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Chapter 15: Problem 126

True or false? Even in a very basic aqueous solution, there are some \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions present. Explain your answer.

Short Answer

Expert verified
True. Even in a very basic aqueous solution, there are some H3O+ ions present. This is because the autoionization of water results in the formation of both H3O+ and OH- ions, maintaining a constant ion product (Kw) at a specific temperature. Even when the concentration of OH- ions is high, the concentration of H3O+ ions cannot become zero, as it would violate the constant Kw value.

Step by step solution

01

Understand Water Autoionization (Dissociation)

In aqueous solutions, water molecules can undergo a process called autoionization or dissociation. In this process, a water molecule loses a proton (H+) to another water molecule, leading to the formation of a hydroxide ion (OH-) and a hydronium ion (H3O+). The reaction can be represented as follows: \[2H_{2}O \rightleftharpoons H_{3}O^{+} + OH^{-}\]
02

Discuss the Equilibrium Constant for Water Dissociation

Since the dissociation of water is a reversible process, it has an equilibrium constant called the ion product of water (Kw). Kw is the product of the concentrations of H3O+ and OH- in a neutral aqueous solution at a specific temperature. At 25°C, the value of Kw is approximately \(1 \times 10^{-14}\). So: \[K_{w} = [H_{3}O^{+}][OH^{-}] = 1 \times 10^{-14}\]
03

Evaluate H3O+ and OH- Concentrations in a Basic Solution

A basic aqueous solution has a greater concentration of OH- ions than H3O+ ions, hence making the solution basic. Since the ion product of water (Kw) must remain constant at a specific temperature: \[[H_{3}O^{+}] = \frac{K_{w}}{[OH^{-}]}\] Even when the concentration of OH- ions is high in a basic solution, the concentration of H3O+ ions cannot become zero because then, the ion product of water (Kw) would not be constant.
04

Conclusion

It is true that even in a very basic aqueous solution, there are some H3O+ ions present. The autoionization of water always results in the formation of both H3O+ and OH- ions, maintaining a constant ion product (Kw) at a specific temperature.

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Most popular questions from this chapter

Does a mixture of carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}\), a weak acid, and sodium bicarbonate, \(\mathrm{NaHCO}_{3}\), in water constitute a buffer? If no, explain why. If yes, explain why and use chemical equations to show what happens when either \(\mathrm{OH}\) or \(\mathrm{H}_{3} \mathrm{O}^{+}\) is added to the solution.

Can a buffer resist \(\mathrm{pH}\) changes for any added amount of strong acid or base? Explain.

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

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?

Are a \(1 \mathrm{M}\) solution of ammonia, \(\mathrm{NH}_{3}\), and a \(1 \mathrm{M}\) solution of lithium hydroxide, I iOH, equally basic, or is one solution more basic than the other? Explain.
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