Write the solubility equilibria and solubility product expressions for the following:
a. Ag2CO3
b. Ca3(PO4)2
Compounds that produce the same number of ions
CuS Ksp = 8.5x10-45
Ag2S p = 1.6 * 10 - 49
Bi2S3 p = 1.1 * 10 - 73
3. Calculate the solubility of solid CaF2 ( sp=4.0*10. ) in a 0.025 M NaF solution.
Ca3(PO4)2 ==> 3Ca^2+ + 2PO4^3-
Ksp = [Ca^2+]^3[PO4^-3]^2
Ksp is the produce of the concentrations and raise each to the power indicated by the coefficient.
The Ag2CO3 is done the dame way.
For the last question note that the first one is the ONLY one with equal ions.
CuS ==> Cu^2+ + S^2-
Ag2S and Bi2S3 do not produce equation ions.
Sure! Let's start with the solubility equilibria and solubility product expressions for the given compounds:
a. Ag2CO3 (Silver carbonate)
The balanced equation for the dissociation of silver carbonate is:
Ag2CO3(s) ⇌ 2Ag+(aq) + CO3^2-(aq)
The solubility product expression (Ksp) for Ag2CO3 would be:
Ksp = [Ag+]^2 [CO3^2-]
b. Ca3(PO4)2 (Calcium phosphate)
The balanced equation for the dissociation of calcium phosphate is:
Ca3(PO4)2(s) ⇌ 3Ca^2+(aq) + 2PO4^3-(aq)
The solubility product expression (Ksp) for Ca3(PO4)2 would be:
Ksp = [Ca^2+]^3 [PO4^3-]^2
To calculate the solubility product constant (Ksp) for these compounds, you would need to know the values of the concentrations of the respective ions (in square brackets) at equilibrium. These values can be determined experimentally or can be calculated using the solubility of the compounds.
I hope this helps! Let me know if you have any further questions.