nickel and silver nitrate reaction

Sodium reacts vigorously with water to produce aqueous sodium hydroxide and hydrogen (see figure below). and nickel (II) nitrate. Easily dissolved in dilute nitric acid. Solution A: 0.1 M sodium sulfide, colorless. The overall chemical equation for the reaction shows each reactant and product as undissociated, electrically neutral compounds: 2AgNO3(aq) + K2Cr2O7(aq) Ag2Cr2O7(s) + 2KNO3(aq) No reaction occurs 2 Na+(aq) + 2 OH-(aq) + Ni2+ (aq) + 2NO3 -(aq) - -> 2Na+(aq) + 2NO3(aq) + Ni(OH)2(s) Nat(aq) + NO3- (aq) - NaNO3(s) 2 Na+ (aq) + 2NO3(aq) Na2(NO3)2(s) Ni2+ (aq) + 2OH- (aq) Ni(OH)2(3) Ni2+ (aq) + OH (aq) NiOH(3) 2) Select the net ionic equation for the . Solution B: 0.2 M nickel (II) nitrate, green. e. Suppose that this reaction is carried. Nickel chloride silver nitrate molecular ionic and net ionic? Use uppercase for the first character in the element and lowercase for the second character. The circuit is closed using a salt bridge, which transmits the current with moving ions. I need help with describing the process of obtaining the following question in detail with a balanced equation and all the calculations. Species which accept electrons in a redox reaction are called oxidizing agents, or oxidants. Because two \(\ce{NH4^{+}(aq)}\) and two \(\ce{F^{} (aq)}\) ions appear on both sides of Equation \(\ref{4.2.5}\), they are spectator ions. A 21.5 g sample of nickel was treated with excess silver nitrate solution to produce silver metal and nickel (II) nitrate. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will. 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