Hello there, I have tried my best to solve this problem, but no matter how I try

Question

Hello there,

I have tried my best to solve this problem, but no matter how I try thinking about it, I am not getting an answer that makes sense. Any help as soon as possible would be appreciated. This lab is due tommorow.

Procedure Reagents 0.1 MCu(NO3 2, 1 M HCl, 1 M NH3 reaction 5, there are two equilibria to consider: For 2 H2O (l) Cu 2+ (aq) 2 NH 3 (aq) Cu(OH) pale blue 2 (s) 4 (a EQ 17.16) blue ppt Cu(OH) 4 NH 2 (s) [Cu(NH3 41 2+ 3 (aq) 2 OH (aq) EQ 17.17) (ag) tetraamminecopper (ID ion blue ppt deep blue Be careful with the amount of reagent added. It is easy to make 2+. [Cu(NH3)4] instead of Cu(O roduced by 2 (s) b. Net Ionic Equation c. Equilibrium shifted to the left by d. Observation e. Net Ionic Equation f. Reason for shift g. Equilibrium shifted to the right by h. Observation i. Net Ionic Equation i. Reason for the shift

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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