The electrode in the left half-cell is the anode because oxidation occurs here. However, if the two compartments are in direct contact, a salt bridge is not necessary. The following video shows an example of this oxidation occurring. Anions in the salt bridge flow toward the anode and cations in the salt bridge flow toward the cathode. and nickel (II) nitrate. Solved Silver nitrate reacts with nickel metal to produce - Chegg Slowly forms a surface oxide at room temperature Very slow reaction. Solved 1). Select the net ionic equation for the reaction - Chegg Solved 1. Consider the reaction when aqueous solutions of - Chegg One half-cell, normally depicted on the left side in a figure, contains the anode. Simply mixing solutions of two different chemical substances does not guarantee that a reaction will take place. a. 6: Types of Chemical Reactions (Experiment - Chemistry LibreTexts Since there is an equal number of each element in the reactants and products of NiCl2 + 2AgNO3 = Ni(NO3)2 + 2AgCl, the equation is balanced. 2NO3-, 2AgNO3 + NiCl2 -------> 2AgCl + Ni(NO3)2, The following uses nickel(II) chloride Aqueous solutions of rubidium hydroxide and cobalt(II) chloride are mixed. Aqueous solutions of calcium bromide and cesium carbonate are mixed. Aqueous solutions of barium chloride and lithium sulfate are mixed. \[\ce{3AgF(aq) + Na_3PO_4(aq) \rightarrow Ag_3PO_4(s) + 3NaF(aq) } \nonumber \], \[\ce{3Ag^+(aq) + 3F^{-}(aq) + 3Na^{+}(aq) + PO_4^{3-}(aq) \rightarrow Ag_3PO_4(s) + 3Na^{+}(aq) + 3F^{-}(aq) } \nonumber \], \[\ce{3Ag^{+}(aq) + PO_4^{3-}(aq) \rightarrow Ag_3PO_4(s)} \nonumber \]. 17.7: Electrolysis - Chemistry LibreTexts Solution A: 0.1 M sodium sulfide, colorless. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. As soon as the copper metal is added, silver metal begins to form and copper ions pass into the solution. Calculate the net ionic equation for NiCl2(aq) + 2AgNO3(aq) = Ni(NO3)2(aq) + 2AgCl(s).