indicate whether the following would increase decrease or have no effect on the solubility of copper (ii) carbonate (ksp - 2.5 x 10^-10) when compared to the solubility of water
1. dissolve it in an acidic solution
2. dissolve it in ammonia, forming a complex
3. dissolve it in Cu(CH3COO)2
To clarify: the Ksp is not negative, it is 2.5 x 10^-10. the negative sign is unintentional
This is Le Chatelier's Principle. What do you not understand about. D it? Do you have any ideas what to do?
I believe the second would increase solubility because it forms a complex, but I do not know the pH of copper (ii) carbonate. Because I think the pH would effect solubility
Right b will increase it for the reason you cite.
Adding HCl certainly will increase the solubility.
CuCO3 ==> Cu^2+ + CO3^2-
You will not that adding HCl reacts with the CO3^2- to form H2CO3 which then decomposes to H2O and CO2. So decreasing the (CO3^2-) forces the equilibrium to the right and means more CuCO3 must dissolve to keep the CO3^2- increasing.
Dissolving in Cu(Ac) [Cu(CH3COO)2] will decreases the solubility because of the common ion effect.
CuCO3 ==> Cu^2+ + CO3^2-
Adding Cu(CH3COO)2 adds the Cu^2+ ion. The reaction will shift to the left so as to reduce the added copper ion and means more CuCO3 will precipitate.
To determine whether the given conditions increase, decrease, or have no effect on the solubility of copper (II) carbonate (CuCO3), we can consider the common ion effect and the formation of complex ions. Let's analyze each condition:
1. Dissolve it in an acidic solution:
When copper (II) carbonate is dissolved in an acidic solution, the concentration of hydrogen ions (H+) increases. According to Le Chatelier's principle, this increase in the concentration of H+ shifts the equilibrium towards the formation of carbonic acid (H2CO3). As a result, the solubility of copper (II) carbonate decreases. Therefore, dissolving copper (II) carbonate in an acidic solution would decrease its solubility compared to water.
2. Dissolve it in ammonia, forming a complex:
Ammonia (NH3) can form a complex with copper (II) ions (Cu2+). When copper (II) carbonate is dissolved in ammonia, the copper (II) ions present react with ammonia to form a complex called tetraamminecopper (II) carbonate. This complex is more soluble in water than copper (II) carbonate alone. Therefore, dissolving copper (II) carbonate in ammonia would increase its solubility compared to water.
3. Dissolve it in Cu(CH3COO)2:
Copper (II) acetate (Cu(CH3COO)2) is a salt that dissociates into copper (II) ions and acetate ions when dissolved in water. The presence of excess copper (II) ions in solution may shift the equilibrium of copper (II) carbonate towards the formation of more solid copper (II) carbonate. Therefore, dissolving copper (II) carbonate in Cu(CH3COO)2 would decrease its solubility compared to water.
In summary:
1. Dissolving copper (II) carbonate in an acidic solution decreases its solubility.
2. Dissolving copper (II) carbonate in ammonia increases its solubility.
3. Dissolving copper (II) carbonate in Cu(CH3COO)2 decreases its solubility.