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Chapter 7: Problem 28

Which one is more acidic in aqueous solution. (a) \(\mathrm{NiCl}_{2}\) (b) \(\mathrm{FeCl}_{3}\) (c) \(\mathrm{AlCl}_{3}\) (d) \(\mathrm{BeCl}_{2}\)

Short Answer

Expert verified
AlCl鈧� is the most acidic in aqueous solution.

Step by step solution

01

Understanding Acidity Concepts

Acidity in aqueous solutions is related to the ability of a substance to donate protons (H鈦� ions). In the case of metal chlorides, the acidity often increases with the positive charge on the metal ion and the ability of the cation to polarize water molecules, promoting the formation of H鈦� ions.
02

Evaluate Metal Ions

Consider the metal ions in each compound: Ni虏鈦� from NiCl鈧�, Fe鲁鈦� from FeCl鈧�, Al鲁鈦� from AlCl鈧�, and Be虏鈦� from BeCl鈧�. The charge of the metal ion plays a significant role in its acidity due to charge density and its ability to hydrolyze water.
03

Analyze Hydrolysis and Charge Density

Higher charged metal ions tend to have higher acidity because they can polarize water molecules more effectively, leading to increased release of H鈦� ions. Fe鲁鈦� and Al鲁鈦� both have a charge of +3, whereas Ni虏鈦� and Be虏鈦� have a charge of +2.
04

Compare Polarizing Power

Between Fe鲁鈦� and Al鲁鈦�, consider the effective nuclear charge and ionic radius. Al鲁鈦� generally has a smaller ionic radius than Fe鲁鈦�, which means it can polarize water molecules more efficiently compared to other ions with similar charge.
05

Determine the Most Acidic Compound

Based on the analysis, Al鲁鈦� in AlCl鈧� has the highest polarizing power due to its small ionic radius and a high positive charge, making AlCl鈧� more acidic in aqueous solutions compared to NiCl鈧�, FeCl鈧�, and BeCl鈧�.

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Key Concepts

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

Metal Chlorides
Metal chlorides are a group of compounds consisting of a metal cation and a chloride anion. In aqueous solutions, these compounds dissolve in water, and the metal ions play a significant role in determining the properties of the solution. When we consider acidity, it's crucial to understand how the metal ions influence this property:
  • Metal cation's charge: The charge on the metal ion affects its ability to interact with water molecules. Higher charged metal ions tend to exhibit higher acidity in solutions.
  • Solubility in water: The solubility of metal chlorides in water allows the metal ions and chloride ions to dissociate and interact with water molecules, a key factor in exhibiting acidic behavior.
Focusing on the compounds from the exercise - the ability of these metal chlorides to release hydrogen ions (H鈦�) can vary due to differences in the positive charge of the metals and their polarizing abilities.
Cation Polarization
Cation polarization is a critical factor when considering the acidity of metal chlorides in aqueous solutions. Simply put, it refers to the ability of a metal cation to distort or polarize its surrounding water molecules, leading to the release of H鈦� ions. When a cation has a high positive charge and a small ionic radius, it is better at polarizing water molecules. The key points to consider are:
  • Charge density: A cation with a higher charge density will have more influence on surrounding water molecules, breaking the oxygen-hydrogen bond more efficiently, leading to higher acidity.
  • Ionic radius: Smaller ions are typically better at polarizing than larger ions. Therefore, among ions with the same charge, an ion with a smaller size will usually have a stronger polarizing effect.
In the context of the exercise, Al鲁鈦� from AlCl鈧� has a higher polarizing power compared to Ni虏鈦�, Fe鲁鈦�, and Be虏鈦�, mainly due to its high charge and small ionic size.
Acid-Base Chemistry
Acid-base chemistry fundamentally revolves around the concepts of proton donors and acceptors. In aqueous solutions, metal chlorides can influence the concentration of H鈦� ions, thereby affecting the acidity of the solution. When we talk about acidity in metal chlorides, it relates to:
  • Proton donation: The primary measurement of acidity is how easily a compound can donate protons to the solution.
  • Water interaction: Metal ions that can efficiently interact and polarize water molecules encourage a higher release of H鈦� ions, thereby increasing acidity.
By analyzing the metal's properties, such as charge and size, in the compounds presented in the exercise, AlCl鈧� stands out due to its ability to significantly increase the concentration of H鈦� ions in water, marking it as the most acidic among the given options.

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Most popular questions from this chapter

An acidic buffer is obtained on mixing : (a) \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}\) and \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{NaOH}\) (b) \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{HCl}\) and \(200 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{NaCl}\) (c) \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}\) and \(200 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{NaOH}\) (d) \(100 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{HCl}\) and \(200 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{CH}_{3} \mathrm{COONa}\)

How many litres of water must be added to 1 litre an aqueous solution of HCl with a pH of 1 to create an aqueous solution with \(\mathrm{pH}\) of 2 ? (a) \(0.1 \mathrm{~L}\) (b) \(0.9 \mathrm{~L}\) (c) \(2.0 \mathrm{~L}\) (d) \(9.0 \mathrm{~L}\)

\(\mathrm{p} K_{\mathrm{a}}\) of a weak acid (HA) and \(\mathrm{p} K_{\mathrm{b}}\) of a weak base \((\mathrm{BOH})\) are \(3.2\) and 3.4, respectively. The \(\mathrm{pH}\) of their salt (AB) solution is (a) \(7.2\) (b) \(6.9\) (c) \(7.0\) (d) \(1.0\)

The following acids have been arranged in the order of decreasing acid strength. Identify the correct order. \(\mathrm{ClOH}\) (I), \(\mathrm{BrOH}(\mathrm{II}), \mathrm{IOH}(\mathrm{III})\) (a) \(\mathrm{I}>\mathrm{II}>\mathrm{III}\) (b) \(\mathrm{II}>\mathrm{I}>\mathrm{III}\) (c) \(\mathrm{III}>\mathrm{II}>\mathrm{I}\) (d) \(\mathrm{I}>\mathrm{III}>\mathrm{II}\)

For the reaction $$ \left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-} \rightleftharpoons \mathrm{Ag}^{+}+2 \mathrm{CN}^{-} $$ the equilibrium costant, at \(25^{\circ} \mathrm{C}\), is \(4.0 \times 10^{-19} .\) Calculate the silver ion concentration in a solution which was originally \(0.10\) molar in KCN and \(0.03\) molar in \(\mathrm{AgNO}_{3}\).
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