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SOLVED: If AgCl(s) is in equilibrium with dissolved AgCl according to the following equation: AgCl(s) → Ag (aq) Cl-(aq). If the equilibrium constant for this process is Kc = 1.8x10^-10, what is the Ag concentration when AgCl is dissolved in pure water?
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Consider the reaction AgCl(s) ⟶Ag^ (a q) Cl^-(a q) (a) Calculate ΔG^∘ at 25^∘ C. (b) What should the concentration of Ag^ and Cl^- be so that ΔG=-1.0  kJ (just spontaneous)? Take [Ag^ ]= [Cl^-] (c) The Ksp for AgCl is 1.8 ×10^-10 . Is the answer to (b) reasonable? | Numerade
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