The Calculation of K3p for Ag2CO3
How can we calculate the equilibrium constant K3p for Ag2CO3?
With the given information about the solubility of Ag2CO3 in water at 25°C and the value of K3p, how can we determine the equilibrium constant K3p for Ag2CO3?
Calculation of K3p for Ag2CO3
To calculate K3p for Ag2CO3, we need to follow these steps:
- First, write the balanced chemical equation for the dissolution of Ag2CO3 in water.
- Next, use the solubility of Ag2CO3 to determine the molar concentration of Ag2CO3 in solution.
- Then, simplify the equilibrium expression to relate the concentrations of Ag+ and CO32- ions.
- Substitute the solubility product constant Ksp to calculate the equilibrium constant K3p.
- Finally, round the value to two significant digits to obtain the final K3p for Ag2CO3.
The solubility of Ag2CO3 in water at 25°C is reported to be 0.035 g/L. To calculate the equilibrium constant K3p for Ag2CO3, we first determine the molar concentration of Ag2CO3 by converting the solubility to moles per liter.
Given that the molar mass of Ag2CO3 is 275.75 g/mol, the molar concentration of Ag2CO3 at equilibrium is 1.27 × 10^-4 mol/L.
By assuming that the concentration of Ag2CO3 is negligible compared to its ions in solution, we simplify the equilibrium expression and relate the concentrations of Ag+ and CO32- ions using the solubility product expression.
Substituting the solubility product constant Ksp for Ag2CO3, which is 8.1 × 10^-12, into the equation allows us to calculate the equilibrium constant K3p as 6.4 × 10^-9.