Trying to Convert an Equation into an Ionic Equation

In summary, when lead and sulfur are mixed together, lead forms a solid solution with sulfur. The lead and sulfur are both solids, so the lead battery cannot work as intended.
  • #1
student34
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Homework Statement



PbSO4(aq) >>> Pb(s) + PbO2(aq) + S042-(aq)

Homework Equations



The Attempt at a Solution



PbSO4(aq) must be Pb2+(aq) SO42-

But PbO2(aq) seems to have to be Pb4+(aq) + 2O-(aq)

How can Pb go from Pb2+(aq) to Pb4+(aq); doesn't it have to keep the same charge?
 
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  • #2
Both PbSO4 and PbO2 are solids.

Note that there is no way to balance the equation as written - charge is only on one side.
 
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  • #3
Borek said:
Both PbSO4 and PbO2 are solids.

Note that there is no way to balance the equation as written - charge is only on one side.

I'm sorry. I just noticed in brackets it says that they are soluble because they are in an acid solution.
 
  • #4
Then the box is simply not true - please read about how the lead battery works. Its construction is based on the fact both these substances are solids immersed in the concentrated sulfuric acid.
 
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  • #5
Borek said:
Then the box is simply not true - please read about how the lead battery works. Its construction is based on the fact both these substances are solids immersed in the concentrated sulfuric acid.

Thanks for the reassurance, it must be another mistake in my textbook.
 
  • #6
When you say it has to keep the same charge, no it does not - you also have Pb metal in there which has another charge (0). In fact not having the same charge is of the essence in oxidation of metals isn't it? and in the lead-acid battery you do have three levels of lead oxidation involved.
It might help to try the formal non-ionic equation first, but you can't do it with what you've got in yours - you also need H2O.
Then try to get the ionic one. Include H+. You are also allowed to use HSO4-. Spend a little time to try and get it, because if you do that first and then look it up it might click whereas if you only look it up you will say yes yes and forget it by next time. It is quite tricky.

There is an account of this quite important application in links here: https://www.physicsforums.com/threa...ipitation-of-unknown-ion.790077/#post-4980286
 
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FAQ: Trying to Convert an Equation into an Ionic Equation

1. What is an ionic equation?

An ionic equation is a chemical equation that shows the formation of ionic compounds in a reaction. It separates the reactants and products into their respective ionic components.

2. How do you convert a regular equation into an ionic equation?

To convert an equation into an ionic equation, first determine the states of matter for each element or compound. Then, break up any ionic compounds into their individual ions. Finally, balance the equation and include the charges for each ion.

3. Why is it important to convert an equation into an ionic equation?

Converting an equation into an ionic equation allows us to see the individual ions involved in a reaction and their charges. This is important for understanding the mechanism of a reaction and predicting the products.

4. Can all equations be converted into ionic equations?

No, not all equations can be converted into ionic equations. Only reactions that involve ionic compounds can be represented by ionic equations. Covalent compounds do not dissociate into ions and therefore cannot be represented by ionic equations.

5. Are there any shortcuts or tricks for converting equations into ionic equations?

Yes, there are a few shortcuts that can make converting equations into ionic equations easier. These include recognizing common polyatomic ions, knowing the solubility rules for ionic compounds, and being familiar with common strong acids and bases.

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