the concentrations of K+(aq) and HC4H4O6-(aq) will not increase further and any additional KHC4H4O6 added after this point will remain as a solid. At this point, the solution is said to be saturated.

The rates at which KHC4H4O6 is dissolving and reprecipitating are equal in a saturated solution, so that no net change is observed. This process is another example of dynamic equilibrium. The equation for potassium hydrogen tartrate dissolving in water

On the other hand, the solubility of a compound refers to the concentration of a solute in equilibrium with undissolved solute in a saturated solution. In this experiment, the solubility and the solubility product constant in water of KHT was determined. The concentration of HC4H4O6- in solution can be determined by the direct titration of a filtered solution with a standard sodium hydroxide solution, since it is a slightly soluble salt. Because one mole of sodium hydroxide neutralizes one mole of HT- ions, the number of moles of sodium hydroxide used in the titration will equal the number of moles of HT

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