Adding $\ce{HCl}$ to silver nitrate solution causes silver chloride to precipitate. Adding more $\ce{HCl}$ causes the silver to re-dissolve. What is happening to the silver chloride when it re-dissolves?
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The precipitation reaction is: $$\ce {Ag+ + Cl- -> AgCl_{(s)}}$$ The next reaction is: $$\ce {AgCl_{(s)} +Cl- -> AgCl2- }$$
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1$\begingroup$ It might be useful to include the equilibrium constants for the two reactions: AgCl's k_sp is 1.77e-10 (so 5.6e9 for the equation as written), and the k_f for AgCl2- is 1.1e5. $\endgroup$ Nov 8, 2014 at 17:55