An Acid-Base Titration Lab Define Lewis acids and bases. Give an example of each

Question

An Acid-Base Titration Lab

Define Lewis acids and bases. Give an example of each.

Based on the Brønsted-Lowry theory of acids and bases, complete the equations for the following acid-base reactions. In your answer be sure to indicate each conjugate acid-base pair:

HNO3 + OH- à

CH3NH2 + H2O à

OH- + HPO4-2 à

When discussing the theories of acids and bases, the Arrhenius, Brønsted-Lowry, and Lewis theories will each describe compounds in their own unique and different way. Based on each of the three theories, describe KOH.

4.Water is a substance that can act as both an acid and a base. Explain this based on the three ways that you can use to define acids and bases.

Explanation / Answer

1.Lewis acid: Any substance that accepts a pair of electrons is called Lewis acid

Ex: All cations, AlCl3 etc.,

Lewis Base: Any substance that donates a pair of electrons is called Lewis base

Ex: All anions, NH3 etc.,

2. A pair of substances that differentiated by a proton is said be its conjugate acid/base

HNO3(acid) + OH-(base) ----> H2O(conjugate acid of OH-) + NO3- (conjugate base of HNO3)

CH3NH2(base) + H2O(acid) ----> CH3NH3+(conjugate acid of CH3NH2) + OH-(conjugate base of H2O)

OH- (base)+ HPO4-2(acid) ----> H2O (conjugate acid of OH-)+ PO43-(conjugate base of HPO42-)

3. According to Arhenius theory, KOH is a base because it produces OH- ions in water

According Bronsted-Lowry theory, it is a base because it accepts H+ with acids

KOH + HCl ----> KCl + H2O

According to Lewis theory, KOH is a base because it donates a pair of electrons to bind with proton

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