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.

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  1. 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.

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