Consider the simple salts NaCl(s) and AgCl(s). We will examine the equilibria in which these salts dissolve in water to formaqueous solutions of ions:NaCl(s)⇌Na+(aq) + Cl-(aq) AgCl(s)⇌Ag+(aq) + Cl-(aq) (a) Calculate the value of ΔG° at 298 K for each of the preceding reactions. (b) The two values from part (a) are very different.Is this difference primarily due to the enthalpy term or the entropy term of the standard free-energy change? (c) Use the valuesof ΔG° to calculate the Ksp values for the two salts at 298 K. (d) Sodium chloride is considered a soluble salt, whereas silverchloride is considered insoluble. Are these descriptions consistent with the answers to part (c)? (e) How will ΔG° for the solutionprocess of these salts change with increasing T ? What effect should this change have on the solubility of the salts?

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Consider the simple salts NaCl(s) and AgCl(s). We will examine the equilibria in which these salts dissolve in water to form
aqueous solutions of ions:
NaCl(s)⇌Na+(aq) + Cl-(aq)
AgCl(s)⇌Ag+(aq) + Cl-(aq)
(a) Calculate the value of ΔG° at 298 K for each of the preceding reactions. (b) The two values from part (a) are very different.
Is this difference primarily due to the enthalpy term or the entropy term of the standard free-energy change? (c) Use the values
of ΔG° to calculate the Ksp values for the two salts at 298 K. (d) Sodium chloride is considered a soluble salt, whereas silver
chloride is considered insoluble. Are these descriptions consistent with the answers to part (c)? (e) How will ΔG° for the solution
process of these salts change with increasing T ? What effect should this change have on the solubility of the salts?

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