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Chapter 15: Problem 43

Determine whether each of the following is a strong acid, weak acid, strong base, or weak base. Then write an equation describing the process that occurs when the substance is dissolved in water. (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{HCl}\) (c) \(\mathrm{KOH}\) (d) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

Short Answer

Expert verified
(a) Weak base: \(\text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons \text{NH}_4^+ + \text{OH}^-\)(b) Strong acid: \(\text{HCl} \rightarrow \text{H}^+ + \text{Cl}^-\)(c) Strong base: \(\text{KOH} \rightarrow \text{K}^+ + \text{OH}^-\)(d) Weak acid: \(\text{HC}_2\text{H}_3\text{O}_2 \rightleftharpoons \text{H}^+ + \text{C}_2\text{H}_3\text{O}_2^-\)

Step by step solution

01

Classify \(\text{NH}_3\)

Determine if \(\text{NH}_3\) is a strong acid, weak acid, strong base, or weak base. Ammonia (\(\text{NH}_3\)) is a weak base. When dissolved in water, it partially ionizes to form ammonium ion (\(\text{NH}_4^+\)) and hydroxide ion (\(\text{OH}^-\)).Write the equation:\( \text{NH}_3 + \text{H}_2\text{O} \rightleftharpoons \text{NH}_4^+ + \text{OH}^- \)
02

Classify \(\text{HCl}\)

Determine if \(\text{HCl}\) is a strong acid, weak acid, strong base, or weak base. Hydrochloric acid (\(\text{HCl}\)) is a strong acid. When dissolved in water, it completely ionizes to form hydrogen ion (\(\text{H}^+\)) and chloride ion (\(\text{Cl}^-\)).Write the equation:\( \text{HCl} \rightarrow \text{H}^+ + \text{Cl}^- \)
03

Classify \(\text{KOH}\)

Determine if \(\text{KOH}\) is a strong acid, weak acid, strong base, or weak base. Potassium hydroxide (\(\text{KOH}\)) is a strong base. When dissolved in water, it completely ionizes to form potassium ion (\(\text{K}^+\)) and hydroxide ion (\(\text{OH}^-\)).Write the equation:\( \text{KOH} \rightarrow \text{K}^+ + \text{OH}^- \)
04

Classify \(\text{HC}_2\text{H}_3\text{O}_2\)

Determine if \(\text{HC}_2\text{H}_3\text{O}_2\) is a strong acid, weak acid, strong base, or weak base. Acetic acid (\(\text{HC}_2\text{H}_3\text{O}_2\)) is a weak acid. When dissolved in water, it partially ionizes to form hydrogen ion (\(\text{H}^+\)) and acetate ion (\(\text{C}_2\text{H}_3\text{O}_2^-\)).Write the equation:\( \text{HC}_2\text{H}_3\text{O}_2 \rightleftharpoons \text{H}^+ + \text{C}_2\text{H}_3\text{O}_2^- \)

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Key Concepts

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

strong acid
A strong acid is one that completely ionizes in water. This means every molecule of the acid releases its hydrogen ions \((H^+)\) when dissolved. For instance, hydrochloric acid \(HCl\) is a strong acid. When it dissolves in water, it fully dissociates into hydrogen ions \((H^+)\) and chloride ions \((Cl^-)\). The equation for this process is: \(\text{HCl} \rightarrow \text{H}^+ + \text{Cl}^-\). The complete ionization of strong acids leads to higher concentrations of hydrogen ions in the solution, thus resulting in a lower pH value.
weak acid
Unlike strong acids, weak acids only partially ionize in water. This means that only a small fraction of the acid molecules release their hydrogen ions. Acetic acid \((HC_2H_3O_2)\) is a classic example of a weak acid. The dissociation of acetic acid in water can be described by the following equilibrium equation: \(HC_2H_3O_2 \rightleftharpoons H^+ + C_2H_3O_2^-\). Because weak acids do not fully ionize, they produce fewer hydrogen ions in the solution, leading to a higher pH compared to strong acids.
strong base
Strong bases, similar to strong acids, completely ionize in water. This means that they fully dissociate into their respective ions. Potassium hydroxide \((KOH)\) is an example of a strong base. When dissolved in water, KOH completely breaks down into potassium ions \((K^+)\) and hydroxide ions \((OH^-)\). The corresponding equation is: \(KOH \rightarrow K^+ + OH^-\). The complete ionization results in a higher concentration of hydroxide ions in the solution, which makes the solution highly basic and increases its pH.
weak base
A weak base, on the other hand, only partially ionizes in water. Ammonia \((NH_3)\) is a typical weak base. When dissolved in water, it reacts partially, forming ammonium ions \((NH_4^+)\) and hydroxide ions \((OH^-)\). This can be expressed by the equilibrium equation: \(NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^-\). Because weak bases do not fully ionize, they produce fewer hydroxide ions in the solution, resulting in a solution that is less basic compared to those of strong bases.
ionization in water
Ionization in water refers to the process where an acid or base breaks down into its respective ions. For acids, ionization involves releasing hydrogen ions \((H^+)\). In the case of bases, it involves releasing hydroxide ions \((OH^-)\). In strong substances, whether acids or bases, ionization is complete, leading to a high concentration of ions in the solution. On the other hand, weak substances ionize only partially, resulting in a lower concentration of ions. The degree of ionization significantly impacts the pH of the solution, with strong acids and bases causing more drastic changes in pH compared to their weak counterparts.

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Most popular questions from this chapter

Balance each of the following equations; then change them into balanced net ionic equations: (a) \(\mathrm{Mg}(s)+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow \mathrm{Cu}(s)+\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (c) \(\mathrm{K}_{2} \mathrm{SO}_{3}(a q)+\mathrm{HClO}_{4}(a q) \longrightarrow\) \(\mathrm{KClO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{2}(g)\)

Write an equation showing how sodium sulfate dissociates in water.

A \(10.0-\mathrm{mL}\) sample of \(\mathrm{HNO}_{3}\) was diluted to a volume of \(100.00 \mathrm{~mL}\). Then \(25 \mathrm{~mL}\) of that diluted solution were needed to neutralize \(50.0 \mathrm{~mL}\) of \(0.60 \mathrm{M} \mathrm{KOH}\). What was the concentration of the original nitric acid?

Calculate the \(\mathrm{pH}\) of (a) orange juice, \(3.7 \times 10^{-4} \mathrm{M} \mathrm{H}^{+}\) (b) vinegar, \(2.8 \times 10^{-3} \mathrm{M} \mathrm{H}^{+}\) (c) shampoo, \(2.4 \times 10^{-6} \mathrm{M} \mathrm{H}^{+}\) (d) dishwashing detergent, \(3.6 \times 10^{-8} \mathrm{M} \mathrm{H}^{+}\)

Determine whether each of the following is a strong acid, weak acid, strong base, or weak base. Then write an equation describing the process that occurs when the substance is dissolved in water. (a) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) (b) \(\mathrm{Ba}(\mathrm{OH})_{2}\) (c) \(\mathrm{HClO}_{4}\) (d) \(\mathrm{HBr}\)
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