6. Reagents: 0.1 MCu(NO,), 1 MHCI, 1 MNH, For reaction 5, there are two equilibr

Question

6. Reagents: 0.1 MCu(NO,), 1 MHCI, 1 MNH, For reaction 5, there are two equilibria to consider: +. 2) -Cu(OH) EQ 17.16) Cu2+(aq) pale blue 2H20 () 2NH, (a) 2 (s) + + blue ppt Ke + 2 OH EQ 17.17) 3 (aq) tetraammineco on blue ppt deep blue Be careful with the amount of rea s eas ![Cu(NH,)41 instead of Cu(OH a. Cu(OF)2 (s) produced by b. Net Ionic Equation c. Equilibrium shifted to the left by d. Observation e. Net Ionic Equati f. Reason for shift g. Equilibrium shifted to the right by h. Observat Net Ionic Reason for the shift i. Equatiorn j.

Explanation / Answer

a. Cu(OH)2 is produced by electrolysis of water in presence of little electrolyte such as sodium sulphate or magnesium sulphate and copper is used as anode.

b.

2H+ (aq) + 2(OH)- (aq) + 2 NH3 (aq) + Cu2+ (aq) = Cu(OH)2 (s)+ 2NH4+ (aq)

Cu2+ (aq) + 2(OH)- (aq) + 4NH3 (aq) = [Cu(NH3)]2+ (aq) + 2(OH)- (aq)

c. Equilibrium is shifted to left by addition of 1 M NH3 and 1 M HCl

d. Increase in color of pale blue color given by Cu2+

e. 2H+ (aq) + 2(OH)- (aq) + 2 NH3 (aq) + Cu2+ (aq) = Cu(OH)2 (s)+ 2NH4+ (aq)

f. NH3 and HCl would increase concentration of NH4+. High NH4+ would tend to balance out the reaction and equilibrium shifts left.

g. Equilibrium shifted to the right by addition of 1 M NH3

h. Increase in deep blue color by [Cu(NH3)]2+

i. Cu2+ (aq) + 2(OH)- (aq) + 4NH3 (aq) = [Cu(NH3)]2+ (aq) + 2(OH)- (aq)

j. NH3 concetration would tend to balance out the equation by shifting the equilibrium towards right.

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