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Chapter 16: Problem 103

In your own words, define or explain the following terms or symbols: (a) \(K_{\mathrm{w}} ;\) (b) \(\mathrm{pH} ;\) (c) \(\mathrm{p} K_{\mathrm{a}} ;\) (d) hydrolysis; (e) Lewis acid.

Short Answer

Expert verified
\(K_{\mathrm{w}}\) is the ion product of water, pH is a measure of acidity or alkalinity of a solution, \(\mathrm{p}K_{\mathrm{a}}\) is a measure of the strength of an acid in solution, Hydrolysis is a type of chemical reaction that involves the breaking of a bond using water and Lewis acid is a substance that can accept an electron pair.

Step by step solution

01

Define \(K_{\mathrm{w}}\)

\(K_{\mathrm{w}}\) represents the ion product of water. It is the equilibrium constant for the self-ionization of water and its value at 25°C is \(1.0 \times 10^{-14}\). It is defined by the equation \(K_{\mathrm{w}} = [H^+][OH^-]\) where [H+] and [OH-] are the concentrations of hydrogen and hydroxide ions respectively.
02

Define pH

pH is a measure of acidity or alkalinity of a solution. It is the negative logarithm (base 10) of the concentration of H+ ions in a solution. Mathematically, \(\mathrm{pH} = -\log[H^+]\), where [H+] stands for the concentration of H+ ions in the solution.
03

Define \(\mathrm{p}K_{\mathrm{a}}\)

\(\mathrm{p}K_{\mathrm{a}}\) is the negative logarithm (base 10) of the acid dissociation constant (Ka). It provides a measure of the strength of an acid in solution. A lower pKa value indicates a stronger acid.
04

Explain Hydrolysis

Hydrolysis is a type of chemical reaction that involves the breaking of a bond in a molecule using water. In the process, water molecule itself splits into H+ and OH- ions.
05

Define Lewis Acid

Lewis acid is a substance that can accept an electron pair. This definition is based on the Lewis concept of acids and bases, where acids are electron pair acceptors and bases are electron pair donors.

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Most popular questions from this chapter

A 625 mL sample of an aqueous solution containing 0.275 mol propionic acid, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H},\) has \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=0.00239 \mathrm{M} .\) What is the value of \(K_{\mathrm{a}}\) for propionic acid? $$\begin{aligned} &\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}\\\ &&K_{\mathrm{a}}=? \end{aligned}$$

Explain why \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a strong acid solution doubles as the total acid concentration doubles, whereas in a weak acid solution, \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) increases only by about a factor of \(\sqrt{2}\)

Each of the following is a Lewis acid-base reaction. Which reactant is the acid, and which is the base? Explain. (a) \(\mathrm{SO}_{3}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(\operatorname{Zn}(\mathrm{OH})_{2}(\mathrm{s})+2 \mathrm{OH}^{-}(\mathrm{aq}) \longrightarrow\left[\mathrm{Zn}(\mathrm{OH})_{4}\right]^{2-}(\mathrm{aq})\)

Use Lewis structures to diagram the following reaction in the manner of reaction (16.19) $$2 \mathrm{NH}_{3}+\mathrm{Ag}^{+} \longrightarrow\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}$$ Identify the Lewis acid and Lewis base.

Suppose you wanted to produce an aqueous solution of \(\mathrm{pH}=8.65\) by dissolving one of the following salts in water. Which salt would you use, and at what molarity? (a) \(\mathrm{NH}_{4} \mathrm{Cl} ;\) (b) \(\mathrm{KHSO}_{4} ;\) (c) \(\mathrm{KNO}_{2}\); (d) \(\mathrm{NaNO}_{3}\).
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