Explanation Given The pH of the solution is 10.17 . The pOH of the solution is calculated by the formula, pOH = 1 4.00 − pH Substitute the value of pH in the above formula. pOH = 1 4.00 − 10.17 = 3.83 The equilibrium reaction between saturated Mg ( OH ) 2 solution and its undissolved form is, Mg ( OH ) 2 ( s ) ⇌ Mg 2 + ( a q ) + 2 OH − ( a q ) The concentration of hydroxyl ion at equilibrium is calculated by the formula, [ OH − ] = 10 ( − pOH ) Where, [ OH − ] is the equilibrium concentration of hydroxyl ions. Substitute the value of pOH in the above formula. [ OH − ] = 10 ( − 3.83 ) = 1.48 × 10 − 4 M It is evident from the above balanced chemical reaction that there must be 2 ions of OH − for 1 ions of Mg 2 + . Thus, the equilibrium concentration of Mg 2 + is calculated by the formula, [ Mg 2 + ] = 1 2 [ OH − ] Where, [ Mg 2 + ] is the equilibrium concentration of Mg 2 +

Chemistry: The Central Science, Books a la Carte Plus MasteringChemistry with eText -- Access Card Package (13th Edition)

13th Edition

ISBN: 9780321934826

Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus

Publisher: PEARSON

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Chapter 3.1, Problem 3.1.2PE

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To determine: The Ksp of Mg(OH)2 in its saturated solution that is in contact with its undissolved form.

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Chapter 3.1, Problem 3.1.1PE

Chapter 3.1, Problem 3.2.1PE

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Chemistry: The Central Science, Books a la Carte Plus MasteringChemistry with eText -- Access Card Package (13th Edition)

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The K s p of Mg ( OH ) 2 in its saturated solution that is in contact with its undissolved form.

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To determine: The Ksp of Mg(OH)2 in its saturated solution that is in contact with its undissolved form.

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Chapter 3 Solutions