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Chapter 16: Problem 110

Arrange the following \(0.10 \mathrm{M}\) solutions in order of increasing acidity: (i) \(\mathrm{HCOONH}_{4}\), (ii) \(\mathrm{NH}_{4} \mathrm{Br}\), (iii) \(\mathrm{NaNO}_{3}\), (iv) \(\mathrm{HCOOK},(\mathrm{v}) \mathrm{KF} .\)

Short Answer

Expert verified
The order of increasing acidity for the given solutions is (iii) \(\mathrm{NaNO}_{3}\) < (iv) \(\mathrm{HCOOK}\) < (v) \(\mathrm{KF}\) < (ii) \(\mathrm{NH}_{4} \mathrm{Br}\) < (i) \(\mathrm{HCOONH}_{4}\).

Step by step solution

01

Identify acidic or basic properties of cations and anions for each solution

We will analyze each of the given solutions to identify the acidic or basic properties of their cations and anions. (i) \(\mathrm{HCOONH}_{4}\) - The cation is \(\mathrm{NH}_{4}^{+}\) (ammonium ion) which is acidic as it donates proton and the anion is \(\mathrm{HCOO}^{-}\) (formate ion) which is basic as it can accept a proton. (ii) \(\mathrm{NH}_{4} \mathrm{Br}\) - The cation is \(\mathrm{NH}_{4}^{+}\) (ammonium ion) which is acidic and the anion is \(\mathrm{Br}^{-}\) (bromide ion), which is neutral. (iii) \(\mathrm{NaNO}_{3}\) - The cation is \(\mathrm{Na}^{+}\) (sodium ion) which is neutral and the anion is \(\mathrm{NO}_{3}^{-}\) (nitrate ion) which is also neutral. (iv) \(\mathrm{HCOOK}\) - The cation is \(\mathrm{K}^{+}\) (potassium ion) which is neutral and the anion is \(\mathrm{HCOO}^{-}\) (formate ion) which is basic. (v) \(\mathrm{KF}\) - The cation is \(\mathrm{K}^{+}\) (potassium ion) which is neutral and the anion is \(\mathrm{F}^{-}\) (fluoride ion) which is basic.
02

Analyze the acidic and basic properties of given solutions and arrange them in order

Below are the acidic and basic properties of the given solutions: (i) \(\mathrm{HCOONH}_{4}\) - Acidic cation and basic anion. (ii) \(\mathrm{NH}_{4} \mathrm{Br}\) - Acidic cation and neutral anion. (iii) \(\mathrm{NaNO}_{3}\) - Neutral cation and neutral anion. (iv) \(\mathrm{HCOOK}\) - Neutral cation and basic anion. (v) \(\mathrm{KF}\) - Neutral cation and basic anion. Now, keeping in mind that acidity is increased by having more acidic cations and decreased by having more basic anions, we can arrange these in order of increasing acidity: Neutral cation and neutral anion: \(\mathrm{NaNO}_{3}\) (iii) Neutral cation and less basic anion: \(\mathrm{HCOOK}\) (iv) Neutral cation and more basic anion: \(\mathrm{KF}\) (v) Acidic cation and less basic anion: \(\mathrm{NH}_{4} \mathrm{Br}\) (ii) Acidic cation and more basic anion: \(\mathrm{HCOONH}_{4}\) (i) So, the order of increasing acidity is (iii) \(\mathrm{NaNO}_{3}\) < (iv) \(\mathrm{HCOOK}\) < (v) \(\mathrm{KF}\) < (ii) \(\mathrm{NH}_{4} \mathrm{Br}\) < (i) \(\mathrm{HCOONH}_{4}\).

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Key Concepts

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

Buffer Solutions
Understanding buffer solutions is essential when studying the acidity and basicity of solutions. A buffer solution is a special type of solution that resists changes in pH when small amounts of acid or base are added. In essence, it "buffers" the solution against dramatic pH changes.

Buffer solutions are typically made from a weak acid and its conjugate base or a weak base and its conjugate acid.
  • For example, a common buffer system includes acetic acid ( CH鈧僀OOH) and its conjugate base, acetate ( CH鈧僀OO鈦�).
  • Similarly, ammonia ( NH鈧�) and ammonium ( NH鈧勨伜) form another classic buffer pair.
The presence of both an acidic and basic component allows the solution to neutralize added acids or bases.

This property is crucial in biological and chemical applications where maintaining a stable pH is necessary for proper functioning.

Buffer solutions are widely used in chemical laboratories, medical formulations, and various industrial applications.
Acid-Base Equilibria
Acid-base equilibria describe how acids and bases react with each other in water and influence the acidity or basicity of solutions. When discussing acid-base reactions, it's important to consider whether the acid or base fully dissociates in water.

There are two categories:
  • **Strong acids** and **bases**, which dissociate completely in aqueous solutions. Examples include hydrochloric acid ( HCl) and sodium hydroxide ( NaOH).
  • **Weak acids** and **bases**, which only partially dissociate in solutions. Examples are acetic acid ( CH鈧僀OOH) and ammonia ( NH鈧�).
Acid-base equilibria explain how ions like H鈦� and OH鈦� affect pH levels. The equilibrium constant ( K_a for acids and K_b for bases) is used to predict the extent of dissociation and subsequently, the pH of a solution.

Understanding these interactions is critical for predicting the impact of substances in solution, particularly in reactions involving ionic compounds or buffer systems.
Ionic Compounds
Ionic compounds play a significant role in determining the acidity or basicity of a solution. These compounds consist of a cation (positively charged ion) and an anion (negatively charged ion). When dissolved in water, ionic compounds disassociate into their constituent ions. This disassociation can affect the pH of the solution, depending on the properties of the ions.

For example:
  • **Sodium chloride ( NaCl)**, a neutral salt, completely dissociates into the neutral Na鈦� and Cl鈦� ions, having no effect on the solution's acidity.
  • **Ammonium chloride ( NH鈧凜l)**, on the other hand, dissociates into the acidic NH鈧勨伜 and neutral Cl鈦� ions, making the solution slightly acidic.
These characteristics of ionic compounds, such as ability of cations to donate protons or of anions to accept them, determine if the resulting solution will be acidic, basic, or neutral.

Understanding how these ions interact when dissolved is critical for predicting the outcomes in various chemical reactions and in formulating buffer solutions.

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Most popular questions from this chapter

The \(\mathrm{p} K_{\mathrm{b}}\) of water is (a) 1 (b) 7 (c) 14 (d) not defined (e) none of the above

Many moderately large organic molecules containing basic nitrogen atoms are not very soluble in water as neutral molecules, but they are frequently much more soluble as their acid salts. Assuming that \(\mathrm{pH}\) in the stomach is 2.5 , indicate whether each of the following compounds would be present in the stomach as the neutral base or in the protonated form: nicotine, \(K_{b}=7 \times 10^{-7}\); caffeine, \(K_{b}=4 \times 10^{-14} ;\) strychnine, \(K_{b}=1 \times 10^{-6} ;\) quinine, \(K_{b}=1.1 \times 10^{-6} .\)

Calculate \(\left[\mathrm{OH}^{-}\right]\) and \(\mathrm{pH}\) for each of the following strong base solutions: (a) \(0.182 \mathrm{M} \mathrm{KOH},\) (b) \(3.165 \mathrm{~g}\) of \(\mathrm{KOH}\) in 500.0 \(\mathrm{mL}\) of solution, \((\mathbf{c}) 10.0 \mathrm{~mL}\) of \(0.0105 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\) diluted to \(500.0 \mathrm{~mL},(\mathbf{d})\) a solution formed by mixing \(20.0 \mathrm{~mL}\) of 0.015 \(M \mathrm{Ba}(\mathrm{OH})_{2}\) with \(40.0 \mathrm{~mL}\) of \(8.2 \times 10^{-3} \mathrm{M} \mathrm{NaOH}\).

At \(50^{\circ} \mathrm{C}\), the ion-product constant for \(\mathrm{H}_{2} \mathrm{O}\) has the value \(K_{w}=5.48 \times 10^{-14} \cdot(\mathbf{a})\) What is the \(\mathrm{pH}\) of pure water at \(50^{\circ} \mathrm{C} ?\) (b) Based on the change in \(K_{w}\) with temperature, predict whether \(\Delta H\) is positive, negative, or zero for the autoionization reaction of water: $$ 2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{OH}^{-}(a q) $$

Write the chemical equation and the \(K_{b}\) expression for the reaction of each of the following bases with water: (a) propylamine, \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{NH}_{2} ;\) (b) monohydrogen phosphate ion, \(\mathrm{HPO}_{4}^{2-} ;(\mathbf{c})\) benzoate ion, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2}^{-}\)
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