pH of transition metal ions

[TXpredent]

I ran across a question that was asking the typical "which one of these ionic compounds will have their solubility greatly affected by pH change?" Basically asking which of the following salts are basic/acidic, since acidic salts are more soluble in bases and basic salts are more soluble in acids. My choices were:

a) CuCl
b) AgBr
c) BaF2
d) AgI
e) none of the above

so I went down the list and crossed off all the neutral ions, which are the group I and II metals and Br-, Cl-, I- in these choices. The answer was C. I know that F- is indeed acidic and that Ba is neutral, but what about Cu+ and Ag+? Are transition metals always neutral too?

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[cdbebeau]

I think a, b, and d are insoluble so they would not be affected by pH.

http://www.ausetute.com.au/solrules.html

 

[Worried12345]

F- would be basic because it is an anion by the way

Cations are the acidic ones (exception being the first two groups etc)
Anions are the basic ones (exception being the halogens etc)

Doesn't completely answer your question, however

 

[njohns24]

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[biomolecmed]

Fluorine will be protonated by the acid quickly because it is very electornegative. That will take it out of the products side of the equation and shift the equilibrium towards right side by dissolving more of the reactant.

 

[TXpredent]

Txpredent I'm going to have to quit reading your posts ha. You have a way of confusing me on things I already understand

Sent from my SCH-I500 using SDN Mobile

I'm really sorry man! I'm not trying to! I used to understand this concept pretty well, I'm working on the DAT destroyer for a second time and for some reason this question doesn't make sense anymore.

I think "cdbebeau" cleared it up. I totally forgot that Ag+ and Cu+ are insoluble!

Thanks yall! Please let me know if there's a different explanation!