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Question: Please number your questions 1) the dissolution of barium sulfate in water at 25.0 degrees Celsiu...

please number your questions

1) the dissolution of barium sulfate in water at 25.0 degrees Celsius has a ksp value 1.1 x 10^-10. If solid barium sulfate is added to water, calculate the concentration of barium ions when the solution has reach saturation.

Please use ice table

Explanation / Answer

1) The dissolution equillibrium is

BaSO4(s) <----------> Ba2+(aq) + SO42-(aq)

Ksp = [Ba2+ ] [ SO42-] = 1.1×10^-10

ICE

Initial concentration

[Ba2+] =0

[ SO42-] =0

Change in Concentration

[Ba2+ ] = +x

[ SO42- ] = +x

Equillibrium Concentration

[ Ba2+ ] = x

[ SO42- ] = x

Therefore, at equillibrium

x^2 = 1.1×10^-10

x = 1.05×10^-5

[ Ba2+] = 1.05×10^-5 mol/L

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