I am sure I am doing this Acid/Base problem wrong

AI Thread Summary
To determine the pH of the solution created by mixing H2SO4 and Al(OH)3, one must first update the concentrations of both the acid and base in the total volume of 76.3 ml. The neutralization reaction between the acid and base should be written to identify the remaining amounts of H+ or OH-. Calculating the leftover acid or base is crucial, as this will allow for the determination of [H+] or [OH-]. The insolubility of Al(OH)3 complicates the problem, as it may not fully dissociate, making accurate calculations challenging. Understanding the solubility product of Al(OH)3 is essential for solving this problem correctly.
Renee Crosby
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What is the pH of a solution made from 34.6 ml if 3.45*10^-4 M of H2SO4 added to 41.7 ml of 4.56*10^-4 M of Al(OH)3?

I know how to find H+ and OH- and pH I also know how to use x mol / L, but I cannot get them to click together. Everyone keeps telling me to use RICE but my professor never explained what this was to us.

I keep trying different ways to start this problem and they all look wrong. This is the only problem that I don't even know how to put together from the start.
 
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First update the concentrations of acid and base in the total solution of 76,3ml
Then write down the chemical neutralization reaction between the acid and the base.
Then calculate how much acid (or it might be base) that will be left. If it is acid that will be left then you can find [H+]* (and [OH-] will follow)
If it is base that will be left then you can find [OH-] and then [H+].

* have in mind that extra water will be produced from the neutralization reaction so you should update the concentration of the acid left (or base left).
 
What if you were told to start it just as a limiting reagent problem?

But I don't like this question. Unless you are expected to ignore the Al(OH)3 insolubility and to treat the solution as if Al(OH)3 was completely dissociated (which is not true) finding the answer is pretty tricky.
 
Borek said:
What if you were told to start it just as a limiting reagent problem?

But I don't like this question. Unless you are expected to ignore the Al(OH)3 insolubility and to treat the solution as if Al(OH)3 was completely dissociated (which is not true) finding the answer is pretty tricky.
Can we say impossible to solve? The solubility product of Al(OH)3 is absolutely essential.
 

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