Will either of the following reactions take place to a...

Will either of the following reactions take place to a significant extent as written, according to the data in Table $2-3 ?$ (a) $\mathrm{HCN}+\mathrm{CH}_{3} \mathrm{CO}_{2}-\mathrm{Na}^{+} \quad \stackrel{?}{\longrightarrow} \quad \mathrm{Na}^{+}-\mathrm{CN}+\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$ (b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+\mathrm{Na}^{+-} \mathrm{CN} \quad \stackrel{\mathrm{P}}{\longrightarrow} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-} \mathrm{Na}^{+}+\mathrm{HCN}$

Will either of the following reactions take place to a significant extent as written, according to the data in Table $2-3 ?$
(a) $\mathrm{HCN}+\mathrm{CH}_{3} \mathrm{CO}_{2}-\mathrm{Na}^{+} \quad \stackrel{?}{\longrightarrow} \quad \mathrm{Na}^{+}-\mathrm{CN}+\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$
(b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+\mathrm{Na}^{+-} \mathrm{CN} \quad \stackrel{\mathrm{P}}{\longrightarrow} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{O}^{-} \mathrm{Na}^{+}+\mathrm{HCN}$

Key Concepts

Acid-Base Equilibrium

Acid–base equilibria describe reactions where a proton (H?) is transferred from an acid to a base. The position of the equilibrium is determined by the relative strengths (acidities and basicities) of the substances involved, with the reaction generally favoring formation of the weaker acid and weaker base.

pKa and Acid Strength Comparison

The pKa value of an acid is a numerical representation of its strength; a lower pKa indicates a stronger acid. In analyzing acid–base reactions, comparing the pKa values of the acids on each side of the reaction helps predict which direction the equilibrium will favor, as a reaction tends to proceed toward the formation of the weaker (higher pKa) acid.

Conjugate Acid-Base Pairs

In acid–base reactions, every acid has a conjugate base, and every base has a conjugate acid. The stability and strength of these conjugate pairs are critical in determining the equilibrium. The reaction is favored when a stronger acid and base produce a conjugate acid and base that are both weaker.

Equilibrium Constant

The equilibrium constant (K) quantifies the ratio of product concentrations to reactant concentrations at equilibrium. For acid–base reactions, a large difference in acidity between the reactants and products leads to a K that favors one side, thereby indicating whether the reaction will proceed to a significant extent.

Transcript

00:01 We want to determine whether either of these reactions will take place to any significant extent as range.

00:07 So they mean in the forward direction here.

00:11 And they also tell us to use that table 2 .3, which has the list of pkks to help us do this.

00:18 So what we're going to do is if it is going to occur, we want to go from a stronger acid to a weaker acid.

00:26 So, i mean, that kind of makes sense.

00:28 If you just leave something out spontaneously, we wouldn't expect it to become stronger.

00:36 We would expect it to become weaker.

00:40 So the stronger acid has a lower pca and a weaker acid has a higher pkk.

00:56 Now, a little jingle that i remember for this is low to high, it will fly, high to low, it won't go.

01:07 So let's see if we can apply that jingle to help us figure out if we will have these reactions occur.

01:13 So we first need to identify what is our acid or conjugate acid.

01:16 The conjugate base and base don't really matter all that much for this.

01:21 So we have hcn, so what's its pair? well, it looks like it's going to pair up with sodium cyanide here.

01:30 So it gives away hydrogen, so that means this is going to be our acid.

01:36 And then our other pair is going to be these two.

01:40 So the acetic acid is our conjugate acid.

01:45 Now, if we go and look at that table, it tells us hcn's pca is 9 .31, and this is going to go and become 4 .76.

01:58 6...

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