Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed. Will it lead to the precipitation of copper iodate? (For cupric iodate Ksp = 7.4 × 10–8).
Solution and Explanation
When equal volumes of sodium iodate and cupric chlorate solutions are mixed, then the molar concentrations of both solutions are reduced to half i.e., 0.001 M.
Then, NaI03 \(\rightarrow\) Na+ + 10-3
0.001M 0.001M
Cu(CIO3)2\(\rightarrow\) Cu2+ + 2CIO3-
0.001M 0.001M
Now, the solubility equilibrium for copper iodate can be written as: Cu(I03)2\(\rightarrow\)Cu2+(aq) + 2I03-(aq)
Ionic product of copper iodate: = [Cu2+] [I03-]2 = (0.001)(0.001)2 = 1 × 10-9
Since the ionic product (1 × 10-9) is less than Ksp (7.4 × 10-8), precipitation will not occur.
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Concepts Used:
Equilibrium Constant
The equilibrium constant may be defined as the ratio between the product of the molar concentrations of the products to that of the product of the molar concentrations of the reactants with each concentration term raised to a power equal to the stoichiometric coefficient in the balanced chemical reaction.
The equilibrium constant at a given temperature is the ratio of the rate constant of forwarding and backward reactions.
Equilibrium Constant Formula:
Kequ = kf/kb = [C]c [D]d/[A]a [B]b = Kc
where Kc, indicates the equilibrium constant measured in moles per litre.
For reactions involving gases: The equilibrium constant formula, in terms of partial pressure will be:
Kequ = kf/kb = [[pC]c [pD]d]/[[pA]a [pB]b] = Kp
Where Kp indicates the equilibrium constant formula in terms of partial pressures.
- Larger Kc/Kp values indicate higher product formation and higher percentage conversion.
- Lower Kc/Kp values indicate lower product formation and lower percentage conversion.
Medium Kc/Kp values indicate optimum product formation.
Units of Equilibrium Constant:
The equilibrium constant is the ratio of the concentrations raised to the stoichiometric coefficients. Therefore, the unit of the equilibrium constant = [Mole L-1]△n.
where, ∆n = sum of stoichiometric coefficients of products – a sum of stoichiometric coefficients of reactants.