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(a)
Interpretation:
The balanced equations for the following reaction in basic solution needs to be determined.
Concept introduction:
Here are the rules to
- Determine the oxidation numbers of the elements and write the oxidation and reduction half equation.
- Balance the atoms of elements other than O and H. Use H2 O to balance O, H+ to balance H, electrons to balance the charges. Equalize the number of electrons on both the half reactions and then add the half reactions.
- Add OH- to neutralize the excess protons since this is a basic medium. Add OH- to both side of the equation to balance it.
![Check Mark](/static/check-mark.png)
Answer to Problem 7QAP
Explanation of Solution
Determining the oxidation numbers:
The oxidation number of I in I2 and I- is 0 and -1 respectively. As the oxidation number of I is decreasing this is the reduction half reaction.
Reduction half reaction:
Oxidation half reaction:
To balance the excess O atoms on the product side we add one H2 O on the reactant side, and then we balance the excess H atom on the reactant side by adding two H+ on the product side. Finally, we balance the charge by adding two electrons to the product side of the half reaction.
Thus, the balanced oxidation half reaction:
Now, balance the charge by adding two electrons to the reactant side of the half reaction.
Thus, the balanced reduction half reaction:
Net reaction:
By adding both the half reaction, the net reaction is obtained as follows:
Basic medium:
Since the reaction takes place in basic medium the excess proton on the reactant side of the net reaction is neutralized with OH-. 2 OH- ions are added on both side of the equation to even out the charges. H+ and OH- combines to form H2 O, which is then cancelled out on both side of the net reaction.
Thus, the balanced net reaction in the basic medium will be:
Or,
(b)
Interpretation:
The balanced equations for the following reaction in basic solution needs to be determined.
Concept introduction:
Here are the rules to balance
- Determine the oxidation numbers of the elements and write the oxidation and reduction half equation.
- Balance the atoms of elements other than O and H. Use H2 O to balance O, H+ to balance H, electrons to balance the charges. Equalize the number of electrons on both the half reactions and then add the half reactions.
- Add OH- to neutralize the excess protons since this is a basic medium. Add OH- to both side of the equation to balance it.
![Check Mark](/static/check-mark.png)
Answer to Problem 7QAP
Explanation of Solution
Determining the oxidation numbers:
The oxidation number of Zn in Zn and Zn2+ is 0 and +2 respectively. As the oxidation number of Zn is increasing this is the oxidation half of the reaction.
Oxidation half reaction:
Reduction half reaction:
Balance the charge by adding two electrons to the product side of the half reaction.
Thus, the balanced oxidation half reaction will be:
To balance the excess O atoms on the product side we add three H2 O on the product side, and then we balance the excess H atom on the product side by adding nine H+ on the reactant side. Finally, we balance the charge by adding eight electrons to the reactant side of the half reaction.
Thus, the balanced reduction half reaction will be:
Net reaction:
Multiply the oxidation half reaction by 4, to cancel out the electrons in the net reaction. We add both the half reaction to get the net reaction.
Basic medium:
Since the reaction takes place in basic medium the excess proton on the reactant side of the net reaction is neutralized with OH-. OH- is added on both side of the equation to even out the charges. H+ and OH- combines to form H2 O, which is then cancelled out on both side of the net reaction. Thus, the balanced net reaction will be:
Or,
(c)
Interpretation:
The balanced equations for the following reaction in basic solution needs to be determined.
Concept introduction:
Here are the rules to balance redox reactions in basic medium:
- Determine the oxidation numbers of the elements and write the oxidation and reduction half equation.
- Balance the atoms of elements other than O and H. Use H2 O to balance O, H+ to balance H, electrons to balance the charges. Equalize the number of electrons on both the half reactions and then add the half reactions.
- Add OH- to neutralize the excess protons since this is a basic medium. Add OH- to both side of the equation to balance it.
![Check Mark](/static/check-mark.png)
Answer to Problem 7QAP
Explanation of Solution
Determining the oxidation numbers:
The oxidation number of Cl in ClO- and Cl- is +1 and -1 respectively. As the oxidation number of Cl is decreasing this is the reduction half of the reaction.
The reduction half reaction:
Oxidation half reaction:
To balance the excess O atoms on the product side we add two H2 O on the reactant side, and then we balance the excess H atom on the reactant side by adding four H+ on the product side. Finally, we balance the charge by adding three electrons to the reactant side of the half reaction.
Thus, the balanced oxidation half reaction will be:
Similarly, to balance the excess O atoms on the reactant side we add one H2 O on the product side, and then we balance the excess H atom on the product side by adding two H+ on the reactant side. Finally, we balance the charge by adding two electrons to the reactant side of the half reaction.
Thus, the balanced reduction half reaction will be:
Net reaction:
Multiply the oxidation half reaction by 2 and reduction half reaction by 3, to cancel out the electrons in the net reaction. We add both the half reaction to get the net reaction.
Basic medium:
Since the reaction takes place in basic medium the excess proton on the reactant side of the net reaction is neutralized with OH-. OH- is added on both side of the equation to even out the charges. H+ and OH- combines to form H2 O, which is then cancelled out on both side of the net reaction.
Or,
(d)
Interpretation:
The balanced equations for the following reaction in basic solution needs to be determined.
Concept introduction:
Here are the rules to balance redox reactions in basic medium:
- Determine the oxidation numbers of the elements and write the oxidation and reduction half equation.
- Balance the atoms of elements other than O and H. Use H2 O to balance O, H+ to balance H, electrons to balance the charges. Equalize the number of electrons on both the half reactions and then add the half reactions.
- Add OH- to neutralize the excess protons since this is a basic medium. Add OH- to both side of the equation to balance it.
![Check Mark](/static/check-mark.png)
Answer to Problem 7QAP
Explanation of Solution
Determining the oxidation numbers:
The oxidation number of K in K and K+ is 0 and +1 respectively. As the oxidation number of K is increasing this is the oxidation half of the reaction.
Oxidation half reaction:
Reduction half reaction:
Balance the charge by adding one electron to the product side of the half reaction.
Thus, the balanced oxidation half reaction will be:
To balance the excess O atoms on the reactant side we add one H2 O on the product side, and then we balance the excess H atom on the product side by adding two H+ on the reactant side. Finally, we balance the charge by adding two electrons to the reactant side of the half reaction.
Thus, the balanced reduction half reaction will be:
Net reaction:
Multiply the oxidation half reaction by 2, to cancel out the electrons in the net reaction. We add both the half reaction to get the net reaction.
Basic medium:
Since the reaction takes place in basic medium the excess proton on the reactant side of the net reaction is neutralized with OH-. OH- is added on both side of the equation to even out the charges. H+ and OH- combines to form H2 O, which is then cancelled out on both side of the net reaction.
Or,
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Chapter 17 Solutions
Chemistry: Principles and Reactions
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