2. The fol1owing questions desl with reactions involving the ironI) nitrate solu

Question

2. The fol1owing questions desl with reactions involving the ironI) nitrate solution. 2) Considering the pH of this solution, what two species, besides the Fe(H20) ions and water, are present in a significant concentration? b) Write the equation for the reaction of a Fe(NO3 3 solution with aqueous HNO3 c) Write the equation for the reaction of FeCH20)63 with HC1 solution. d) krite the equation for the reaction of SCN- with the complex ion produced in (c) 3. Write an equation for each of these reactions involving Cu(II) a) The addition of excess 6 M HC1 solution to Cu(H20) 62: b) The acid-base reaction for dissolving Cuo with aqueous Ho

Explanation / Answer

Answer:

A) as given, when pH is involved there are definitely H+ Ions(also known as H3O+) and OH- ions.

B)  oxidation: Fe(NO3)2 with Fe's at +2, losing 1 electron ---> forming Fe(NO3)3 with Fe's at +3
reduction: HNO3 with N's at +5, takes 3 electrons -> forming NO with N's at +2

electrons balance as:
3 Fe(NO3)2 loses 3 e- ---> 3 Fe(NO3)3
1 HNO3 takes 3 e- -> 1 NO

which gives us:
3 Fe(NO3)2 + 1 HNO3 -> 3 Fe(NO3)3 +1 NO + H2O

to get the extra nitrates to make Fe(NO3)3 we add 3 additional HNO3 's that do not redox:
3 Fe(NO3)2 + 1 HNO3 & 3 HNO3 -> 3 Fe(NO3)3 +1 NO + H2O

balance H's:
3 Fe(NO3)2 + 1 HNO3 & 3 HNO3 -> 3 Fe(NO3)3 +1 NO + 2H2O

done, oxygens balance already...
just combine the two batches of HNO3 's:
3 Fe(NO3)2 & 4 HNO3 -> 3 Fe(NO3)3 +1 NO + 2H2O.

C) Fe(H2O)6 3+ with HCl solution
[Fe(H2O)6]3+ + 4HCl(aq)<==> [FeCl4]- + 4H+ + 6H2O

D)  SCN- with the complex ion produced in C
[FeCl4]- + SCN- <==> [FeSCN]2+ + 4Cl- .

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