Question 1

Which of the following is the correct first step when balancing a redox reaction in a basic solution?

Accepted Answer

Break the full reaction into two half-reactions focusing on elements that are not oxygen or hydrogen.

Question 2

When balancing redox reactions in basic solution, after balancing all elements except hydrogen and oxygen, what is the next step?

Accepted Answer

Balance the number of oxygens by adding H$$_2O.$$

Question 3

In the example reaction: $$\mathrm{$$MnO_4$$^- (aq) + NH_4$^+ (aq) \rightarrow $$MnO_2$$ (aq) + NO_3$^- (aq)}$$, which element should you focus on first when splitting into half-reactions?

Accepted Answer

Manganese and Nitrogen

Question 4

After balancing the atoms in each half-reaction, what is the correct way to balance the charge in basic solution?

Accepted Answer

Add OH$$^-$$ ions to both sides.

Question 5

If, after balancing a redox reaction in basic solution, you have H$$^+$$ and OH$$^- on $$the same side, what should you do?

Accepted Answer

Combine them to form H$$_2O.$$

Question 6

Which of the following is TRUE about balancing redox reactions in basic solution compared to acidic solution?

Accepted Answer

You add OH$$^-$$ ions after balancing as if in acid.

Question 7

In the reaction $$\mathrm{H_2O_2 (aq) + $$ClO_2$$ (aq) \rightarrow $$ClO_2$$^- (aq) + O_2$ (g)}$$, which species is being reduced?

Accepted Answer

ClO$$_2$$

Question 8

When balancing the following reaction in basic solution: $$\mathrm{$$ClO_2$$^- (aq) \rightarrow Cl^- (aq) + $$ClO_4$$^- (aq)}$$, what is the oxidation state change for chlorine in ClO$$_2^- to $$ClO$$_4^-$$?

Accepted Answer

From +3 to +7

Question 9

Why is it necessary to multiply the half-reactions by the lowest common multiple when balancing redox reactions?

Accepted Answer

To ensure the number of electrons lost equals the number gained.

Question 10

Which of the following steps is unique to balancing redox reactions in basic solution?

Accepted Answer

Adding OH$$^- to $$both sides to neutralize H$$^+.$$

Question 11

A student balances a redox reaction in acidic solution and then wants to convert it to basic solution. What should they do next?

Accepted Answer

Add OH$$^- to $$both sides for every H$$^+$$ present.

Question 12

In a basic solution, which of the following is used to balance hydrogen atoms in a redox reaction?

Accepted Answer

H$$_2O $$molecules

Question 13

Which statement best describes the role of electrons in balancing redox reactions?

Accepted Answer

Electrons are added to balance the charge in each half-reaction.

Question 14

In the reaction $$\mathrm{$$MnO_4$$^- (aq) + NH_4$^+ (aq) \rightarrow $$MnO_2$$ (aq) + NO_3$^- (aq)}$$, what is the oxidation state of Mn in MnO$$_4^-$$?

Accepted Answer

+7

Question 15

Which of the following is a correct reason for using OH$$^-$$ ions when balancing redox reactions in basic solution?

Accepted Answer

OH$$^-$$ ions neutralize H$$^+$$ ions to form H$$_2O.$$

Question 16

A medical chemist is analyzing a redox reaction in blood, which is a basic environment. What must they remember when balancing the reaction?

Accepted Answer

Add OH$$^-$$ ions to neutralize any H$$^+$$ ions formed.

Question 17

Which of the following is the correct sequence of steps for balancing a redox reaction in basic solution?

Accepted Answer

Split into half-reactions, balance all elements except O and H, balance O with H$$_2O$$, balance H with H$$_2O$$, balance charge with electrons, add OH$$^- to $$neutralize H$$^+$$, combine and simplify.

Question 18

In a laboratory, a student balances the following reaction in basic solution: $$\mathrm{H_2O_2 (aq) + $$ClO_2$$ (aq) \rightarrow $$ClO_2$$^- (aq) + O_2$ (g)}. $$After balancing, the student finds extra H$$^+$$ ions on one side. What should they do?

Accepted Answer

Add OH$$^-$$ ions to both sides to neutralize H$$^+.$$

Balancing Basic Redox Reactions in Basic Solutions

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