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Chapter 14: Problem 166

Rank the following \(0.10 M\) solutions in order of increasing pH. a. \(\mathrm{NH}_{3}\) d. \(\mathrm{KCl}\) b. \(\mathrm{KOH}\) e. \(\mathrm{HCl}\) c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

Short Answer

Expert verified
The order of increasing pH for the given 0.10 M solutions is: e. \(\mathrm{HCl}\), c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\), d. \(\mathrm{KCl}\), a. \(\mathrm{NH}_{3}\), and b. \(\mathrm{KOH}\).

Step by step solution

01

Identify the nature of each solution

Begin by identifying the nature of each given compound (acidic, basic, or neutral) when dissolved in water. a. \(\mathrm{NH}_{3}\) - Ammonia is a weak base. d. \(\mathrm{KCl}\) - Potassium chloride is a neutral salt. b. \(\mathrm{KOH}\) - Potassium hydroxide is a strong base. e. \(\mathrm{HCl}\) - Hydrochloric acid is a strong acid. c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) - Acetic acid is a weak acid.
02

Compare acidic and basic strengths

Now we need to compare the acidic and basic strengths of these compounds: Strong acids, like HCl, will have the lowest pH. Among bases, the strong base (KOH) will have the highest pH. Weak acids and weak bases will have pH values in the middle range. Neutral salts like KCl will have a pH of 7, which is between acidic and basic pH values.
03

Rank the solutions by pH

Now we can rank these solutions in order of increasing pH: 1. \(\mathrm{HCl}\) - Strong acid (lowest pH) 2. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) - Weak acid (moderate pH) 3. \(\mathrm{KCl}\) - Neutral salt (pH 7) 4. \(\mathrm{NH}_{3}\) - Weak base (moderate to high pH) 5. \(\mathrm{KOH}\) - Strong base (highest pH) Thus, the order of increasing pH is: e. \(\mathrm{HCl}\), c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\), d. \(\mathrm{KCl}\), a. \(\mathrm{NH}_{3}\), and b. \(\mathrm{KOH}\).

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Most popular questions from this chapter

Write the reaction and the corresponding \(K_{\mathrm{b}}\) equilibrium expression for each of the following substances acting as bases in water. a. aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\) b. dimethylamine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}\)

Students are often surprised to learn that organic acids, such as acetic acid, contain - OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as \(\mathrm{H}_{2} \mathrm{SO}_{4}\), has the structural formula \(\mathrm{SO}_{2}(\mathrm{OH})_{2}\), where \(\mathrm{S}\) is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while \(\mathrm{NaOH}\) and \(\mathrm{KOH}\) are bases? a. \(\mathrm{SO}(\mathrm{OH})_{2}\) b. \(\mathrm{ClO}_{2}(\mathrm{OH})\) c. \(\mathrm{HPO}(\mathrm{OH})_{2}\)

Calculate the \(\mathrm{pH}\) of each of the following solutions. a. \(0.10 \mathrm{MCH}_{3} \mathrm{NH}_{3} \mathrm{Cl}\) b. \(0.050 M \mathrm{NaCN}\)

Identify the Lewis acid and the Lewis base in each of the following reactions. a. \(\mathrm{Fe}^{3+}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)\) b. \(\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)\) c. \(\mathrm{HgI}_{2}(s)+2 \mathrm{I}^{-}(a q) \rightleftharpoons \mathrm{HgI}_{4}{ }^{2-}(a q)\)

Calculate the percent dissociation of the acid in each of the following solutions. a. \(0.50 M\) acetic acid b. \(0.050 M\) acetic acid c. \(0.0050 M\) acetic acid d. Use Le Châtelier's principle to explain why percent dissociation increases as the concentration of a weak acid decreases. e. Even though the percent dissociation increases from solutions a to \(\mathrm{c}\), the \(\left[\mathrm{H}^{+}\right]\) decreases. Explain.
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