#3-c Post-lab exp. 24 3. Concerning the applicability of the titration method, comment on if and...

#3-c Post-lab exp. 24

3. Concerning the applicability of the titration method, comment on if and how you could use it to determine K_sp for the following:

c. copper (II) iodate

Expert Solution

To measure the solubility product (Ksp) of Cu(IO3)2

When an excess of slightly soluble salt is left in contact with water, a dynamic equilibrium between the solid and the ions in solution results. In the case of copper (II) iodate in water this salt would dissolve to a very small extent according to the reaction:

Ca(IO3)2(s) <------> Ca2+(aq) + 2 IO3 -(aq)

to determine the K_sp for Ca(IO3)₂(s) by calculating the concentration of either Ca²⁺(aq) or IO₃^?(aq). The balanced equilibrium as shown above and K_sp expression are shown below:

K_sp = [Ca²⁺] [IO₃^?]²

In this experiment it is much easier to calculate the concentration of IO₃^?(aq) and this concentration is determined by a common technique used by chemists called a titration. In a typical titration the concentration of a certain ion [in this case IO₃^?(aq)] is unknown and it is combined with a reagent solution whose concentration is known. Chemists refer to the known solution as the standard solution [in this case S₂O₃^2?]. Notice that the Na₂S₂O₃ standardized solution is listed as having a concentration of 0.05xx (four decimals) in the lab procedure. It really doesn

queen_honey_blossom answered 1 day ago

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