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Chapter 15: Problem 118

When water undergoes autoionization, is it serving as an acid, a base, or neither? Explain.

Short Answer

Expert verified
During autoionization, water serves as both an acid and a base. This is because one water molecule donates a proton (H⁺) to another water molecule, acting as an acid, while the second water molecule accepts the proton (H⁺), acting as a base. The autoionization of water can be represented by the equation: \(2H_2O \rightleftharpoons H_3O^+ + OH^-\).

Step by step solution

01

Define autoionization of water

Autoionization of water is a chemical equilibrium process in which water molecules dissociate into hydronium ions (H₃O⁺) and hydroxide ions (OH⁻). The process can be represented by the following equation: \[2H_2O \rightleftharpoons H_3O^+ + OH^-\]
02

Define acid and base

According to the Brønsted-Lowry theory, an acid is a substance that donates a proton (H⁺) to another substance, while a base is a substance that accepts a proton (H⁺) from another substance.
03

Determine the role of water in autoionization

In the autoionization equation, we can see that one water molecule donates a proton (H⁺) to another water molecule: \[H_2O + H_2O \rightleftharpoons H_3O^+ + OH^-\] This proton transfer results in the formation of a hydronium ion (H₃O⁺) and a hydroxide ion (OH⁻).
04

Identify water as both an acid and a base

During autoionization, one water molecule acts as an acid because it donates a proton (H⁺) to another water molecule. The second water molecule acts as a base because it accepts the proton (H⁺) from the first water molecule. Therefore, water serves as both an acid and a base during autoionization.

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Most popular questions from this chapter

How many moles of \(\mathrm{Ba}(\mathrm{OH})_{2}\) does it take to neutralize \(0.50\) mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) ? Why does the resulting solution after the neutralization no longer conduct electricity? Why does the solution then conduct electricity after an excess of \(\mathrm{Ba}(\mathrm{OH})_{2}\) is added?

A solution is prepared by dissolving \(2.40 \mathrm{~g}\) of \(\mathrm{Mg}(\mathrm{OH})_{2}\) in enough water to get \(4.00 \mathrm{~L}\) of solution. What are the \(\mathrm{OH}^{-}\) and \(\mathrm{H}_{3} \mathrm{O}^{+}\) molar concentrations? (Hint: You need to calculate the molar mass of \(\mathrm{Mg}(\mathrm{OH})_{2}\).)

Amines are organic compounds that contain an \(\mathrm{NH}_{2}\) group, and water-soluble amines are weak bases in water. For example, the compound methylamine, \(\mathrm{H}_{3} \mathrm{C}-\mathrm{NH}_{2}\), is a weak base. (a) Draw a dot diagram for methylamine. (b) Using dot diagrams, show the equilibrium reaction between methylamine and water. (c) To which side does the equilibrium in part (b) lie? What did we tell you that allowed you to figure out the answer? (d) The similar compound ethane, \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}\), does not act as a weak base. Why can methylamine act as a weak base but \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}\) can't? (Hint: Draw a dot diagram for \(\mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}\).) (e) Is it appropriate to call methylamine an electrolyte? If so, is it weak or strong? Explain.

Why is a pH of 7 equal to neutrality?

The oxide ion, \(\mathrm{O}^{2-}\), present in sodium oxide \(\left(\mathrm{Na}_{2} \mathrm{O}\right)\) reacts violently with water to produce a highly basic solution. The hydride ion, \(\mathrm{H}^{-}\), in sodium hydride (NaH) does the same. (a) Write a balanced total ionic equation for the reaction of sodium oxide with water. (b) In terms of the Bronsted-Lowry definition, how are oxide and hydride similar? (c) What is it about the hydride and oxide ions that allow them to do what they do in water?
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