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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, \(\mathrm{Ca}(\mathrm{OH})_{2}\), is: \[2\mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_2 \rightarrow 2\mathrm{Mg}(\mathrm{OH})_2 + \mathrm{Ca}^{2+}\]

Step by step solution

01

Identify the Reactants

In this reaction, the reactants are magnesium ions in water (suppose as \(\mathrm{Mg}^{2+}\)) and slaked lime, \(\mathrm{Ca}(\mathrm{OH})_{2}\).
02

Write the Unbalanced Reaction

In this step, we combine the reactants to form the products. Calcium in \(\mathrm{Ca}(\mathrm{OH})_{2}\) will react with magnesium ions to form solid magnesium hydroxide \(\mathrm{Mg}(\mathrm{OH})_{2}\) and aqueous calcium ions \(\mathrm{Ca}^{2+}\). The unbalanced reaction is: \(\mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_2 \rightarrow \mathrm{Mg}(\mathrm{OH})_2 + \mathrm{Ca}^{2+}\)
03

Balance the Chemical Equation

We will now balance the chemical equation, ensuring the number of atoms of each element is the same on both sides of the equation. There are equal numbers of magnesium, calcium, and oxygen atoms on both sides of the equation, but the number of hydrogen atoms is not equal. We need to balance the hydrogen atoms by multiplying the \(\mathrm{Mg}^{2+}\) ions by 2. Balanced chemical equation: \(2\mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_2 \rightarrow 2\mathrm{Mg}(\mathrm{OH})_2 + \mathrm{Ca}^{2+}\) Now, the number of atoms for each element is the same on both sides. The balanced chemical equation is: \[2\mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_2 \rightarrow 2\mathrm{Mg}(\mathrm{OH})_2 + \mathrm{Ca}^{2+}\]

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Most popular questions from this chapter

(a) With respect to absorption of radiant energy, what distinguishes a greenhouse gas from a nongreenhouse gas? (b) \(\mathrm{CH}_{4}\) is a greenhouse gas, but \(\mathrm{Ar}\) is not. How might the molecular structure of \(\mathrm{CH}_{4}\) explain why it is a greenhouse gas?

Why is rainwater naturally acidic, even in the absence of polluting gases such as \(\mathrm{SO}_{2} ?\)

Natural gas consists primarily of methane, \(\mathrm{CH}_{4}(\mathrm{~g})\). (a) Write a balanced chemical equation for the complete combustion of methane to produce \(\mathrm{CO}_{2}(g)\) as the only carbon-containing product. (b) Write a balanced chemical equation for the incomplete combustion of methane to produce \(\mathrm{CO}(g)\) as the only carbon-containing product. (c) At \(25^{\circ} \mathrm{C}\) and \(1.0\) atm pressure, what is the minimum quantity of dry air needed to combust \(1.0 \mathrm{~L}\) of \(\mathrm{CH}_{4}(\mathrm{~g})\) completely to \(\mathrm{CO}_{2}(\mathrm{~g})\) ?

A reaction that contributes to the depletion of ozone in the stratosphere is the direct reaction of oxygen atoms with ozone: $$\mathrm{O}(\mathrm{g})+\mathrm{O}_{3}(g) \longrightarrow 2 \mathrm{O}_{2}(g)$$ At \(298 \mathrm{~K}\) the rate constant for this reaction is \(4.8 \times 10^{5} \mathrm{M}^{-1} \mathrm{~s}^{-1}\). (a) Based on the units of the rate constant, write the likely rate law for this reaction. (b) Would you expect this reaction to occur via a single elementary process? Explain why or why not. (c) From the magnitude of the rate constant, would you expect the activation energy of this reaction to be large or small? Explain. (d) Use \(\Delta H_{f}^{\circ}\) values from Appendix \(C\) to estimate the enthalpy change for this reaction. Would this reaction raise or lower the temperature of the stratosphere?

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