Skip to Content

Common Ion ICE

How many moles of Mg(OH)2_2 can be dissolved in a 1 L solution that already contains 0.52 moles Mg2+^{2+}.

Mg(OH)2_2 Ksp_{sp} = 8.9 x 1012^{-12}

Posted by Mike Pruitt 8 months ago

Related Problems

Calculate the solubility (in grams per liter) of PbI2_2 in water from the solubility product constant 1.4 x 108^{-8}.

What are the concentrations of the ionic species in a saturated solution of Ag2_2CrO4_4

Ksp_{sp} = 1.1 x 1012^{-12}

Calculate the equilibrium concentration of Pb2+^{2+}, I^-, Na(\^+,andNO, and NO_3^-when100.0mLof0.0500MPb(NO when 100.0 mL of 0.0500 M Pb(NO_3))_2## and 200.0 mL of 0.100 M NaI are mixed.

PbI2_2 Ksp_{sp} = 1.4 x 108^{-8}

The solubility of Ce(IO3_3)3_3 in a 0.20 M KIO3_3 solution is 4.4 x 108^{-8} mol/L. Calculate Ksp_{sp} for Ce(IO3_3)3_3.