Question

What is the Ksp of Hg2Cl2 at 298 K?

Half-Reaction Eº, V (at 298 K)
Hg22+ + 2e- -> 2 Hg(l) +0.80
Hg2Cl2(s) + 2e- -> 2 Hg(l) + 2 Cl-(aq) +0.31

Answer 1

The Ksp of Hg2Cl2 at 298 K is a measure of its solubility in water and can be calculated by knowing its concentration of ions at equilibrium, which is given as 1.1 × 10−18.

Step-by-step explanation:

The question asks for the solubility product constant (Ksp) of mercury(I) chloride (Hg2Cl2) at a temperature of 298 K. The Ksp is an equilibrium constant that indicates the degree to which a compound can dissolve in water. In the case of Hg2Cl2, also known as calomel, it has a very low solubility in water, which suggests that its Ksp will also be very low.

To determine the Ksp of Hg2Cl2 at 298 K, we can use the information provided regarding the solubility product constant of similar types of reactions. For example, we have a reference Ksp value for AgCl, and we are given a solubility equilibrium of PbCl2. From this, we understand that for Hg2Cl2, which dissolves according to the stoichiometry Hg2Cl2(s) ⇌ Hg22+(aq) + 2Cl−(aq), the Ksp expression can be written as Ksp = [Hg22+][Cl−]2. Using the given value of Ksp = 1.1 × 10−18 for Hg2Cl2, we can solve for the concentration of ions at equilibrium.