A chemist designs an ion-specific probe for measuring [Ag⁺] in an NaCl solution saturated with AgCl. One halfcell has an Ag-wire electrode immersed in the unknown AgCl-saturated NaCl solution. It is connected through a salt bridge to the other half-cell, which has a calomel reference electrode [a platinum wire immersed in a paste of mercury and calomel (Hg₂Cl₂)] in a saturated KCl solution. The measured E_{\text {cell }} is 0.060 V.(a) Given the following standard half-reactions, calculate [Ag⁺]. Calomel: Hg₂Cl₂(s) + 2e⁻ → 2Hg(l) + 2Cl⁻(aq) E°=0.24VSilver Ag⁺(aq) + e⁻ → Ag(s) E° = 0.80 V(Hint: Assume that [Cl⁻] is so high that it is essentially constant.)