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Chapter 15: Problem 192

Other than water, what would you expect to find in the highest concentration in an aqueous solution of \(\mathrm{Ca}(\mathrm{OH})_{2} ?\) Explain.

Short Answer

Expert verified
In an aqueous solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\), other than water, the hydroxide ion (\(\mathrm{OH}^-\)) would be present in the highest concentration. This is because the dissociation of \(\mathrm{Ca}(\mathrm{OH})_{2}\) in water produces one mole of calcium ions (\(\mathrm{Ca}^{2+}\)) and two moles of hydroxide ions (\(\mathrm{OH}^-\)) for every mole of \(\mathrm{Ca}(\mathrm{OH})_{2}\) dissolved.

Step by step solution

01

Write the Dissociation Equation of \(\mathrm{Ca}(\mathrm{OH})_{2}\)

First, we need to write the balanced chemical equation for the dissociation of \(\mathrm{Ca}(\mathrm{OH})_{2}\) in water: \(\mathrm{Ca}(\mathrm{OH})_{2} \longrightarrow \mathrm{Ca}^{2+}(aq) + 2\mathrm{OH}^-(aq)\) This equation shows that for every one mole of calcium hydroxide that dissolves in water, one mole of calcium ions (\(\mathrm{Ca}^{2+}\)) and two moles of hydroxide ions (\(\mathrm{OH}^-\)) are produced.
02

Analyze the Dissociation Ratio

From step 1, we can deduce that the ratio of the ions produced when \(\mathrm{Ca}(\mathrm{OH})_{2}\) dissolves in water is: \(\frac{1\ \text{mol}\; \mathrm{Ca}^{2+} }{1\ \text{mol}\ \mathrm{Ca}(\mathrm{OH})_{2}} \quad \text{and} \quad \frac{2\ \text{mol}\; \mathrm{OH}^-}{1\ \text{mol}\ \mathrm{Ca}(\mathrm{OH})_{2}}\) Here, we see that the concentration of hydroxide ions (\(\mathrm{OH}^-\)) is double to the concentration of calcium ions (\(\mathrm{Ca}^{2+}\)) when the same amount of \(\mathrm{Ca}(\mathrm{OH})_{2}\) is dissolved in water.
03

Identify the Ion with the Highest Concentration

Based on the dissociation ratio that we obtained in step 2, it is now clear that hydroxide ions (\(\mathrm{OH}^-\)) are produced in the highest concentration when \(\mathrm{Ca}(\mathrm{OH})_{2}\) dissolves in water. So, other than water, the hydroxide ion (\(\mathrm{OH}^-\)) is the component we would expect to find in the highest concentration in an aqueous solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\).

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Most popular questions from this chapter

If pure water has both hydronium ions (acid) and hydroxide ions (base) in it, how can it be neutral?

A solution is formed by mixing \(50.0 \mathrm{~mL}\) of \(0.015 \mathrm{M} \mathrm{NaOH}(a q)\) with \(50.0 \mathrm{~mL}\) of \(0.010 \mathrm{M}\) \(\mathrm{HNO}_{3}(a q)\) (a) Is the solution acidic or basic? (b) Draw a beaker and show all species present in the solution. (c) What is the pH of the solution?

You mix \(500 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{NaOCl}\) with \(500 \mathrm{~mL}\) of \(0.500 \mathrm{MHNO}_{3}\). Write an equation for the reaction that occurs. Besides water, what species are in the solution after reaction? Is this solution a buffer?

How does a buffer "kill" added strong base?

Aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), is a weak base, with a lone pair of electrons on the nitrogen atom. (a) According to Bronsted and Lowry, what must aniline do to act as a base? (b) Why can aniline act as a base? (c) What are the molecular formula and charge of the conjugate acid of aniline?
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