[calaren]

Here goes...
I'm working on my U Chem II homework and I'm stuck on the last 2 parts of the last problem. Here they are exactly as written:

You are given a saturated MnCO₃ solution at equilibrium.
D. Upon addition on 3M HCl, what will happen to the concentration of Mn²⁺_(aq)? Hint: What do acids and carbonates do?

E. Upon addition of 0.5M AgNO₃, what will happen to the molar solubility of MnCO₃? Hint: What will happen when Ag⁺ and CO₃^2- are mixed (think K_sp)?

OK, for part D, I know that carbonates neutralize acids - so does that mean that the concentration of Mn²⁺_(aq) will go up since some of the carbonate is going to neutralize the HCl?

For part E, I haven't got a clue - if someone could gently nudge me in the right direction, I'd be so thankful!!

[opti384]

Ag₂CO₃ will precipitate.

[rabolisk]

For E, there are two simultaneous "reactions" going on.

MnCO₃  Mn²⁺ + CO₃^2- and
Ag₂CO₃  2 Ag⁺ + CO₃^2-

both with their own individual K_sp that are not affected by each other. But while the constants are unaffected, both have carbonate.

[calaren]

Rabolisk,
It's Ag₂NO₃ - sorry!

[rabolisk]

My post was not a mistake. AgNO₃ is added but there is no equilibrium going on there because it is a nitrate.