Aqueous copper(II) sulfate (CuSO₄) solution can react with various substances to yield different products depending on the reactants involved. Here are some common reactions:
-
With barium hydroxide (Ba(OH)₂): When barium hydroxide is added to aqueous copper(II) sulfate, a double displacement reaction occurs, producing barium sulfate (a solid precipitate) and copper(II) hydroxide (which may also precipitate depending on the conditions): \[ \text{CuSO}_4 (aq) + \text{Ba(OH)}_2 (aq) \rightarrow \text{BaSO}_4 (s) + \text{Cu(OH)}_2 (s) \]
-
With sodium carbonate (Na₂CO₃): This reaction leads to the formation of copper(II) carbonate (CuCO₃, which may decompose) and sodium sulfate: \[ \text{CuSO}_4 (aq) + \text{Na}_2\text{CO}_3 (aq) \rightarrow \text{CuCO}_3 (s) + \text{Na}_2\text{SO}_4 (aq) \]
-
With ammonia (NH₃): When ammonia is added to copper(II) sulfate solution, it can form a complex compound known as [Cu(NH₃)₄]²⁺ (tetraamminecopper(II) complex): \[ \text{CuSO}_4 (aq) + 4 \text{NH}_3 (aq) \rightarrow [\text{Cu(NH}_3)_4]^{2+}(aq) + \text{SO}_4^{2-}(aq) \]
-
With reducing agents: Upon reaction with a suitable reducing agent (like zinc or iron), copper(II) ions can be reduced to elemental copper: \[ \text{CuSO}_4 (aq) + \text{Zn} (s) \rightarrow \text{Cu} (s) + \text{ZnSO}_4 (aq) \]
These are just a few examples; the specific products will depend on the other substances you are reacting with the copper(II) sulfate solution.
4 answers