/sci/ - Science & Math

>>9547881
I don't know if I'm an idiot or if this question is poorly worded. I'm trying to learn hydrometallurgy on my own so I don't have a prof to bug about this.

>Determine the equilibrium concentration of Ag+ and the equilibrium pH when when 0.05 mol of AgNO3 are added to 1000 g of water with an initial pH of 12.3,
I think I could figure this out. I have silver ions, I have nitrate ions, I can use Gibb's free energy to determine the activity ratio of my ions in solution. I'm not sure how the pH got to be 12.3 (maybe NaOH is in there?) but I can accept that.

>Assume I = 0.1.
Okay, so I can use the Debye-Huckel equation to figure out what my activity coefficient ought to be. This isn't too bad.

>assuming the only product is Ag(OH).
Wait, what? What happened to the Nitrate? Is the nitrate just not a part of this equation? The fact that the only product is Ag(OH) makes me want to think the equilibrium I want to worry about is Ag+ + OH- <-> AgOH, but then why was I told about the nitrate?

Can anybody help me out with this?