Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq)0.0500 M Ca2+(aq) and 0.0260...

Question

Question

Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq)0.0500 M Ca2+(aq) and 0.0260 M Ag+(aq)0.0260 M Ag+(aq).

What will be the concentration of Ca2+(aq)Ca2+(aq) when Ag2SO4(s)Ag2SO4(s) begins to precipitate?

Solubility-product constants, KspKsp, can be found in the chempendix. Ksp values : silver sulfat (1.20x10^-5) calcium sulfate (4.93x10^-5)

[Ca2+]=

Answer 1

Answer #1

Ksp = 1,20x105 = [Agt ? 2 (so,?] W g [Ag+] = 0.0260 M [s042-] = 0.017775M Ksp = 4.93410-5 = [Ca 2+ ] [Son] 2ta 4:93x10-5 0.01

Answer 2

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