The equilibrium constant for the reaction Hg^2+(a q)+2 Cl^-(a q) ⇌HgCl2(a q) is 1.6 ×10^13 . Is

step 1 Hello everyone, this is Ricky. And today we're working on problem 91. All right, so we're given

The equilibrium constant for the reaction Hg^2+(a q)+2...

The equilibrium constant for the reaction $\mathrm{Hg}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{HgCl}_{2}(a q)$ is $1.6 \times 10^{13} .$ Is $\mathrm{HgCl}_{2}$ a strong electrolyte or a weak electrolyte? What are the concentrations of $\mathrm{Hg}^{2+}$ and $\mathrm{Cl}^{-}$ in a $0.015-\mathrm{M}$ solution of $\mathrm{HgCl}_{2} ?$

The equilibrium constant for the reaction $\mathrm{Hg}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{HgCl}_{2}(a q)$ is $1.6 \times 10^{13} .$ Is $\mathrm{HgCl}_{2}$ a
strong electrolyte or a weak electrolyte? What are the concentrations of $\mathrm{Hg}^{2+}$ and $\mathrm{Cl}^{-}$ in a $0.015-\mathrm{M}$ solution of $\mathrm{HgCl}_{2} ?$

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Key Concepts

Strong vs. Weak Electrolytes

Electrolytes are substances that dissociate into ions in solution. A strong electrolyte dissociates completely, resulting in high ion concentrations, whereas a weak electrolyte dissociates only partially. In this context, a very high equilibrium constant for the formation of the molecular species implies that the compound, when dissolved, produces only negligible amounts of ions, classifying it as a weak electrolyte.

Dissociation Equilibrium

Dissociation equilibrium describes the balance between the undissociated compound and its ionized components in solution. The relative position of this equilibrium is governed by the equilibrium constant. When a compound has an equilibrium that strongly favors the undissociated form, its ions are present in only minute amounts, which is characteristic of a weak dissociation process.

Equilibrium Constant

The equilibrium constant (K) quantifies the ratio of product concentrations to reactant concentrations at equilibrium. A large equilibrium constant indicates that the reaction strongly favors the products, meaning that the reverse reaction (or dissociation) occurs to a very limited extent, leading to very low concentrations of the reactant ions in solution.

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