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Chapter 2: Problem 35

A sample of solid \(\mathrm{MgCl}_{2}\) would be most soluble in which of the following solutions? (A) \(\operatorname{LiOH}(a q)\) (B) \(\operatorname{CBr}_{4}(a q)\) (C) \(\operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) (D) \(\mathrm{AlCl}_{3}(a q)\)

Short Answer

Expert verified
The sample of solid \(\mathrm{MgCl}_{2}\) would be most soluble in \(\mathrm{AlCl}_{3}(a q)\).

Step by step solution

01

Identify the Anion in \(\mathrm{MgCl}_{2}\)

The given salt is \(\mathrm{MgCl}_{2}\) and the anion in this salt is Cl-.
02

Compare the anion with the ions in given solvents

Now the aim is to find out a solvent which also has Cl- ions. Going through the solvents,(A) \(\operatorname{LiOH}(a q)\): Here, the solvent does not have Cl- ion.(B) \(\operatorname{CBr}_{4}(a q)\): This solvent also does not have Cl- ion.(C) \(\operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\): This solvent also does not have Cl- ion.(D) \(\mathrm{AlCl}_{3}(a q)\): This solvent does have Cl- ions.
03

Choose the correct option

The solvent with the same anion as the given salt is \(\mathrm{AlCl}_{3}(a q)\). So, \(\mathrm{MgCl}_{2}\) would be most soluble in \(\mathrm{AlCl}_{3}(a q)\) .

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Key Concepts

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

Ionic Compounds
Ionic compounds are formed when atoms bond together through the transfer of electrons. In these compounds, one atom donates electrons and becomes a positive ion, or cation, while the other atom accepts electrons and becomes a negative ion, or anion. The electrostatic attraction between oppositely charged ions holds the compound together.To better understand this, consider the example of magnesium chloride (\( \text{MgCl}_2 \)). Here, magnesium (\( \text{Mg}^{2+} \)) is the cation, while chlorine (\( \text{Cl}^- \)) is the anion. The ratio in which these ions combine creates a neutral compound, hence the formula \( \text{MgCl}_2 \).
  • Strong Ionic Bonds: These result from the electrostatic forces which create a lattice structure where each ion is surrounded by ions of opposite charge.
  • Solubility: This is influenced by the lattice energy and the hydration energy when ionic compounds dissolve in water.
Ionic compounds like \( \text{MgCl}_2 \) dissociate into their respective ions when dissolved in water, allowing ions to move freely.
Anion Comparison
In anion comparison, the presence of common ions in a solution affects the solubility of a compound. This concept is included in the solubility rules used to predict the solubility of ionic compounds in water. The solubility of a salt can decrease if a common ion is present in the solution. For instance, in the exercise featuring \( \text{MgCl}_2 \), the anion is \( \text{Cl}^- \).
  • Anion Matches: The solution containing \( \text{AlCl}_3 \) also has \( \text{Cl}^- \) ions. Due to common ion presence, it affects the solubility of \( \text{MgCl}_2 \) in \( \text{AlCl}_3 \) solution.
  • Solubility Trends: Generally, when an anion matches between a solute and solvent, it influences the behavior of the solubility.
This idea guides us to predict which solutions will allow salts to dissolve or precipitate when introduced into them.
Common Ion Effect
The common ion effect describes the decrease in solubility of a solute due to the presence of a common ion. This effect illustrates how the addition of a common ion shifts the equilibrium of a dissolving ionic compound.Taking our case with \( \text{MgCl}_2 \), a solution containing the same \( \text{Cl}^- \) ions, such as \( \text{AlCl}_3 \), demonstrates this principle.
  • Ionic Equilibrium: The dissolution of compounds in water reaches an equilibrium state. When a common ion is present, it shifts the equilibrium towards the formation of the solid, reducing solubility.
  • Le Ch芒telier's Principle: This principle predicts that an equilibrium will adjust to counteract the change, in this case, the change being the addition of a common ion.
Understanding the common ion effect is crucial in predicting how mixtures behave in various solutions, particularly in chemical reactions and processes where solubility is a factor.

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Most popular questions from this chapter

Consider the Lewis structures for the following molecules: $$\begin{equation} \mathrm{CO}_{2}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-}, \text {and } \mathrm{NO}_{3}^{-} \end{equation}$$ Which molecules are best represented by multiple resonance structures? (A) \(\mathrm{CO}_{2}\) and \(\mathrm{CO}_{3}^{2-}\) (B) \(\mathrm{NO}_{2}^{-}\) and \(\mathrm{NO}_{3}^{-}\) (C) \(\mathrm{CO}_{3}^{2-}\) and \(\mathrm{NO}_{3^{-}}^{-}\) (D) \(\mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-},\) and \(\mathrm{NO}_{3}^{-}\)

Which of the following pairs of ions would make the best buffer with a pH between 6 and 7? \(K_{\mathrm{a}}\) for \(\mathrm{HC}_{3} \mathrm{H}_{2} \mathrm{O}_{2}=1.75 \times 10^{-5}\) \(K_{\mathrm{a}}\) for \(\mathrm{HPO}_{4}^{2-}=4.8 \times 10^{-13}\) (A) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{H}_{2} \mathrm{PO}_{4}\) (B) \(\mathrm{HPO}_{4}^{2-}\) and \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) (C) \(\mathrm{HC}_{3} \mathrm{H}_{2} \mathrm{O}_{2}\) and \(\mathrm{NaC}_{3} \mathrm{H}_{2} \mathrm{O}_{2}\) (D) \(\mathrm{NaOH}\) and \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

\(14 \mathrm{H}^{+}(a q)+\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+3 \mathrm{Ni}(s) \rightarrow\) \(2 \mathrm{Cr}^{3+}(a q)+3 \mathrm{Ni}^{2+}(a q)+7 \mathrm{H}_{2} \mathrm{O}(l)\) In the above reaction, a piece of solid nickel is added to a solution of potassium dichromate. Which species is being oxidized and which is being reduced? \(\quad\) Oxidized \(\quad\) Reduced (A) \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q) \quad \mathrm{Ni}(s)\) (B) \(\mathrm{Cr}^{3+}(a q) \quad \mathrm{Ni}^{2+}(a q)\) (C) \(\mathrm{Ni}(s) \quad \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)\) (D) \(\mathrm{Ni}^{2+}(a q) \quad \mathrm{Cr}^{3+}(a q)\)

An unknown substance is found to have a high melting point. In addition, it is a poor conductor of electricity and does not dissolve in water. The substance most likely contains (A) ionic bonding (B) nonpolar covalent bonding (C) covalent network bonding (D) metallic bonding

Consider the Lewis structures for the following molecules: $$\begin{equation} \mathrm{CO}_{2}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-}, \text {and } \mathrm{NO}_{3}^{-} \end{equation}$$ Which molecule would have the shortest bonds? (A) \(\mathrm{CO}_{2}\) (B) \(\mathrm{CO}_{3}^{2-}\) (C) \(\mathrm{NO}_{2}^{-}\) (D) \(\mathrm{NO}_{3}^{-}\)
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