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Chapter 15: Problem 110

Why aren't ionic compounds like \(\mathrm{NaOH}\) and \(\mathrm{Mg}(\mathrm{OH})_{2}\) weak bases?

Short Answer

Expert verified
Ionic compounds like NaOH and Mg(OH)₂ are not considered weak bases because they completely dissociate in water, forming a high concentration of hydroxide ions. This makes them strong bases, as weak bases are characterized by incomplete dissociation and an equilibrium between the base molecule and its ions.

Step by step solution

01

1. Definition of Weak and Strong Bases

A weak base is a base that does not completely dissociate in water, meaning not all the base molecules break apart into their ions. This results in an equilibrium between the base molecule and its ions. A strong base, on the other hand, is a base that completely dissociates in water, meaning all the base molecules break apart into their ions.
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2. Ionic Compounds

Ionic compounds are formed when a metal and a nonmetal combine, resulting in a compound held together by ionic bonds. Ionic bonds form when atoms transfer electrons to achieve a stable electron configuration. In the case of NaOH, a sodium ion (\(\mathrm{Na^+}\)) forms an ionic bond with a hydroxide ion (\(\mathrm{OH^-}\)).
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3. Dissociation of NaOH and Mg(OH)₂

When ionic compounds dissolve in water, they dissociate into their constituent ions. For example, when sodium hydroxide (\(\mathrm{NaOH}\)) dissolves in water, it dissociates into sodium (\(\mathrm{Na^+}\)) ions and hydroxide (\(\mathrm{OH^-}\)) ions. The same process occurs for magnesium hydroxide (\(\mathrm{Mg(OH)_2}\)), which dissociates into magnesium (\(\mathrm{Mg^{2+}}\)) ions and two hydroxide (\(\mathrm{OH^-}\)) ions. \[ \mathrm{NaOH \rightarrow Na^+ + OH^-} \] \[ \mathrm{Mg(OH)_2 \rightarrow Mg^{2+} + 2OH^-} \]
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4. Strong Base Character

As ionic compounds, both NaOH and Mg(OH)₂ dissociate completely into their respective ions in water. Since the solutions of these ionic compounds contain a high concentration of hydroxide (\(\mathrm{OH^-}\)) ions, they are considered strong bases. The complete dissociation of NaOH and Mg(OH)₂ means that they are not in equilibrium with their ions, which is a characteristic of weak bases. In conclusion, ionic compounds like NaOH and Mg(OH)₂ are not considered weak bases because they dissociate completely in water and form a high concentration of hydroxide ions, making them strong bases.

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Most popular questions from this chapter

Complete the following sentence: "The lower the \(\mathrm{p} K_{\mathrm{a}}\), the (stronger/weaker) the acid." \(^{\prime \prime}\) How does this parallel pH?

What is the \(\mathrm{pH}\) of these aqueous solutions? (a) \(1.0 \mathrm{M} \mathrm{HCl}\), (b) \(0.1 \mathrm{M} \mathrm{HCl}\), (c) \(0.001 \mathrm{M} \mathrm{HCl}\), (d) \(1.0 \times 10^{-5} \mathrm{M} \mathrm{HCl}\), (e) \(1.10 \times 10^{-7} \mathrm{M} \mathrm{HCl}\)

A solution is prepared by dissolving \(2.50\) moles of \(\mathrm{LiOH}\) in enough water to get \(4.00 \mathrm{~L}\) of solution. What are the \(\mathrm{OH}^{-}\) and the \(\mathrm{H}_{3} \mathrm{O}^{+}\) molar concentrations?

What is the molar concentration of hydronium ion and hydroxide ion in pure water at \(25{ }^{\circ} \mathrm{C}\) ?

Based solely on concentrations, when is an aqueous solution judged to be acidic? Give two answers to this question.
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