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Chapter 5: Problem 80

Name two anions that combine with \(\mathrm{Al}^{3+}\) ion to produce water- soluble compounds.

Short Answer

Expert verified
Common anions like nitrate (\(\mathrm{NO}_3^-\)) and perchlorate (\(\mathrm{ClO}_4^-\)) form water-soluble compounds with \(\mathrm{Al}^{3+}\).

Step by step solution

01

Understand Aluminum Ion

The given ion is the aluminum ion, denoted as \( \mathrm{Al}^{3+} \). This is a cation with a 3+ charge, indicating it can combine with anions to form compounds.
02

Identify Soluble Compounds

To find anions that form water-soluble compounds with \( \mathrm{Al}^{3+} \), recall common solubility rules. Anions that often form soluble compounds include perchlorate (\( \mathrm{ClO}_4^- \)) and nitrate (\( \mathrm{NO}_3^- \)). Both tend to form water-soluble compounds regardless of the accompanying cation.
03

Combine Anions with Aluminum Ion

Combine each identified anion with the \( \mathrm{Al}^{3+} \) ion. With perchlorate, the compound formed is \( \mathrm{Al(ClO}_4)_3 \). With nitrate, the compound formed is \( \mathrm{Al(NO}_3)_3 \). Both are known to be highly soluble in water.

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Key Concepts

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

Aluminum Ion
The aluminum ion, represented as \( \mathrm{Al}^{3+} \), is a very common cation in chemistry. Cations are positively charged ions, and the number \( 3+ \) indicates that the aluminum ion has lost three electrons. This gives it a positive charge of three. Because it is a cation, aluminum is eager to interact with anions, which are negatively charged ions. This interaction helps to stabilize the compound created.
  • The charge of \( \mathrm{Al}^{3+} \) plays a critical role in how it bonds with other ions.
  • Being a metal, aluminum usually donates electrons, making it a stable ion.
  • Its positive charge means it can form bonds with anions which have a total charge of \(-3\). This creates neutral compounds where the charges balance out.
Understanding aluminum ions is crucial when studying the formation of ionic compounds and predicting their properties, such as solubility.
Anions
Anions are ions that carry a negative charge. This charge results from an atom gaining extra electrons. In the context of combining with aluminum ions, anions play a key role in forming ionic compounds. Two anions that are often examined in relation to solubility with aluminum ions are perchlorate (\( \mathrm{ClO}_4^- \)) and nitrate (\( \mathrm{NO}_3^- \)).
  • Perchlorate, \( \mathrm{ClO}_4^- \), is a type of oxyanion. It's known for forming stable, soluble ionic compounds with many cations including \( \mathrm{Al}^{3+} \).
  • Nitrate, \( \mathrm{NO}_3^- \), is another common anion that combines well with a variety of cations and is almost always soluble in water.
In chemical reactions, the role of anions is to balance the positive charge from cations like aluminum, forming stable and often water-soluble compounds.
Solubility Rules
Solubility rules are guidelines that indicate whether a compound will dissolve in water, creating a solution. These rules are essential for predicting the behavior of ionic compounds in aquatic environments. The solubility of a compound depends on the combination of ions it contains, particularly on the specific anions in question.
  • Compounds containing nitrate (\( \mathrm{NO}_3^- \)) and perchlorate (\( \mathrm{ClO}_4^- \)) anions are generally soluble in water. This makes them reliable choices for forming soluble compounds with various cations, such as \( \mathrm{Al}^{3+} \).
  • The rule of thumb is that if a compound contains an alkali metal cation or ammonium, it typically dissolves in water. However, certain anions like nitrate and perchlorate ensure solubility irrespective of the cation.
Knowing these solubility rules allows chemists to predict which ionic compounds will dissolve in water, thus understanding their potential applications in various chemical reactions and real-world applications.

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Most popular questions from this chapter

Identify the spectator ion or ions in the reaction of nitric acid and magnesium hydroxide, and write the net ionic equation. What type of exchange reaction is this? $$\begin{aligned} 2 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{NO}_{3}^{-}(\mathrm{aq})+\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s}) \longrightarrow & \\ 2 \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{Mg}^{2+}(\mathrm{aq})+2 \mathrm{NO}_{3}^{-}(\mathrm{aq})\end{aligned}$$

Which of the following methods would you use to prepare \(1.00 \mathrm{L}\) of \(0.125 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4} ?\) (a) Dilute \(20.8 \mathrm{mL}\) of \(6.00 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) to a volume of \(1.00 \mathrm{L}\) (b) Add \(950 .\) mL of water to 50.0 mL. of \(3.00 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\).

Which has the larger concentration of hydrogen ions, \(0.015 \mathrm{M} \mathrm{HCl}\) or a hydrochloric acid solution with a \(\mathrm{pH}\) of \(1.2 ?\)

Describe how to prepare zinc chloride by (a) an acid-base reaction, (b) a gas- forming reaction, and (c) an oxidation-reduction reaction. The available starting materials are \(\mathrm{ZnCO}_{3}, \mathrm{HCl}, \mathrm{Cl}_{2}, \mathrm{HNO}_{3}, \mathrm{Zn}(\mathrm{OH})_{2}\) \(\mathrm{NaCl}, \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2},\) and Zn. Write complete, balanced equations for the reactions chosen.

A Two students titrate different samples of the same solution of HCl using \(0.100 \mathrm{M} \mathrm{NaOH}\) solution and phenolphthalein indicator (see Figure 5.23). The first student pipets \(20.0 \mathrm{mL}\) of the HCl solution into a flask, adds 20 mL of distilled water and a few drops of phenolphthalein solution, and titrates until a lasting pink color appears. The second student pipets \(20.0 \mathrm{mL}\), of the HCl solution into a flask, adds 60 mL. of distilled water and a few drops of phenolphthalein solution, and titrates to the first lasting pink color. Each student correctly calculates the molarity of a HCl solution. What will the second student's result be? (a) four times less than the first student's result (b) four times greater than the first student's result (c) two times less than the first student's result (d) two times greater than the first student's result (e) the same as the first student's result
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