In 'Synthesis of an Iron Complex Salt', a student added 95% ethyl alcohol to a solution containing iron and oxalate ions. This was done to titrate the solution until its endpoint create a metal-chelate complex

Explain why addition of NH3 or HNO3 to a saturated solution of Cu(OH)2 in contact with solid Cu(OH), increases the solubility of the solid. O NH3 forms a complex ion with OH-, reducing its concentration and allowing more OH- ions to dissolve from the solid phase. HNO3 reacts with Cu2", thereby reducing the Cu2 concentration and allowing more solid to dissolve O NH3 forms a complex ion with Cu2, increasing the Cu2 concentration. HNO3 reacts with OH-, thereby increasing the OH- concentration and allowing more solid to dissolve O NH3 forms a complex ion with Cu2, reducing the Cu2 concentration and allowing more Cu2 ions to dissolve from the solid phase. HNO3 reacts with OH-, thereby reducing the OH- concentration and allowing more solid to dissolve

The formation constant of a silver cyano complex is 5.6 x 1018 Ag+ + 2 CN Ag(CN)," If a certain solution have the equilibrium concentrations of 5.0 x 10-3 M and 0.20 M for Ag+ and CN", respectively, then what is the equilibrium concentration for the silver cyano complex? O1.1 x 1015 O5.6 x 1015 02.8 x 1016 02.4 x 109

After completing the experiment, a student finds that the equilibrium concentrations of the reactants and product are as follows. Calculate the equilibrium constant for the complex ion formation. [SCN¯]eg= 6.45x10-4 M %3D [Fe3+]eg = 8.42x10-4 M leq [FENCS2+]eg = 1.50x10-4 M %3D

Formation constant and Gibbs free energy For the complex formation reaction where Mis any metal and L is any ligand, M+ + 2L = [ML2]* Kr is the formation constant for the complex at equilibrium and AG is the Gibbs free energy change for the reaction at equilibrium. The formation constant (K) can be related to the Gibbs free energy change (AG°) for a reaction by the equation AG° = RT In Kr where T is the temperature in kelvins and R is the gas constant equal to 8.314 J K. mol. The complex formation is generally a spontaneous process; thus, the Gibbs free energy change is negative. Part B Calculate the formation constant for the formation of [Cu(en) (H2O)4 from (Cu(H20)6]+, given that AG° is -60.1kJ - mol at 298 K.

Please use the values in the resources listed below instead of the textbook values. Sometimes equilibria for complex ions are described in terms of dissociation constants, Ka. For the complex ion Cu(CN)4 3- the dissociation reaction is as follows. [Cu*]• [CN 14 Kd [Cu(CN)43-] Cu(CN)4 3- = Cu+ + 4 CN- = 5.0X10° n-31 = Calculate the value of the formation constant, Kf, for Cu(CN)4°¯. 4.0

The chemical reaction for the formation of the red-orange iron(III) thiocyanate complex ion is Fe3+ (aq) +  SCN- (aq)  <==> [FeSCN2+] (aq)   What is the source of the Fe3+ ions?   What is the source of the SCN- ions?   The equilibrium constant for this reaction is given by what