Chemistry > Lab Report > Binghamton University CHEM 108 Copy_of_Laboratory_Exercise_7_CHEM_108-REVIEWED BY EXPERTS-GRADED A+ (All)

Binghamton University CHEM 108 Copy_of_Laboratory_Exercise_7_CHEM_108-REVIEWED BY EXPERTS-GRADED A+

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Laboratory Exercise #7: Determination of Ksp of a Tartrate Salt Department of Chemistry, Binghamton University, Binghamton, NY 13902 Introduction: The objective of this laboratory experiment was to... determine the solubility product constant of the potassium hydrogen tartrate salt that is used in Cream of Tartar. In order to determine the solubility constant of a slightly soluble ionic salt, the dissociation of the salt in a solution must be examined. Ex. Aa Bb y−¿ x+¿+bB (aq) ¿ A a Bb(s)⇔ a A( ¿aq) y−¿¿b B¿ x+¿¿a¿ A¿ K sp=¿ Using the example shown above, the dissociation reaction and Ksp of KH C4 H4O6 can be determined. −¿❑ (aq) +¿+ H C 4 H4 O6 ¿ KH C 4 H4O6(s)⇔ K(¿aq) +¿ −¿¿❑ H C4 H4O6 ¿ K (aq) ¿ ¿ K sp=¿ When expressing the molar solubility for the tartrate salt in pure water, it should be expressed as “s” which would allow for the Ksp equilibrium constant to be re-written. Using a simple acidbase titration, the molar solubility can be calculated due to the hydrogen tartrate being a monoprotic weak acid. K sp=[s][s]=s2 2−¿❑ (aq)+H2O(l) −¿→C4 H4 O6 ¿ −¿❑ (aq)+O H¿ H C 4H 4O6 ¿ In addition to determining the solubility of the tartrate salt in pure water, the solubility will be determined of tartrate salt in a 0.10 M KCl solution. This will cause the Ksp equilibrium constant to be modified. The total concentration of +¿ K (aq) ¿ differs from the concentration of the hydrogen tartrate. K sp=[s+0.10][ s] [Show More]

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