Galvanic cells: H+ vs H2SO4, and Br2(aq) vs Br2(l)

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In galvanic cell reactions, H2SO4(aq) is used to provide a stable source of protons (H+) in the cathode, while H+(aq) can be present at both the cathode and anode depending on the reaction specifics. The choice between H2SO4(aq) and H+(aq) often hinges on the need for a strong acid to facilitate proton transfer in redox reactions. Br2(aq) is preferred over Br2(l) in galvanic cells because its electrode potential is influenced by concentration, which is fixed in a saturated solution, ensuring consistent potential. The redox properties of H2SO4 are significant as it acts as a proton donor, simplifying the analysis of reactions. Understanding these distinctions is crucial for accurately describing galvanic cell behavior.
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For the reaction 12H+ + 2 IO(3-) + 10 Fe(2+) - > I2 + 6 H2O + 10 Fe(3+), the solution says that H2SO4(aq) is in the cathode. For the reaction 2 H2O2 - > O2 + 2 H2O, the solution says that H+(aq) is in the cathode and anode. When is H2SO4(aq) or H+(aq) more appropriate in the galvanic cell description?

Also, why is Br2(aq) in galvanic cells rather than Br2(l)?

Thanks.
 
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i_love_science said:
Also, why is Br2(aq) in galvanic cells rather than Br2(l)?
Not sure why H2SO4(aq) rather than H+(aq).
Br2(aq) has electrode potential that depends on its concentration in solution. In saturated solution in equilibrium with Br2(l), the concentration of Br2(aq) is fixed by solubility and potential should be the same for Br2(aq) as for Br2(l).
 
H2SO4 acts very much as a proton donor in redox chemistry and the redox properties of its deprotonated forms can often be neglected AFAIK.
 
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