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Chapter 16: Problem 28

(a) Write a chemical equation that illustrates the autoionization of water. (b) Write the expression for the ionproduct constant for water, $K_{w} .(\mathbf{c})$ If a solution is described as basic, which of the following is true: (i) \(\left[\mathrm{H}^{+}\right]>\left[\mathrm{OH}^{-}\right]\), (ii) \(\left[\mathrm{H}^{+}\right]=\left[\mathrm{OH}^{-}\right],\) or (iii) \(\left[\mathrm{H}^{+}\right]<\left[\mathrm{OH}^{-}\right] ?\)

Short Answer

Expert verified
(a) The chemical equation for the autoionization of water is: \[ H_2O \rightleftharpoons H^+ + OH^- \] (b) The expression for the ion product constant for water, \(K_w\), is: \[ K_w = [H^+][OH^-] \] (c) For a basic solution, the following condition is true: (iii) \([H^+] < [OH^-]\).

Step by step solution

01

A chemical equation representing autoionization of water

Autoionization of water involves the self-ionization of water molecules into hydronium ions (H+) or protons and hydroxide ions (OH-). The chemical equation can be written as follows: \[ 2H_2O \rightleftharpoons H_3O^+ + OH^- \] Or we can more simply write: \[ H_2O \rightleftharpoons H^+ + OH^- \] In both cases, it depicts the autoionization of water. #b) Writing the expression for the ion product constant for water#
02

Ion product constant expression

The ion product constant for water, denoted as \(K_w\), is the equilibrium constant for the autoionization of water. It is the product of the equilibrium concentrations of H+ ions and OH- ions in water. The expression can be written as: \[ K_w = [H^+][OH^-] \] #c) Identifying the true condition for a basic solution#
03

True condition for a basic solution

A basic solution is characterized by a higher concentration of hydroxide ions (OH-) compared to hydronium ions (H+). Hence, we compare the given options (i), (ii), and (iii) to determine which condition is true for a basic solution: (i) \([H^+] > [OH^-]\): This is true for an acidic solution, not basic. (ii) \([H^+] = [OH^-]\): This is true for a neutral solution, not basic. (iii) \([H^+] < [OH^-]\): This is true for a basic solution, as it indicates the concentration of hydroxide ions is greater than the concentration of hydronium ions. Therefore, option (iii) \([H^+] < [OH^-]\) is true for a basic solution.

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Most popular questions from this chapter

Predict which member of each pair produces the more acidic aqueous solution: (a) \(\mathrm{K}^{+}\) or \(\mathrm{Cu}^{2+}\), (b) \(\mathrm{Fe}^{2+}\) or \(\mathrm{Fe}^{3+}\) (c) \(\mathrm{Al}^{3+}\) or \(\mathrm{Ga}^{3+}\)

At the boiling point of water $\left(100^{\circ} \mathrm{C}\right), K_{w}=5.6 \times 10^{-13} .\( Calculate \)\left[\mathrm{H}^{+}\right]$ and \(\left[\mathrm{OH}^{-}\right]\) for a neutral solution at this temperature.

If a neutral solution of water, with \(\mathrm{pH}=7.00,\) is cooled to \(10^{\circ} \mathrm{C},\) the pH rises to \(7.27 .\) Which of the following three statements is correct for the cooled water: (i) \(\left[\mathrm{H}^{+}\right]>\left[\mathrm{OH}^{-}\right]\) (ii) \(\left[\mathrm{H}^{+}\right]=\left[\mathrm{OH}^{-}\right], \mathrm{or}\) (iii) \(\left[\mathrm{H}^{+}\right]<\left[\mathrm{OH}^{-}\right] ?\)

Calculate the number of \(\mathrm{H}^{+}(a q)\) ions in \(1.0 \mathrm{~mL}\) of pure water at \(25^{\circ} \mathrm{C}\).

Indicate whether each of the following statements is correct or incorrect. (a) Every Brønsted-Lowry acid is also a Lewis acid. (b) Every Lewis acid is also a Bronsted-Lowry acid. (c) Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases. (d) \(\mathrm{K}^{+}\) ion is acidic in water because it causes hydrating water molecules to become more acidic. (e) The percent ionization of a weak acid in water increases as the concentration of acid decreases.
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