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Chapter 17: Problem 103

Arrange the following \(0.10 \mathrm{M}\) solutions in order of increasing pH. (a) \(\mathrm{NaCl}\) (b) \(\mathrm{NH}_{4} \mathrm{Cl}\) (c) \(\mathrm{HCl}\) $$\begin{aligned} &\text { (d) } \mathrm{NaCH}_{3} \mathrm{CO}_{2}\\\ &\text { (e) } \mathrm{KOH} \end{aligned}$$

Short Answer

Expert verified
Order of increasing pH: HCl, NH4Cl, NaCl, NaCH3CO2, KOH.

Step by step solution

01

Identify the nature of each solute

\(\mathrm{NaCl}\) is a neutral salt, \(\mathrm{NH}_4\mathrm{Cl}\) is an acidic salt due to the \(\mathrm{NH}_4^+\) ion, \(\mathrm{HCl}\) is a strong acid, \(\mathrm{NaCH}_3\mathrm{CO}_2\) is a basic salt because of the acetate ion \(\mathrm{CH}_3\mathrm{COO}^-\), and \(\mathrm{KOH}\) is a strong base.
02

Determine the effect on pH for each solution

Neutral salts like \(\mathrm{NaCl}\) do not affect pH, acidic salts like \(\mathrm{NH}_4\mathrm{Cl}\) decrease pH, strong acids like \(\mathrm{HCl}\) even more decrease pH, basic salts like \(\mathrm{NaCH}_3\mathrm{CO}_2\) increase pH, and strong bases like \(\mathrm{KOH}\) significantly increase pH.
03

Rank the solutions based on pH effect

The order based on pH from lowest to highest is: \(\mathrm{HCl} < \mathrm{NH}_4\mathrm{Cl} < \mathrm{NaCl} < \mathrm{NaCH}_3\mathrm{CO}_2 < \mathrm{KOH}\). \(\mathrm{HCl}\) is most acidic, \(\mathrm{NH}_4\mathrm{Cl}\) is less acidic, \(\mathrm{NaCl}\) is neutral, \(\mathrm{NaCH}_3\mathrm{CO}_2\) is slightly basic, and \(\mathrm{KOH}\) is strongly basic.

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Key Concepts

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

Acidic Solutions
When we talk about acidic solutions, we refer to solutions with a pH less than 7. These solutions have a higher concentration of hydrogen ions (H extsuperscript{+}) compared to hydroxide ions (OH extsuperscript{-}). This high concentration of H extsuperscript{+} ions is what gives these solutions their acidic properties.
In the exercise above, hydrochloric acid ( HCl ) and ammonium chloride ( NH_4Cl ) are examples of substances that can create acidic solutions.
  • Hydrochloric Acid (HCl): This is a strong acid that completely dissociates in water, releasing one hydrogen ion for every molecule of HCl. Hence, it significantly lowers the pH of a solution.
  • Ammonium Chloride (NH_4Cl): This is an acidic salt due to the presence of the ammonium ion ( NH_4^+ ), which can release a hydrogen ion by reacting with water, thereby slightly lowering the pH.
Understanding how these substances affect pH is crucial in predicting whether solutions will be acidic.
Basic Solutions
Basic solutions have a pH greater than 7 and contain more hydroxide ions (OH extsuperscript{-}) than hydrogen ions (H extsuperscript{+}). These solutions can neutralize acids and feel slippery to the touch.
In the given exercise, potassium hydroxide ( KOH ) and sodium acetate ( NaCH_3CO_2 ) are examples of substances leading to basic solutions.
  • Potassium Hydroxide (KOH): This is a strong base, dissociating completely in water to yield hydroxide ions, thus significantly increasing the pH.
  • Sodium Acetate (NaCH_3CO_2): This is a basic salt. The acetate ion can react with water to produce OH extsuperscript{-} ions, slightly increasing the pH of the solution.
Recognizing these components helps us foresee their impact on the basic nature of a solution.
Neutral Solutions
Neutral solutions have a pH of around 7, meaning the concentration of hydrogen ions (H extsuperscript{+}) is equal to that of hydroxide ions (OH extsuperscript{-}). Typically, pure water is the standard example of a neutral solution.
In the exercise, sodium chloride (NaCl) represents a neutral salt. When dissolved in water, NaCl dissociates into sodium ( Na^+ ) and chloride ( Cl^- ) ions, neither of which affects the pH of the solution.
  • Sodium Chloride (NaCl): Being a neutral salt, it does not alter the concentration of H extsuperscript{+} or OH extsuperscript{-} ions in the solution, maintaining neutrality.
Identifying neutral solutions is essential for maintaining a balanced pH in various chemical processes.
Chemical Salts
Chemical salts are compounds resulting from the neutralization reaction between an acid and a base. These salts can be neutral, acidic, or basic in nature, depending on the strengths of the acid and base from which they are formed.
For example, in the original exercise:
  • Sodium Chloride (NaCl): Formed from a strong acid (HCl) and a strong base (NaOH), NaCl is a neutral salt as both components are equally strong.
  • Ammonium Chloride (NH_4Cl): Resulting from a weak base (NH_3) and a strong acid (HCl), NH_4Cl is an acidic salt.
  • Sodium Acetate (NaCH_3CO_2): Created from a strong base (NaOH) and a weak acid (acetic acid), making it a basic salt.
Understanding these salts helps in predicting their effect on a solution鈥檚 pH.
Strong Acids and Bases
Strong acids and bases are substances that completely dissociate into their ions in water. They have a major impact on the pH of solutions, driving the pH far from neutrality.
  • Strong Acids (e.g., HCl): Fully ionize to give high concentrations of H extsuperscript{+} ions, dramatically lowering the pH.
  • Strong Bases (e.g., KOH): Fully ionize to release high concentrations of OH extsuperscript{-} ions, substantially raising the pH.
Recognizing strong acids and bases is crucial for effectively managing chemical reactions and solution pH.

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Most popular questions from this chapter

Given the following solutions: (a) \(0.1 \mathrm{M} \mathrm{NH}_{3}\) (e) \(0.1 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) (b) \(0.1 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}\) (f) \(0.1 \mathrm{M} \mathrm{NaCH}_{3} \mathrm{CO}_{2}\) (c) \(0.1 \mathrm{M} \mathrm{NaCl}\) (g) \(0.1 \mathrm{M} \mathrm{NH}_{4} \mathrm{CH}_{3} \mathrm{CO}_{2}\) (d) \(0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\) (i) Which of the solutions are acidic? (ii) Which of the solutions are basic? (iii) Which of the solutions is most acidic?

About this time, you may be wishing you had an aspirin. Aspirin is an organic acid (page 507 ) with a \(K_{\mathrm{a}}\) of \(3.27 \times\) \(10^{-4}\) for the reaction \(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftarrows \mathrm{C}_{9} \mathrm{H}_{7} \mathrm{O}_{4}^{-}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})\) If you have two tablets, each containing \(0.325 \mathrm{g}\) of aspirin (mixed with a neutral "binder" to hold the tablet together), and you dissolve them in a glass of water to give 225 mL of solution, what is the pH of the solution?

Dissolving \(\mathrm{K}_{2} \mathrm{CO}_{3}\) in water gives a basic solution. Write a balanced equation showing how the carbonate ion is responsible for this effect.

A 0.10 M solution of chloroacetic acid, \(\mathrm{ClCH}_{2} \mathrm{CO}_{2} \mathrm{H}\), has a pH of \(1.95 .\) Calculate \(K_{\mathrm{a}}\) for the acid.

What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base, and the base and its conjugate acid. (a) \(\mathrm{HClO}_{4}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (b) \(\mathrm{NH}_{4}^{+}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (c) \(\mathrm{HCO}_{3}^{-}+\mathrm{OH}^{-} \longrightarrow\)
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