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Chapter 18: Problem 41

Write a balanced chemical equation to describe how magnesium ions are removed in water treatment by the addition of slaked lime, \(\mathrm{Ca}(\mathrm{OH})_{2}\).

Short Answer

Expert verified
The balanced chemical equation for the removal of magnesium ions in water treatment by the addition of slaked lime is: \(Mg^{2+} + Ca(OH)_2 \rightarrow Mg(OH)_2 + Ca^{2+}\).

Step by step solution

01

Identify the Reactants

In this chemical reaction, the reactants are magnesium ions (Mg虏鈦�) present in the water and slaked lime, calcium hydroxide (Ca(OH)鈧�).
02

Write the Unbalanced Chemical Equation

The unbalanced chemical equation combining magnesium ions and calcium hydroxide can be written as: Mg虏鈦� + Ca(OH)鈧� 鈫� ?
03

Predict the Products of the Reaction

The magnesium ions will combine with the hydroxide ions (OH鈦�) present in the calcium hydroxide and form magnesium hydroxide (Mg(OH)鈧�). However, since calcium ions (Ca虏鈦�) are also present in the reaction, they will remain as a spectator ion, not participating directly in the reaction: Mg虏鈦� + Ca(OH)鈧� 鈫� Mg(OH)鈧� + Ca虏鈦�
04

Balance the Chemical Equation

The balanced chemical equation is: Mg虏鈦� + Ca(OH)鈧� 鈫� Mg(OH)鈧� + Ca虏鈦� Here, the number of atoms of each element is equal on both sides of the equation, which indicates that the reaction is balanced. So, the balanced chemical equation describing how magnesium ions are removed in water treatment by the addition of slaked lime is: Mg虏鈦� + Ca(OH)鈧� 鈫� Mg(OH)鈧� + Ca虏鈦�

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Most popular questions from this chapter

(a) Explain why \(\mathrm{Mg}(\mathrm{OH})_{2}\) precipitates when \(\mathrm{CO}_{3}{ }^{2-}\) ion is added to a solution containing \(\mathrm{Mg}^{2+}\). (b) Will \(\mathrm{Mg}(\mathrm{OH})_{2}\) precipitate when \(40 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) is added to 1.00 L of a solution containing \(125 \mathrm{ppm}\) of \(\mathrm{Mg}^{2+}\) ?

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