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Chapter 6: Q28P (page 143)

Distinguish Lewis acids and bases from Brønsted-Lowry acids and bases. Give an example of each.

Short Answer

Expert verified

The differences between Bronsted-Lowry acid and bases and Lewis acids and bases are given below:

Bronsted –Lowry concept	Lewis concept
The Bronsted-Lowry acid dissociates in aqueous solution to give ions.	The Lewis acid can accept a pair of electrons.
The Bronsted-Lowry base dissociates in aqueous solution to give ions.	The Lewis acid can donate a pair of electron.

Step by step solution

01

Bronsted-Lowry acid and bases.

The Bronsted-Lowry acid is a chemical species which is capable of donating a proton in an aqueous solution.

An example of Bronsted-Lowry acid is HCI.

$HCI + H_{2} O \to {CI}^{+} + H_{3} O^{+}$

The Bronsted-Lowry base is a chemical species which can liberate OH ions in aqueous solution.

An example of Bronsted-Lowry base is NaOH.

$NaOH (aq) \to {Na}^{+} (aq) + {OH}^{-} (aq)$

02

Lewis Acid and Base.

The chemical species which is able to accept a pair of an electron called Lewis acid. Lewis acids have vacant orbitals where they can accept electron pairs.

An example of a Lewis acid is ${BF}_{3}$ .

The chemical species which can donate a pair of electrons is called a Lewis base.

An example of a Lewis base is ${NH}_{3}$

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Most popular questions from this chapter

For $H_{2} (g) + B r_{2} (g) ⇌ 2 H B r (g), K = 7.2 \times 10^{- 4}$ at 1362Kand $∆ H^{°}$ is positive. A vessel is charged with $48.0 Pa H Br, 1370 Pa H_{2}$ , and $3310 Pa {Br}_{2}$ at1362K.

(a) Will the reaction proceed to the left or the right to reach equilibrium?

(b) Calculate the pressure (Pa) of each species at equilibrium.

(c) If the mixture at equilibrium is compressed to half of its original volume, will the reaction proceed to the left or the right to re-establish equilibrium?

(d) If the mixture at equilibrium is heated from 1362 to 1407K , will HBr be formed or consumed in order to re-establish equilibrium?

Identify the conjugate acid-base pairs in the following reactions:

(a) $H_{3} {NCH}_{2} {CH}_{2} {NH}_{3} + H_{2} O ⇌ H_{3} {NCH}_{2} {CH}_{2} {NH}_{2} + H_{3} O^{+}$

(b) Benzoicacid+ Pyridine $⇌$ Benzoate+ Pyridinium

Find $[Cu *]$ in equilibrium with CuBr(s) and 0.10MB $r^{-}$ .

For the reaction ${HCO}_{3}^{-} ⇌ H^{+} + " {CO}_{3}^{2 -}$ , $ΔG ° = + 59.0 kJ / mol$ at $298.15 K$ . Find the value of Kfor the reaction.

Find $[{Cu}^{2 +}]$ in a solution saturated with ${Cu}_{4} {(OH)}_{6} ({so}_{4})$ if $[{OH}^{-}]$ is fixed at $1.0 \times 10^{- 6} M$ . Note that ${Cu}_{4} {(OH)}_{6} ({so}_{4})$ gives 1mol of ${SO}_{4}^{2 -}$ 4 mol for of ${Cu}^{2 +}$ .

${Cu}_{4} {(OH)}_{6} ({so}_{4}) (s) ⇋ 4 C u^{2 +} + 6 O H^{-} + S O_{4}^{2 -} K_{s p} = 2.3 \times 10^{- 69}$

See all solutions

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