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Chapter 16: Problem 14

Which of the following statements is false? (a) An Arrhenius base increases the concentration of \(\mathrm{OH}^{-}\) in water. (b) A Br酶nsted-Lowry base is a proton acceptor. (c) Water can act as a Br酶nsted-Lowry acid. (d) Water can act as a Br酶nsted-Lowry base. (e) Any compound that contains an -OH group acts as a Br酶nsted-Lowry base.

Short Answer

Expert verified
The false statement is (e): Any compound that contains an -OH group acts as a Br酶nsted-Lowry base.

Step by step solution

01

Statement (a)

An Arrhenius base is a substance that produces hydroxide ions (\(\mathrm{OH}^{-}\)) when dissolved in water. Therefore, according to Arrhenius definition, this statement is true.
02

Statement (b)

A Br酶nsted-Lowry base is defined as a proton acceptor, meaning that it can accept a hydrogen ion (\(\mathrm{H}^{+}\)) from another substance. This is the main concept of the Br酶nsted-Lowry definition, making this statement also true.
03

Statement (c)

Water (\(\mathrm{H}_{2}\mathrm{O}\)) can indeed act as a Br酶nsted-Lowry acid, as it can donate a hydrogen ion (\(\mathrm{H}^{+}\)) to another substance. For example, when water reacts with ammonia, it donates a hydrogen ion to form the ammonium ion and hydroxide ion. Thus, this statement is true.
04

Statement (d)

Water can also act as a Br酶nsted-Lowry base because it can accept a hydrogen ion from another substance. When water reacts with an acid, it accepts a hydrogen ion to form the hydronium ion (\(\mathrm{H}_{3}\mathrm{O}^{+}\)). This behavior confirms that this statement is true.
05

Statement (e)

While many compounds containing an -OH group (hydroxyl group) can act as Br酶nsted-Lowry bases, it is not universally true for all compounds. Some compounds, like alcohols, do not readily donate or accept protons in water, and thus do not behave as bases. Therefore, this statement is false. The result is, the false statement is (e): Any compound that contains an -OH group acts as a Br酶nsted-Lowry base.

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Key Concepts

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

Arrhenius Base
The term "Arrhenius Base" comes from a model developed by Svante Arrhenius to describe how substances behave in aqueous solutions. According to this model, an Arrhenius base is a substance that increases the concentration of hydroxide ions (\( \mathrm{OH}^{-} \)) when it dissolves in water. Such bases typically have a chemical structure that allows them to release hydroxide ions directly when mixed with water.
  • Common examples include sodium hydroxide (NaOH), potassium hydroxide (KOH), and calcium hydroxide (Ca(OH)\(_2\)).
  • These substances dissolve in water and dissociate to release hydroxide ions, making the solution more basic or alkaline.
Understanding the Arrhenius definition is crucial because it directly relates to the chemical behavior in a water-based environment, explaining why bases neutralize acids by providing hydroxide ions, which combine with hydrogen ions to form water.
Br酶nsted-Lowry Base
The Br酶nsted-Lowry concept expands the definition of what can be considered a base. According to this theory, a Br酶nsted-Lowry base is any substance that can accept a proton (\( \mathrm{H}^{+} \)). This definition is broader than the Arrhenius model, as it does not restrict bases to only those that produce hydroxide ions.
  • The classic example is ammonia (\( \mathrm{NH}_3 \)), which can accept a proton to form \( \mathrm{NH}_4^+ \).
  • This concept is useful in more complex chemical environments, such as organic chemistry, where reactions do not always occur in water.
  • A molecule or ion acting as a Br酶nsted-Lowry base doesn't need to release \( \mathrm{OH}^{-} \) ions; it only needs to accept a proton from a donor.
The versatility of this definition allows for a more comprehensive understanding of basicity, particularly in non-aqueous systems.
Br酶nsted-Lowry Acid
The Br酶nsted-Lowry Acid concept complements that of the base. Under this framework, an acid is any substance that can donate a proton (\( \mathrm{H}^{+} \)) to another substance. This is pivotal because it broadens the context in which acids can be recognized beyond aqueous solutions, as emphasized in Arrhenius's concept.
  • For instance, hydrochloric acid (\( \mathrm{HCl} \)) donates a proton to water, forming hydronium ions (\( \mathrm{H}_3\mathrm{O}^{+} \)).
  • The reaction of acetic acid with water is another example, where it donates a proton to form acetate ions.
  • Water itself is an interesting case, as it can act both as an acid and a base (amphoteric behavior).
This dual ability to donate and accept protons makes the Br酶nsted-Lowry definitions very adaptable and relevant across diverse chemical environments, portraying acids and bases as parts of pairs known as conjugate acid-base pairs.
Hydroxide Ion
The hydroxide ion (\( \mathrm{OH}^{-} \)) is a key component in understanding basicity, especially in the context of Arrhenius bases. It is negatively charged, consisting of one oxygen atom covalently bonded to one hydrogen atom, and it plays a vital role in acid-base chemistry.
  • In aqueous solutions, hydroxide ions increase the pH level, making the environment less acidic and more basic.
  • Hydroxide ions readily combine with hydrogen ions (\( \mathrm{H}^{+} \)) to form water (\( \mathrm{H}_2\mathrm{O} \)), a process that is central to neutralization reactions.
  • The presence of \( \mathrm{OH}^{-} \) ions is a hallmark of many strong bases, which can completely dissociate in water.
Recognizing the role and behavior of hydroxide ions helps in identifying and understanding the nature of bases and their interactions with acids, facilitating the prediction of chemical behaviors in different reactions.

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Most popular questions from this chapter

Using data from Appendix \(D\), calculate \(p O H\) and \(p H\) for each (a) \(0.080 M\) potassium hypobromite of the following solutions: \((\mathrm{KBrO}),\) (b) \(0.150 \mathrm{M}\) potassium hydrosulfide \((\mathrm{KHS}),(\mathbf{c})\) a mixture that is \(0.25 \mathrm{M}\) in potassium nitrite \(\left(\mathrm{KNO}_{2}\right)\) and \(0.15 \mathrm{M}\) in magnesium nitrite \(\left(\mathrm{Mg}\left(\mathrm{NO}_{2}\right)_{2}\right)\).

Which, if any, of the following statements are true? (a) The stronger the base, the smaller the \(\mathrm{p} K_{b}\). (b) The stronger the base, the larger the \(\mathrm{p} K_{b}\). (c) The stronger the base, the smaller the \(K_{b}\). (d) The stronger the base, the larger the \(K_{b}\). (e) The stronger the base, the smaller the \(\mathrm{p} K_{a}\) of its conjugate acid. (f) The stronger the base, the larger the \(\mathrm{p} K_{a}\) of its conjugate acid.

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 \(8.2 \times 10^{-3} \mathrm{M} \mathrm{NaOH}\).

Which member of each pair produces the more acidic aqueous solution: \((\mathbf{a}) \mathrm{Zn} \mathrm{Br}_{2}\) or \(\mathrm{CdCl}_{2},\) (b) \(\mathrm{CuCl}\) or \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\), (c) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) or \(\mathrm{NiBr}_{2} ?\)

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) \(\mathrm{HCOOK},(\mathrm{v}) \mathrm{KF} .\)
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