posted by Paul .
The maximum solubility of silver sulfate, Ag2SO4 [molar mass = 312], is 4.50 g/L at 25°C. Silver sulfate dissociates by the reaction below:
Ag2SO4(s) <--> 2 Ag+ (aq)+ SO4¯² (aq)
1.What are the [Ag+] and [SO4¯²] in a saturated solution of silver sulfate made by dissolving excess solid in distilled water at 25°C?
2.Write the Ksp expression for silver sulfate and calculate its value at 25°C.
3.Will precipitation of silver sulfate occur if 0.100 mol of silver ions are added to 2500.0 ml of 0.100M sulfuric acid, H2SO4 ? Show calculations to support your conclusion.
1. Convert solubility in g/L to moles/L for Ag2SO4. Then (SO4^-) = (Ag2SO4) and (Ag^+) will be 2x that.
2. Ksp = (Ag^+)^2(SO4^-2)
3. Calculate Qsp and compare to Ksp.
Post your work if you get stuck.