Write two chemical equations, one that shows H2 O reacting...

Write two chemical equations, one that shows $\mathrm{H}_{2} \mathrm{O}$ reacting (with HBr) as a Bronsted base and a second that shows $\mathrm{H}_{2} \mathrm{O}$ reacting (with $\mathrm{NH}_{3}$ ) as a Bronsted acid.

Key Concepts

Bronsted-Lowry Acid-Base Theory

The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. This concept is fundamental to understanding acid-base reactions where the focus is on the transfer of protons between reactants, highlighting the roles that different species can play in facilitating these transfers.

Amphiprotic Nature of Water

Water is amphiprotic, which means it has the ability to either donate or accept a proton depending on the reaction environment. This dual functionality is key to its role in many chemical reactions, making it capable of acting as either an acid or a base in proton transfer processes.

Proton Transfer Reactions

Proton transfer reactions involve the movement of a proton from one molecule (the acid) to another (the base). This exchange is central to many chemical interactions and underpins the mechanistic understanding of acid-base chemistry.

Conjugate Acid-Base Pairs

In the context of a proton transfer, once an acid donates a proton, it forms its conjugate base, and when a base accepts a proton, it becomes its conjugate acid. Recognizing these conjugate pairs is essential for analyzing the reversible nature and equilibria of acid-base reactions.

Transcript

00:01 Hello everyone.

00:02 Today we're going to be talking about amphiprotic substances, which are substances that can be either an acid or a base, specifically for bronze -dolary acid -based theory.

00:14 In this problem, we're going to look at two separate chemical equations, both with water as one of our reactants.

00:23 The first reaction is hbr, which will likely be a gas, reacting with water, the second reaction is ammonia and h3, also a gas reacting with water.

00:54 And let's take a look at the products that these form.

00:57 This is going to form, i'm going to put the bromide ion first, br minus, and h3o plus.

01:13 Now according to bronstead lorry, an acid is a proton or hydrogen.

01:18 Ion donor.

01:21 Hydrogen bromide is an acid.

01:27 It has this hydrogen ion to donate.

01:30 And then if we go over to the other side, this is also an acid because it has a hydrogen ion to donate.

01:41 That makes this a base.

01:45 This is a base.

01:46 And let's double check.

01:47 Remember, a base is a hydrogen ion accepter.

01:51 This br can accept a hydrogen to become hbr.