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Chapter 8: Problem 53

Describe the process by which water self-ionizes, and explain why pure water is considered to be neutral.

Short Answer

Expert verified
Water self-ionizes into H鈧僌鈦� and OH鈦�, maintaining equal concentrations, resulting in a neutral pH of 7.

Step by step solution

01

Water Molecule Structure

Water (H鈧侽) is made up of two hydrogen atoms and one oxygen atom. These atoms share electrons in covalent bonds, with the oxygen atom possessing a partial negative charge and the hydrogen atoms possessing partial positive charges.
02

Self-Ionization Process

During self-ionization, a small fraction of water molecules interact with each other. In this process, one water molecule donates a proton (H鈦�) to another water molecule, leading to the formation of a hydronium ion (H鈧僌鈦�) and a hydroxide ion (OH鈦�). This can be represented by the equation: H鈧侽 + H鈧侽 鈬� H鈧僌鈦� + OH鈦� This process occurs naturally in water.
03

Equilibrium in Pure Water

The self-ionization reaches an equilibrium where the concentration of hydronium ions [H鈧僌鈦篯 equals the concentration of hydroxide ions [OH鈦籡. Each has a concentration of approximately 1.0 脳 10鈦烩伔 M at 25掳C, which maintains the condition of neutrality in pure water.
04

Neutral pH of Pure Water

The pH is a measure of the concentration of hydronium ions. At equilibrium in pure water, the pH is calculated using the formula: pH = -log([H鈧僌鈦篯) Since [H鈧僌鈦篯 is 1.0 脳 10鈦烩伔, the pH is 7. Being midway between 0 and 14 on the pH scale, this indicates that pure water is neutral.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Water Molecule Structure
Water, represented chemically as H鈧侽, consists of two hydrogen atoms bonded to one oxygen atom. This is a classic example of a covalent bond, where atoms share electrons. Oxygen, being more electronegative, draws these shared electrons closer, resulting in a slight negative charge. Meanwhile, hydrogen atoms gain a slight positive charge.
The unique shape of the water molecule, with its bent structure, is due to the angle formed by the hydrogen-oxygen-hydrogen atoms. This leads to water's polar nature. Its polarity causes water molecules to attract each other, a fundamental property for many of water鈥檚 behaviors.
Hydronium Ions
When discussing water's self-ionization, hydronium ions (H鈧僌鈦�) play a central role. A hydronium ion is formed when a water molecule (H鈧侽) accepts a proton (H鈦�) from another water molecule.
This results in the hydronium ion, H鈧僌鈦�, alongside the creation of a hydroxide ion (OH鈦�).
  • The formula representing this interaction is H鈧侽 + H鈦� 鈫� H鈧僌鈦�.
  • This process is reversible and happens continually in water.
The presence of hydronium ions is what defines the acidity or basicity of the solution measured through the pH scale.
Hydroxide Ions
Hydroxide ions (OH鈦�) are another product of water's self-ionization. These ions form when one water molecule loses a proton, parallel to the production of hydronium ions. The equation indicating the formation of hydroxide ions is quite simple:
  • H鈧侽 - H鈦� 鈫� OH鈦�
This remains a critical component in understanding water's neutral nature.
While hydronium ions influence acidity, hydroxide ions contribute to the basic properties of a solution.
Neutral pH
A neutral pH of 7 is a significant concept for students to grasp, especially when it comes to pure water. Pure water is said to be neutral because it contains equal concentrations of hydronium and hydroxide ions. At 25掳C, both [H鈧僌鈦篯 and [OH鈦籡 are approximately 1.0 脳 10鈦烩伔 M, balancing out the acidic and basic properties perfectly.
  • The pH is calculated using the formula: pH = -log([H鈧僌鈦篯)
  • With a concentration of 1.0 脳 10鈦烩伔 M, the resulting pH is exactly 7.
This balance is key to the definition of neutrality in pure water.
Equilibrium in Water
Water's self-ionization involves a dynamic equilibrium that ensures the concentration of hydronium and hydroxide ions remains constant. This equilibrium reflects the natural tendency for chemical reactions to occur at certain rates until a balance of reactants and products is achieved. In the context of water:
  • The self-ionization of water is represented as H鈧侽 + H鈧侽 鈬� H鈧僌鈦� + OH鈦�.
  • At equilibrium, the rates of the forward and reverse reactions are equal.
This equilibrium allows water to sustain its neutral pH, providing an environment where acidity and basicity are balanced.

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Most popular questions from this chapter

Which statement below is true? Explain. a. All Arrhenius bases are also Br酶nsted-Lowry bases. b. All Br酶nsted-Lowry bases are also Arrhenius bases.

Explain why the hydrogen phosphate ion \(\left(\mathrm{HPO}_{4}^{2-}\right)\) is amphoteric.

Indicate whether solutions with the following \(\mathrm{pH}\) values are acidic, basic, or neutral. a. \(\mathrm{pH}=9.4\) b. \(\mathrm{pH}=7.0\) c. \(\mathrm{pH}=5.0\)

Calculate how many grams of each solute would be required in order to make the given solution. a. \(3.40 \mathrm{~L}\) of a \(0.780 \mathrm{M}\) solution of iron(III) chloride, \(\mathrm{FeCl}_{3}\) b. \(60.0 \mathrm{~mL}\) of a \(4.10 \mathrm{M}\) solution of calcium acetate, \(\mathrm{Ca}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\)

Write the formula of each base's conjugate acid. a. \(\mathrm{BrO}_{3}^{-}\) b. \(\mathrm{NH}_{3}\) c. \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) d. \(\mathrm{HCO}_{3}^{-}\) e. \(\mathrm{CN}^{-}\) f. \(\mathrm{HPO}_{4}^{2-}\) g. HS- \(\mathrm{h} . \mathrm{SO}_{4}^{2-}\) i. \(\mathrm{CO}_{3}^{2-}\) \(\mathrm{j} . \mathrm{HCO}_{3}^{-}\) k. \(\mathrm{PH}_{3}\)
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