a) Determine how many molesof I3 are produced by 1 mole of Cu(IO3)2.
b)Determine the stoichiometric ratio between iodate and thiosulfate.
c)Determine the molar solubity expression for Cu(IO3)2
For C) I got ksp=[Cu2+][IO3-]^2
Is this correct?
Your answer for c is right. The equations below should help with a and b.
Cu(IO3)2 ==> Cu^2+ + 2IO3^-; i.e., 1 mol Cu(IO3)2 produces 2 mols IO3^-
IO3^- + 8I^- + 6H^+ ==> 3[I3]^- + 3H2O
For a) To determine how many moles of I3 are produced by 1 mole of Cu(IO3)2, we need to look at the balanced chemical equation for the reaction involving Cu(IO3)2.
The formula for Cu(IO3)2 suggests that it consists of 1 Cu2+ ion and 2 IO3- ions. The balanced chemical equation will guide us on the stoichiometry of the reaction.
Based on the balanced equation, if 1 mole of Cu(IO3)2 reacts, it will produce 2 moles of I3.
Therefore, 1 mole of Cu(IO3)2 produces 2 moles of I3.
For b) To determine the stoichiometric ratio between iodate (IO3-) and thiosulfate, we need to once again refer to the balanced chemical equation for the reaction between these two compounds.
The balanced equation will help us determine the ratio of the number of moles of IO3- to the number of moles of thiosulfate (S2O3^2-).
Please provide the specific balanced chemical equation for the reaction between iodate and thiosulfate so that I can guide you further in determining the stoichiometric ratio.
For c) Let's determine the molar solubility expression for Cu(IO3)2.
The solubility product expression (Ksp) represents the equilibrium expression for the dissolution of a sparingly soluble salt. In this case, Cu(IO3)2 is the sparingly soluble salt.
The balanced equation for the dissolution of Cu(IO3)2 would be:
Cu(IO3)2 (s) ⇌ Cu2+ (aq) + 2 IO3- (aq)
Based on this equation, the molar solubility expression for Cu(IO3)2 is:
Ksp = [Cu2+] * [IO3-]^2
Therefore, your expression for Ksp, which is Ksp = [Cu2+]*[IO3-]^2, is indeed correct.