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Problem 65 Hard Difficulty

The concepts of acid–base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted–Lowry acid–base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia, $\mathrm{NH}_{3}$ .
a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia.
b. Write a chemical equation indicating how $\mathrm{OH}^{-}$ behaves as a base in liquid ammonia.

Answer

(a) $H C l+N H_{3} \rightarrow N H_{4}^{+}+C l^{-}$
(b) $N H_{3}+O H^{-} \rightarrow N H_{2}^{-}+H_{2} O$

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Video Transcript

Okay, Sis Lerby A review on Bronston Laurie Assets and basis. So under this definition, in acid is a species access a pro time donor and a base of the species the access of proton Except er So in this case, we're just talking about the transfer of a proton from one species to another. So we often use these two equations that I have written here to describe the association of either a weak acid or a weak base in solution. So often we apply this definition when we're talking about a Prius systems, So something in which water is the solvent. So you see it from the one that I have on the top here. I'm representing the weak acid in this case as H A. So as it associates and water, it's transferring this acidic proton here to the water molecule to form this hydro Nia my on as well as its congregate base, which is the A minus. On the other hand, if we talking said about the base as they interact with water, the base will be picking up a proton or accepting a proton. And we have it's country get after it formed as well as the hydroxide ion. So as I mentioned, usually we talk about water being solvent here, and water is an important part in the reaction equation. We can extend this definition to talk about systems in which we have a solvent that's different than water. So one example that we can use is it. We're talking about a solvents such as liquid ammonia, so ammonia is and each story So just a quick note on this. I probably done some previous examples where you talk about ammonia. Ennis cashes form, so ammonia is a gas at room temperature. When it's very, very cold, it will be in the liquid fees. So if we're talking about ammonia basically stepping in and taking the place of water in this reaction, we can see how the pro time transfer sort of proceeds. So let's use, for example, hydrochloric acid. So H CEO. So we know this is a strong acid, so it should be acting as a Proton donor. And just like the equation we have up here, it would be transferring the proton to the ammonia, so we'll then have it in its pro donated form and each four so the ammonium ion and then the conjugal base over acid, which is just the chloride ion. Soon as that, instead of the equilibrium arrows just using the Ford Arrow because we have hydrochloric acid, which is a strong acid. What? We're talking about the same sort of reaction here so we can have the same sort of reaction if we're talking about a base as well. So we have our liquid ammonia in hydroxide. I am so this is O H. Minus. So we know this is going to be acting as a base. So we know that under the brown, said Lori definition of a base that needs to act as a proton except er so again the proton will be coming from. In this case, it was coming from the water molecule. So it's going to be coming from the ammonia when pneumonias a solvent. So if we d prone eight ammonia, we're then going to have an each to it lost one of its protons, so we'll have a minus one charge and will that be picking up the proton the base? So this will become water with no chart, so you can see from both of these equations here that we can apply the bronze, said Lori Definitions for acid and base, four solutions that don't have water as a solvent, and we showed that with liquid ammonia.

Topics

Liquids

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