Answer to Question #155418 in General Chemistry for C

Question

The molar solubility of cobalt(II) iodate, Co(IO₃)₂, is 0.011 mol/L.  

1.Write the equilibrium dissociation of Co(IO₃)₂.

2. Given the molar solubility of Co(IO₃)₂, what is the concentration of each ion in a saturated solution?

3. Calculate the solubility product constant, Ksp, for Co(IO₃)₂.

Answer 1

1. Equilibrium dissociation of Co(IO3)2

  Co(IO₃)₂ ⇌ Co²⁺ + 2IO₃^-

  

2. molar solubility of cobalt(II) iodate, Co(IO3)2, is 0.011 mol/L.  

 

 It means 0.011 mol Co(IO3)2 get solvated in 1liters solution and get dissociated into ions

From dissociation equilibrium,

  1 mole of Co(IO3)2 dissociated into 1 mole of Co²⁺ and 2 moles of IO₃^-.

  

So, 0.011 mol Co(IO3)2 dissociated into 0.011 mole of Co²⁺ and 0.022 moles of IO₃^- in 1 liter solution.

So, concentration of [Co²⁺] = 0.011 M

    concentration of [IO₃^-] = 0.022 M

    

3. Calculate the solubility product constant, Ksp = [Co²⁺]×[IO₃^-]²

             = 0.011×(0.022)²

             = 5.324×10^-6