[Null Hikari]

Hi there, am new to these forums and I need some help with this problem

Calculate the potential needed for copper to start precipitating from a solution containing (0.01 M) of CuSO4 with ((enough H2SO4 for pH to be 4)).

I tried my best doing this (see attached image)
but in the end i doubt i even got the right half reactions.

no data about standard reduction potentials is given within the problem, thus there is no hint to that.

Any help would be appreciated

[Borek]

Question asks only about a potential necessary for the copper half reaction to work, and if no other information is given you should report the potential as measured against the SHE.

[Null Hikari]

if that was the case then what does pH have to do with things?

I do know that pH affects some redox reactions, but in this case where there's only a half reaction then does it even matter?.

[Borek]

IMHO pH doesn't matter here - acid is added just to prevent copper hydroxide precipitation.

To be sure you may want to check what is the Ksp of Cu(OH)₂, and what is the maximum possible concentration of Cu²⁺ in your solution.

[Null Hikari]

Thanks for your help  .