In: Chemistry
Write balanced net ionic equations for the following reactions in basic solution.
A. S2O32−(aq)+I2(aq)→S4O62−(aq)+I−(aq)
Express your answer as a chemical equation. Identify all of the phases in your answer.
Part B Mn2+(aq)+H2O2(aq)→MnO2(s)+H2O(l)
Part C Zn(s)+NO3−(aq)→NH3(aq)+Zn(OH)42−(aq)
Part D Bi(OH)3(s)+Sn(OH)3−(aq)→Bi(s)+Sn(OH)62−(aq)
NOTE :-
Follow the following steps while balancing the Redox reaction by ion-exchange method :-
Step.1 :- Write and balance the oxidation and reduction half cell reactions separately.
Step.2 :- Balance the atoms other than hydrogen and oxygen
Step.3 :- Balance the oxygen atom by adding suitable number of H2O on the oxygen deficient side.
Step.4 :- After that balance the hydrogen atom by adding suitable number of H+ on the hydrogen deficient side.
Step.5 :- Finally balance the charge on both side by adding suitable number of electrons.
Step.6 :- First balance the equation in acidic medium and then converted this equation in basic medium by adding same number of moles of OH- ( as that of H+) on both the sides.
1.
Balanced Oxidation half cell reaction is :
2 S2O32−(aq) ----------------> S4O62−(aq) + 2e-
Balanced Reduction half cell reaction is :
I2 (aq) + 2e- --------------> 2 I- (aq)
Adding both the half cell reaction, we have balanced chemical equation in basic medium is :
2 S2O32−(aq) + I2 (aq) ---------------> S4O62−(aq) + 2 I- (aq)
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2.
Balanced Oxidation half cell reaction is :
Mn2+(aq) + 2 H2O (l) ----------------> MnO2(s) + 2e- + 4 H+ (aq)
Adding 4 OH- on both sides in order to write equation in basic medium, we have
Mn2+(aq) + 4 OH- (aq) ----------------> MnO2(s) + 2e- + 2 H2O (l)
Balanced Reduction half cell reaction is :
H2O2(aq) + 2 H+ (aq) + 2e- --------------> 2 H2O(l)
Adding 2 OH- on both sides in order to write equation in basic medium, we have
H2O2(aq) + 2e- --------------> 2 OH- (aq)
Adding both the half cell reaction, we have balanced chemical equation in basic medium is :
Mn2+(aq) + H2O2(aq) + 2 OH- (aq) --------------> MnO2(s) + 2 H2O (l)