Identify the Brønsted–Lowry acid and the Brønsted–Lowry base on the left side of each of the following equations, and also identify the conjugate acid and conjugate base of each on the right side: (b) 1CH323N1aq2 + H2O1l2Δ1CH323NH +1aq2 + OH -1aq2

Question

Accepted Answer

Hello everyone today. We are being asked to consider the following reaction. So we have this species here anally reacting with water to perform to give this ammonium funeral ion and hydroxide? We're being asked to determine the bronze Hillary acid and the bronze Hillary base that's on the left side. And then determine the corresponding conjugate acid and conjugate base on the right side. So the first thing I wanna do is you want to note our definitions? So brown said Laurie acid, B. L. A. Is going to be a proton donor. So it is going to donate one H plus ions. Now its corresponding conjugate base is going to have one less so one less hydrogen from our Bronson glory acid. Now our Bronston Laurie base is going to be the opposite. It's going to be a proton except er so it's going to take up a hydrogen plus ion. So that means that its conjugate acid is going to have one more H plus from the Bronson Laurie base. And so with that we can apply these concepts to our equation for part two. So between our an allen and water, we see which one gained a proton and lost a proton on the other side. And so we see that our an alan R C six H five N H two, it's going to be a proton except er because it gained a proton right? If it's a proton except er that makes it our bronze ted Laurie base by default. This makes water our proton donor. And so why is the water the donor? It's because it lost a proton on the right hand side, and so that becomes our browns Hillary acid. Moving to the right hand side. We have to figure out which one is our conjugate acid and base. We look at the newly formed product ammonium ion product, and so we see that it has one greater hydrogen or one more hydrogen from the Bronze Hillary base. This by default makes this our conjugate acid, and then by default, our hydroxide has one less hydrogen than the water, which makes this our conjugate base. And so this is our final answer. I hope this helped. And until next time.

Identify the Brønsted–Lowry acid and the Brønsted–Lowry base on the left side of each of the following equations, and also identify the conjugate acid and conjugate base of each on the right side: (b) 1CH323N1aq2 + H2O1l2Δ1CH323NH +1aq2 + OH -1aq2

Verified Solution

Key Concepts

Brønsted–Lowry Acid-Base Theory

Conjugate Acid-Base Pairs

Chemical Equations and Reaction Dynamics