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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 (Mg²⁺) present in the water and slaked lime, calcium hydroxide (Ca(OH)₂).
02

Write the Unbalanced Chemical Equation

The unbalanced chemical equation combining magnesium ions and calcium hydroxide can be written as: Mg²⁺ + Ca(OH)₂ → ?
03

Predict the Products of the Reaction

The magnesium ions will combine with the hydroxide ions (OH⁻) present in the calcium hydroxide and form magnesium hydroxide (Mg(OH)₂). However, since calcium ions (Ca²⁺) are also present in the reaction, they will remain as a spectator ion, not participating directly in the reaction: Mg²⁺ + Ca(OH)₂ → Mg(OH)₂ + Ca²⁺
04

Balance the Chemical Equation

The balanced chemical equation is: Mg²⁺ + Ca(OH)₂ → Mg(OH)₂ + Ca²⁺ 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: Mg²⁺ + Ca(OH)₂ → Mg(OH)₂ + Ca²⁺

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Most popular questions from this chapter

One of the possible consequences of global warming is an increase in the temperature of ocean water. The oceans serve as a "sink" for \(\mathrm{CO}_{2}\) by dissolving large amounts of it. (a) How would the solubility of \(\mathrm{CO}_{2}\) in the oceans be affected by an increase in the temperature of the water? (b) Discuss the implications of your answer to part (a) for the problem of global warming.

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In 1986 an electrical power plant in Taylorsville, Georgia, burned \(8,376,726\) tons of coal, a national record at that time. (a) Assuming that the coal was \(83 \%\) carbon and \(25 \%\) sulfur and that combustion was complete, calculate the number of tons of carbon dioxide and sulfur dioxide produced by the plant during the year. (b) If \(55 \%\) of the \(\mathrm{SO}_{2}\) could be removed by reaction with powdered \(\mathrm{CaO}\) to form \(\mathrm{CaSO}_{3}\), how many tons of \(\mathrm{CaSO}_{3}\) would be produced?
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