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Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.16 - Acid-Base EquilibriaProblema 28a
Capitolo 16, Problema 28a

Write a chemical equation that illustrates the autoionization of water.

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Identify the process of autoionization of water, which involves water molecules reacting with each other to form ions.
Write the chemical formula for water: \( \text{H}_2\text{O} \).
Recognize that in autoionization, one water molecule donates a proton (\( \text{H}^+ \)) to another water molecule.
Write the chemical equation for the autoionization: \( 2\, \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_3\text{O}^+(aq) + \text{OH}^-(aq) \).
Understand that this equilibrium process is essential for the concept of pH and the self-ionization constant of water, \( K_w \).

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Autoionization of Water

Autoionization of water refers to the process where two water molecules interact to produce hydronium (H3O+) and hydroxide (OH-) ions. This reaction is essential in understanding the behavior of water as both an acid and a base, and it establishes the foundation for the pH scale, which measures the acidity or basicity of solutions.
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Reaction with Water

Chemical Equations

A chemical equation is a symbolic representation of a chemical reaction, showing the reactants and products along with their respective quantities. In the case of the autoionization of water, the equation is represented as 2 H2O ⇌ H3O+ + OH-, indicating that water can dissociate into its ionic components in a reversible manner.
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Balancing Chemical Equations

Equilibrium in Chemical Reactions

Equilibrium in chemical reactions occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. For the autoionization of water, this equilibrium is crucial as it determines the concentrations of H3O+ and OH- ions in pure water, which are both 1.0 x 10^-7 M at 25°C, leading to a neutral pH of 7.
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Chemical Equilibrium Concepts
Pratica correlata
Domanda del libro di testo

Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow:

(a) NH4+(aq) + OH-(aq) ⇌

(b) CH3COO-(aq) + H3O+(aq) ⇌

(c) HCO3-(aq) + F-(aq) ⇌

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Domanda del libro di testo

Write the expression for the ion product constant for water, Kw.

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Domanda del libro di testo

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M

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Domanda del libro di testo

Calculate [H+] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [OH-] = 0.00045 M (b) [OH-] = 8.8 × 10-9 M (c) a solution in which [OH-] is 100 times greater than [H+].

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