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At a certain temperature, the solubility of strontium arsenate, sr3(aso4)2, is 0.0490 g/l. what is the ksp of this salt at this temperature?

Bethany Evans

in Chemistry

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Justin Parker on September 24, 2018

Sr₃(AsO₄)₂, partially dissociates into its ions as Sr2⁺ and AsO₄3⁻. The balanced equation is Sr₃(AsO₄)₂(s) ⇄ 3Sr2⁺(aq) + 2AsO₄3⁻(aq)X +3X +2XEquilibrium 3X 2XSince the solubility of Sr₃(AsO₄)₂ is 0.0490 g/L, X = 0.0490 g/Lmolar mass of Sr₃(AsO₄)₂ =540.7 g/molHence, X = (0.0490 g/L) / 540.7 g/mol = 9.06 x 10⁻⁵ mol/LKsp = [Sr2⁺(aq)]3 [AsO₄3⁻(aq)]2Ksp = (3X)3 (2X)2Ksp = 108X⁵Ksp = 108 x (9.06 x 10⁻⁵ mol/L)⁵ = 6.59 x 10⁻1⁹ mol⁵/L⁻⁵


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