Metal cations in solution are complexed to HO molecules and exist as hydrated ions. For example,...

 

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Metal cations in solution are complexed to H₂O molecules and exist as hydrated ions. For example, Ni²+ 2+ complexes to form the hydrated ion Ni(H₂0)62. Metal cations are also able to complex to other ligands, such as NH3. An aqueous solution is prepared in which 0.00139 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62* is equal to 5.5 x 108 answer plz: Calculate the concentration of Ni(H₂O)62+ ions at equilibrium in the solution formed. Metal cations in solution are complexed to H₂O molecules and exist as hydrated ions. For example, Ni²+ 2+ complexes to form the hydrated ion Ni(H₂0)62. Metal cations are also able to complex to other ligands, such as NH3. An aqueous solution is prepared in which 0.00139 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62* is equal to 5.5 x 108 answer plz: Calculate the concentration of Ni(H₂O)62+ ions at equilibrium in the solution formed.

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To calculate the concentration of NiH2O2 ions at equilibrium in the solution formed we need to use ... View the full answer