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Chapter 15: Problem 94

Describe the following reaction in terms of the Lewis theory of acids and bases: $$ \mathrm{AlCl}_{3}(s)+\mathrm{CI}^{-}(a q) \longrightarrow \mathrm{AlCl}_{4}^{-}(a q) $$

Short Answer

Expert verified
In Lewis theory, a substance that can accept an electron pair is a Lewis acid, while one that can donate an electron pair is a Lewis base. In the give reaction, AlCl3(s) is the Lewis acid as it accepts an electron pair from Cl^−(aq), the Lewis base, to form the complex ion AlCl4^−(aq).

Step by step solution

01

Understanding Lewis Theory

Lewis theory of acids and bases defines a Lewis Acid as a substance that accepts an electron pair to form a covalent bond. A Lewis base is a substance that donates an electron pair to form a covalent bond.
02

Identify Lewis Acid and Base

In the given reaction, AlCl3(s) can accept an electron pair, so it's a Lewis Acid. Cl^−(aq) can donate an electron pair, making it a Lewis Base.
03

Describing the reaction

In the reaction, the Lewis base (Cl^−(aq)) donates an electron pair to the Lewis acid (AlCl3(s)), forming a covalent bond. This results in the formation of the AlCl4^−(aq) complex ion.

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Most popular questions from this chapter

Consider the two weak acids HX (molar mass = \(180 \mathrm{~g} / \mathrm{mol}\) ) and \(\mathrm{HY}\) (molar mass \(=78.0 \mathrm{~g} / \mathrm{mol}\) ). If a solution of \(16.9 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{HX}\) has the same \(\mathrm{pH}\) as one containing \(9.05 \mathrm{~g} / \mathrm{L}\) of \(\mathrm{HY},\) which is the stronger acid at these concentrations?

The ion product of \(\mathrm{D}_{2} \mathrm{O}\) is \(1.35 \times 10^{-15}\) at \(25^{\circ} \mathrm{C}\). (a) Calculate \(\mathrm{pD}\) where \(\mathrm{pD}=-\log \left[\mathrm{D}^{+}\right]\). (b) For what values of \(\mathrm{pD}\) will a solution be acidic in \(\mathrm{D}_{2} \mathrm{O} ?\) (c) Derive a relation between \(\mathrm{pD}\) and \(\mathrm{pOD}\).

Calculate the concentrations of \(\mathrm{H}^{+}, \mathrm{HCO}_{3}^{-},\) and \(\mathrm{CO}_{3}^{2-}\) in a \(0.025 \mathrm{M} \mathrm{H}_{2} \mathrm{CO}_{3}\) solution.

Why do we normally not quote \(K_{\mathrm{a}}\) values for strong acids such as \(\mathrm{HCl}\) and \(\mathrm{HNO}_{3}\) ? Why is it necessary to specify temperature when giving \(K_{\mathrm{a}}\) values?

What are the Lewis definitions of an acid and a base? In what way are they more general than the Brønsted definitions?
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