What is the coefficient of Fe 3+ when the following reaction is balanced? Bi 3+ (aq) + Fe 3+ (aq) + H 2 O (l) → BiO 3 - (aq) + Fe 2+ (aq) + H + (aq)

Here it says, what is the coefficient of iron 3 ion when the following reaction is balanced? Alright. So first of all, we have the presence of h+ion. This tells me that this is a redox reaction in acidic solution because, remember, the presence of h plus means we have an acid involved in some way. What we need to realize here is that as we're balancing a redox reaction, we add in water and we add in h plus to balance oxygen and hydrogen. Let's take them out for now because as we're balancing we're gonna add them. So what's left represents our most basic redox reaction. Now let's work on balancing it and figure out what the coefficient of iron 3 ion will be. So step 1, look for elements that are not oxygen or hydrogen. Bismuth with bismuth, iron with iron. So here we have b I three plus gives me b I o three minus. F e three plus gives me f e two plus. Now we're gonna balance elements that are not oxygen or hydrogen, 1 bismuth, 1 bismuth, 1 iron, 1 iron, so we're fine. Next, we're gonna balance out oxygens by adding water. We have here 3 oxygens, the other side has none, so add 3 waters. The other half reaction has no oxygens on either side so we don't have to add water. Next, we're gonna add h plus to balance out the number of hydrogens. So that's 3 times 2 is 6, so I'll have to put 6 h plus here. The other half reaction has no hydrogens. Now, balance overall charge, this side here overall is plus 3, this side here is minus 1, and then 6 times plus 1 is plus 6, so it's plus 5 overall. Remember, we're gonna add electrons to the more positively charged side so that it has the same charge at the end as this side. So to go from plus 5 to plus 3, I need to add 2 electrons. Plus 2. I need to add electrons to the more positive plus 2. I need to add electrons to the more positive side, so it has the same overall charge as this side. How do I go from a +3 to a+1 on a+2? I add 1 electron. Now remember your electrons in both half reactions must be the same. We have 2 electrons and 1 electron, So the lowest common multiple between them is 2. So do I have to multiply this whole thing by 2? That would mean that my coefficient in front of iron 3 ion would be 2. So this would be my answer. Here we're not asking for the redo balance redox reaction, all we're asking for is what is the coefficient of iron 3? So you can just stop here. And again the answer would be 2 as a coefficient of Iron 3 ion.

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1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
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BONUS: Mathematical Operations and Functions47m
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13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
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5. Classification & Balancing of Chemical Reactions

Balancing Redox Reactions: Acidic Solutions

GOB Chemistry

5. Classification & Balancing of Chemical Reactions

Balancing Redox Reactions: Acidic Solutions

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Multiple Choice

What is the coefficient of Fe³⁺ when the following reaction is balanced?
Bi³⁺ (aq) + Fe³⁺ (aq) + H₂O (l) → BiO₃^-(aq) + Fe²⁺ (aq) + H⁺ (aq)

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Identify the oxidation states of each element in the reaction. Bi3+ is in the +3 oxidation state, Fe3+ is in the +3 oxidation state, and Fe2+ is in the +2 oxidation state.

Determine the changes in oxidation states. Bi3+ is reduced to BiO3-, and Fe3+ is reduced to Fe2+. This indicates that electrons are transferred in the reaction.

Write the half-reactions for the oxidation and reduction processes. The reduction half-reaction involves Bi3+ gaining electrons to form BiO3-. The oxidation half-reaction involves Fe3+ losing electrons to form Fe2+.

Balance the electrons transferred in the half-reactions. Ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.

Combine the balanced half-reactions to form the overall balanced equation. Adjust the coefficients of each species to ensure mass and charge balance, focusing on the coefficient of Fe3+.