1. Formation of complex compounds Put 4-5 drops of silver nitrate AgNO_(3) into a test tube. Add ammonium hydroxide NH_(4)OH until the precipitate is formed. Add excess of NH_(4)OH and observe the formation of a complex compound. Similarly, to perform a reaction for salts CuSO4, NiCl2 and Zn(NO3)2 Write down your observations and the reaction equation of obtaining complex compounds (in molecular and ionic-molecula : forms). For all complex compounds obtained, express the value of the instability constant. 2. Destruction of complex compounds Take solutions of silver (I) chloride diammine [Ag(NH3)2]Cl and copper (II) sulphate tetraammine [Cu(NH3)4]SO4 . obtained from the previous experiment, add dropwise diluted (1:1) nitric acid HNO3 until the complex compounds are destroyed. Write down your observations and the reaction equation of obtaining complex compounds (in molecular and ionic-molecular forms).

1. Formation of complex compounds:<br /><br />a. Silver nitrate and ammonium hydroxide:<br />Observation: A white precipitate of silver hydroxide is formed, which dissolves upon adding excess ammonium hydroxide to form a complex compound.<br />Reaction equation (molecular form): AgNO3 + 2NH4OH → [Ag(NH3)2]+ + NO3- + 2H2O<br />Reaction equation (ionic-molecular form): Ag+ + 2NH3 + NO3- + 2H2O → [Ag(NH3)2]+ + NO3- + 2H2O<br /><br />b. Copper(II) sulfate and ammonium hydroxide:<br />Observation: A blue precipitate of copper(II) hydroxide is formed, which dissolves upon adding excess ammonium hydroxide to form a complex compound.<br />Reaction equation (molecular form): CuSO4 + 4NH4OH → [Cu(NH3)4]SO4 + 4H2O<br />Reaction equation (ionic-molecular form): Cu2+ + 4NH3 + SO4^2- + 4H2O → [Cu(NH3)4]2+ + SO4^2- + 4H2O<br /><br />c. Nickel(II) chloride and ammonium hydroxide:<br />Observation: A green precipitate of nickel(II) hydroxide is formed, which dissolves upon adding excess ammonxide to complex compound.<br />Reaction equation (molecular form): NiCl2 + 4NH4OH → [Ni(NH3)4]Cl2 + 4H2O<br />Reaction equation (ionic-molecular form): Ni2+ + 4NH3 + 2Cl- + 4H2O → [Ni(NH3)4]2+ + 2Cl- + 4H2O<br /><br />d. Zinc nitrate and ammonium hydroxide:<br />Observation: A white precipitate of zinc hydroxide is formed, which dissolves upon adding excess ammonium hydroxide to form a complex compound.<br />Reaction equation (molecular form): Zn(NO3)2 + 4NH4OH → [Zn(NH3)4](NO3)2 + 4H2O<br />Reaction equation (ionic-molecular form): Zn2+ + 4NH3 + 2NO3- + 4H2O → [Zn(NH3)4]2+ + 2NO3- + 4H2O<br /><br />The instability constant (Kf) for the formation of these complex compounds can be expressed as:<br />Kf = [Complex]/([Metal ion][Base]^n), where n is the number of ligand molecules coordinated to the metal ion.<br /><br />2. Destruction of complex compounds:<br /><br />a. Silver(I) chloride diammine:<br />Observation: Upon adding dilute nitric acid, the complex compound [Ag(NH3)2]Cl dissociates, and a white precipitate of silver chloride is formed.<br />Reaction equation (molecular form): [Ag(NH3)2]Cl + HNO3 → AgCl + 2NH3 + H+<br />Reaction equation (ionic-molecular form): [Ag(NH3)2]+ + Cl- + H+ → AgCl + 2NH3 + H+<br /><br />b. Copper(II) sulfate tetraammine:<br />Observation: Upon adding dilute nitric acid, the complex compound [Cu(NH3)4]SO4 dissociates, and a blue precipitate of copper(II) hydroxide is formed.<br />Reaction equation (molecular form): [Cu(NH3)4]SO4 + 2H+ → Cu(OH)2 + 4NH3 + SO4^2-<br />Reaction equation (ionic-molecular form): [Cu(NH3)4]2+ + SO4^2- + 2H+ → Cu(OH)2 + 4NH3 + SO4^2-