What is the solubility of silver carbonate (Ag2CO3) in pure water
Let x = solubility in moles/L or M.
Ag2CO3 ==> 2Ag^+ + CO3^2-
...x........2x......x
Ksp = (Ag^+)(CO3^2-)
Substitute Ksp and from the table above and solve for x in moles/L.
To determine the solubility of silver carbonate (Ag2CO3) in pure water, we can refer to solubility rules and use the concept of ionic equations.
1. First, let's write down the balanced chemical equation for the dissociation of silver carbonate in water:
Ag2CO3(s) → 2Ag+(aq) + CO3^2-(aq)
2. According to solubility rules, most carbonates are insoluble in water. However, there are exceptions, such as carbonates of group 1 elements (alkali metals) and ammonium (NH4+), which are soluble.
3. Since silver carbonate is not one of the exceptions mentioned above, we can conclude that it is generally insoluble in water.
4. Therefore, the solubility of silver carbonate in pure water is considered very low, and we can say that it is essentially insoluble.
Please note that while most Ag2CO3 will remain as a solid when mixed with pure water, a very small amount may still dissolve due to the concept of solubility equilibrium. However, the concentration of Ag2CO3 dissolved in water would be extremely low.