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Chapter 16: Problem 104

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

Short Answer

Expert verified
In summary, the more acidic compounds among each pair are: (a) CdCl鈧, because Cd虏鈦 is more metallic than Zn虏鈦, making it more acidic. (b) CuCl, because Cl鈦 has a stronger polarizing effect on Cu鈦 than NO鈧冣伝, making it more acidic. (c) NiBr鈧, because the greater polarizing effect of Br鈦 on Ni虏鈦 and the weaker nature of NO鈧冣伝 outweighs the effect of Ca虏鈦 in Ca(NO鈧)鈧, making NiBr鈧 more acidic.

Step by step solution

01

Identify acidic strength trends in the periodic table

Elements that are more metallic in nature (located further to the left and bottom of the periodic table) are more likely to form acidic solutions. The acidity of a solution depends on the ability of the positive ion (cation) to polarize the anions in solution. Stronger anions (halides) will have a greater polarizing effect on the metal cation, leading to the release of more H+ ions (protons) in the solution. (a) ZnBr鈧 and CdCl鈧
02

Compare cations in each compound

For the first pair, we have ZnBr鈧 and CdCl鈧. Both compounds have the same anion group (halides) - bromide (Br-) and chloride (Cl-). When comparing Zn虏鈦 and Cd虏鈦 cations, Cadmium (Cd) is more metallic in nature as it is located below Zinc (Zn) in the periodic table. Therefore, it has stronger acidic characteristics.
03

Identify the more acidic compound

As Cd虏鈦 has stronger acidic characteristics, CdCl鈧 will produce a more acidic aqueous solution compared to ZnBr鈧. (b) CuCl and Cu(NO鈧)鈧
04

Compare anions in each compound

For the second pair, we have CuCl and Cu(NO鈧)鈧. Both compounds have the same cation, Cu鈦. Therefore, we need to compare their anions, which are Cl鈦 and NO鈧冣伝. Cl鈦 ions have a greater polarizing effect on the Cu鈦 cation, as they are stronger anions than NO鈧冣伝.
05

Identify the more acidic compound

As Cl鈦 has a stronger polarizing effect on Cu鈦, the compound CuCl will produce a more acidic aqueous solution compared to Cu(NO鈧)鈧. (c) Ca(NO鈧)鈧 and NiBr鈧
06

Compare cations in each compound

For the third pair, we have Ca(NO鈧)鈧 and NiBr鈧. Both compounds have the same anion group: nitrate (NO鈧冣伝) for Ca(NO鈧)鈧, and bromide (Br鈦) for NiBr鈧. Now we compare the corresponding cations, which are Ca虏鈦 and Ni虏鈦. Calcium (Ca) is more metallic in nature as it is located further to the left and bottom of the periodic table.
07

Compare anions in each compound

In this case, we also need to compare the anions, NO鈧冣伝 for Ca(NO鈧)鈧, and Br鈦 for NiBr鈧. Br鈦 is a stronger anion as compared to NO鈧冣伝.
08

Identify the more acidic compound

Even though Ca虏鈦 is more metallic, the greater polarizing effect of Br鈦 on the Ni虏鈦 cation and the weaker nature of NO鈧冣伝 outweighs the effect of Ca虏鈦, making NiBr2 more acidic. Therefore, NiBr鈧 will produce a more acidic aqueous solution compared to Ca(NO鈧)鈧. In summary, the more acidic compounds among each pair are: (a) CdCl鈧 (b) CuCl (c) NiBr鈧

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Key Concepts

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

Cation Polarization
Cation polarization is an essential consideration when analyzing the acidity of aqueous solutions. It occurs when a metal cation, such as \( ext{Cd}^{2+}\) or \( ext{Cu}^{+}\), affects the electrons of the anion it is associated with, such as \( ext{Cl}^{-}\) or \( ext{Br}^{-}\). This influence can polarize the anion, distorting the electron cloud, and facilitating the release of \( ext{H}^{+}\) ions into the solution. More polarized anions lead to higher acidity.
  • Smaller cations like \( ext{Cu}^{+}\) can polarize surrounding anions more efficiently due to their high charge density.
  • Cations with higher polarization power can lead to weaker bonds in the anions, making it easier to release protons into the solution.
Understanding cation polarization helps predict the strength of acid formed in solutions, influencing which compound will ultimately be more acidic.
Metallic Elements
The position of metallic elements on the periodic table is crucial for determining their potential to form acidic solutions. Metals that are located more to the left and towards the bottom of the table are considered more metallic in nature.
Elements like Calcium (Ca) and Cadmium (Cd) exhibit such metallic properties.
  • Metallic elements tend to donate electrons more freely, forming positively charged cations that can influence anions to release \( ext{H}^{+}\) ions.
  • These properties are because metals lower down the groups like \( ext{Cd}^{2+}\) are more metal-like than those such as \( ext{Zn}^{2+}\), influencing the acidity of the solution they form.
Hence, the metallic nature isn't just about conductivity or luster; it directly impacts the chemical behavior, especially in aqueous environments.
Halide Anions
Halide anions are a class of anions derived from halogens, such as \( ext{Cl}^{-}\) and \( ext{Br}^{-}\). These anions are particularly significant in determining the acidity of a solution when paired with metal cations.
  • Halides exert a strong polarizing effect on metal cations due to their size and the nature of their charge.
  • Larger halides such as \( ext{Br}^{-}\) are more easily polarized compared to smaller ones like \( ext{Cl}^{-}\).
For instance, \( ext{NiBr}_2\) is more acidic than \( ext{Ca(NO}_3 ext{)}_2\) largely because the \( ext{Br}^{-}\) ions can polarize \( ext{Ni}^{2+}\) more effectively, leading to a higher release of protons into the solution.
Periodic Table Trends
Periodic table trends offer a roadmap for predicting chemical behaviors, including the acidity of metal salts in aqueous solutions. As you move across periods and down groups in the periodic table, several trends emerge that influence acidity.
  • Elements to the left are more metallic, often forming cations which lead to more acidic solutions.
  • Moving down a group increases an element's metallic character, impacting how they interact with anions.
  • For example, Cd is below Zn in the table and more metallic, leading to CdCl鈧 being more acidic than ZnBr鈧.
These trends help us understand the interaction between cations and anions, enabling us to predict and explain the resulting acidity of solutions more accurately.

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Most popular questions from this chapter

Caproic acid \(\left(\mathrm{C}_{5} \mathrm{H}_{11} \mathrm{COOH}\right)\) is found in small amounts in coconut and palm oils and is used in making artificial flavors. A saturated solution of the acid contains \(11 \mathrm{~g} / \mathrm{L}\) and has a pH of 2.94. Calculate \(K_{a}\) for the acid.

Calculate [OH \(^{-}\) ] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) \(\left[\mathrm{H}^{+}\right]=0.0045 \mathrm{M}\) (b) \(\left[\mathrm{H}^{+}\right]=1.5 \times 10^{-9} \mathrm{M} ;\) (c) a solution in which \(\left[\mathrm{H}^{+}\right]\) is 10 times greater than \(\left[\mathrm{OH}^{-}\right]\).

Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs: (a) \(\mathrm{NO}_{3}^{-}\) or \(\mathrm{NO}_{2}^{-}\), (c) \(\mathrm{HCO}_{3}^{-}\) or \(\mathrm{CO}_{3}^{2-}\). (b) \(\mathrm{PO}_{4}{ }^{3-}\) or \(\mathrm{AsO}_{4}{ }^{3-}\)

(a) How does the strength of an acid vary with the polarity and strength of the \(\mathrm{H}-\mathrm{X}\) bond? (b) How does the acidity of the binary acid of an element vary as a function of the electronegativity of the element? How does this relate to the position of the element in the periodic table?

(a) What is the difference between the Arrhenius and the Bronsted-Lowry definitions of a base? (b) When ammonia is dissolved in water, it behaves both as an Arrhenius base and as a Bronsted-Lowry base. Explain.
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