Use this list of important industrial compounds (and Figure...

Use this list of important industrial compounds (and Figure 14.8 ) to answer the following questions regarding: $\mathrm{CaO}, \mathrm{Ca}(\mathrm{OH})_{2}, \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}, \mathrm{CO}_{2}, \mathrm{HCl}, \mathrm{H}_{2} \mathrm{CO}_{3}, \mathrm{HF}, \mathrm{HNO}_{2}, \mathrm{HNO}_{3}, \mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{NH}_{3}, \mathrm{NaOH}, \mathrm{Na}_{2} \mathrm{CO}_{3}$ (a) Identify the strong Bronsted-Lowry acids and strong Bronsted-Lowry bases. (b) List those compounds in (a) that can behave as Bronsted-Lowry acids with strengths lying between those of $\mathrm{H}_{3} \mathrm{O}^{+}$ and $\mathrm{H}_{2} \mathrm{O}$ (c) List those compounds in (a) that can behave as Bronsted-Lowry bases with strengths lying between those of $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{OH}^-$.

Use this list of important industrial compounds (and Figure 14.8 ) to answer the following questions regarding: $\mathrm{CaO}, \mathrm{Ca}(\mathrm{OH})_{2}, \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}, \mathrm{CO}_{2}, \mathrm{HCl}, \mathrm{H}_{2} \mathrm{CO}_{3}, \mathrm{HF}, \mathrm{HNO}_{2}, \mathrm{HNO}_{3}, \mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{NH}_{3}, \mathrm{NaOH}, \mathrm{Na}_{2} \mathrm{CO}_{3}$ (a) Identify the strong Bronsted-Lowry acids and strong Bronsted-Lowry bases.
(b) List those compounds in (a) that can behave as Bronsted-Lowry acids with strengths lying between those of $\mathrm{H}_{3} \mathrm{O}^{+}$ and $\mathrm{H}_{2} \mathrm{O}$
(c) List those compounds in (a) that can behave as Bronsted-Lowry bases with strengths lying between those of $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{OH}^-$.

Key Concepts

Comparative Acid-Base Strength Relative to Water

Water plays a dual role in acid–base chemistry as both a proton donor and acceptor. The strength of acids and bases is often gauged relative to water, with substances that donate protons more readily than water being considered strong acids, and those that accept protons more readily than water being strong bases. Understanding these reference points is key in classifying and predicting the behavior of various compounds, especially in industrial chemistry.

Bronsted-Lowry Acid?Base Theory

This concept defines acids as substances that donate protons (H+) and bases as those that accept protons. It provides a framework for understanding proton-transfer reactions and is central to classifying substances as acids or bases in aqueous solutions. This theory helps explain the behavior of many compounds in industrial and laboratory settings through the identification of donor and acceptor properties.

Acid and Base Strength

Acid and base strength refers to the degree to which an acid can donate a proton or a base can accept a proton. In the context of the Bronsted-Lowry theory, strong acids and bases ionize completely in water, whereas weak acids and bases only partially ionize. This concept is crucial when comparing compounds to reference points such as H3O+ (the strongest acid in water) and OH– (the strongest base in water), as well as in determining intermediate strengths.

Transcript

00:01 So this problem gives us a list of different compounds and asks us to choose the bronzed lowry strong acids and bases.

00:11 Now to solve this problem, we're going to want to have a good understanding of what exactly is the bronset -lauri definition of acids and bases.

00:21 So under the bronsid -lowary definition, an acid is any compound that, when placed in an acquivis solution, will donate protons or hydrogen and ions.

00:32 Now, when you're talking about acids and bases, the terms proton and hydrogen ion will be used pretty much interchangeably.

00:40 And then a base would be any compound that accepts a hydrogen ion or a proton in an aqueous solution.

00:48 Now, i've written down a quick example of each.

00:51 So hydrochloric acid, when placed in water, will dissociate to form chlorine ion and hydrogen ion and hydrogen ion.

01:01 So you can think of this as the acid donating the hydrogen to the water.

01:08 And then the base is kind of the opposite, so this is ammonia in water, and this will dissociate to form an ammonium ion and hydroxide ion.

01:21 So here the base is accepting a hydrogen from the water.

01:29 And out of these acids and bases, some of them are stronger than a hydrogen from the water.

01:33 Others and basically what that means is some will dissociate completely in an acreous solution and others will not so for example this hydrochloric acid when place in water it will completely turn into chlorine ions and hydrogenium but ammonia will dissociate only partially so out of the the acids there are seven strong ones which you should probably memorize.

02:05 And out of the bases, the strong ones are basically just hydroxide of the group 1 metals and strontium beryum and calcium hydroxide.

02:16 All right, now back to the problem.

02:19 Part a wants us to identify all the strong acids and bases.

02:24 So for the strong acids, which i'll do first, all we are looking for are the acids that are in this list of seven.

02:31 So if you look at the list, we can see hydrochloric acid, let me do that in red, hydrochloric acid, nitric acid, and sulfuric acid.

02:46 Now, these in the list are the only strong acids.

02:50 Now, that doesn't mean that they're the only acids.

02:53 This is carbonic acid, hydrofluoric acid.

02:55 Now, the strong acids that i've marked are the ones that are going to dissociate completely in water...

Please give Ace some feedback