4.6 of Ag2SO4 will dissolve in 1L of water. Calculate the solubility product constant for this salt.

Question

please hELP? i got 1.4 x 10^-5 but it says it’s wrong 😔

Answer 1

Hi Jina L.,

First of all,units on your solubility? 4.6 mg? Let's assume g/L. Convert that to M . Then write the individual ion concentrations (note: Ag₂ !), then put them into the Ksp format: Ksp = [Ag]² [SO₄ ] . Now how does it look? By the way, that solubility is quite dependent on temperature (look it up on Google). What does that tell you about the temperature change that occurs when Ag2SO4 dissolves in water? Now, your initial solubility statement: how does it compare with the Google-stated range? Aha! Caught another one!

-- Cheers, --Mr. d.