Question
16) (8 pts:) For the proton transfer reaction below:Acid pKaConj: Acid pKaDraw the mechanism and show the productsUsing Table 2.1, determine the approximate pKa of the acid and conjugate acidIndicate the direction of equilibrium using appropriate equilibrium arrows.Draw reaction coordinate diagram that illustrates the energetics of the reactionReaction coordinate
16) (8 pts:) For the proton transfer reaction below: Acid pKa Conj: Acid pKa Draw the mechanism and show the products Using Table 2.1, determine the approximate pKa of the acid and conjugate acid Indicate the direction of equilibrium using appropriate equilibrium arrows. Draw reaction coordinate diagram that illustrates the energetics of the reaction Reaction coordinate
Answers
For each acid and base given in this section, complete a protontransfer equation for the transfer of one proton. Predict the direction in which the resulting equilibrium will be favored. $$\mathrm{HSO}_{4}^{-}(\mathrm{aq})+\mathrm{HC}_{2} \mathrm{O}_{4}^{-}(\mathrm{aq}) \rightleftharpoons$$
Question. Number 26 is a continuation of the concept of first identifying what is the acid base reaction and then identifying where the equilibrium lies. The reaction that is given is the reactant H c n with H C three c O minus. The only one that conserve is an acid, in this case is the one that has a hydrogen ion up front that could be donated So the H C N is going to donate its hydrogen ion to the acetate ch three c o minus and produce C and minus and acetic acid in order to determine where the equilibrium lies. We need to identify the strength of the acids. The two acids are acetic acid and hydrogen tannic acid going to table 17 1. We see that hydro satanic acid is the weaker acid and the weaker acid. Our and the equilibrium always favors decide that has the weaker acid, so the equilibrium favors the reactant sor the reactant side
Questions 25 through 34 are all pretty much the same were given reactant. One reactant is an acid. The other, reactant, is a base. In order to identify which one is going to serve as the acid and which one is going to serve as the base for the first few, it is the one that does not have a hydrogen ion is going to serve as the base. So we'll stick with that for now until we get to some of the more challenging ones. So for the first chemical reaction, we will, right? What was given to us as the reactant We see that the species that does not have a hydrogen ion will serve as the base. This one will serve as the acid. So this hydrogen will then be noted, donated thio the P O for three minus. And these will be the products that we get C three h 50 to minus. In order to determine in which direction they were, equilibrium is favored. We simply need to identify the two acids. After we have identified the two acids, we then go to table 17 1 and determine which one is the weakest. The equilibrium will always favor the side With the weakest acid, we see that H peel four to minus is weaker than H C three h 502 So because a product has the weaker acid, it's going to favor the product side again. It always favors the side that has the weakest acid.
Question Number 27 also gives you just the reactant. It wants you to identify what the products are for an acid base reaction and then determine where the equilibrium lies on the product side or the reactant side. First, we need to identify what the products are. We see that this has ah, hydrogen I and it can donate. This doesn't so this will serve as our acid carbonate will serve as our base. We will produce hydrogen carbonate as one of the products when carbonate takes on the hydrogen ion and sulfate as the other product. When hydrogen sulfate gives up its hydrogen ion, we then need to go to the table 7 17 1 and find the two acids H C 03 minus and H s 04 minus and determine which one is weakest. It turns out that hydrogen carbonate is the weaker of the two acids and the equilibrium will always favor the side that has the weaker acid. Therefore, this equilibrium is going to favor the product side
Question. Number 34 is the last one in the long list of chemical reactions for which you have been given just the reactant, and you're asked to complete the reaction as if it were an acid based reaction. Then identify on which side, um, the equilibrium lies or which side of the equilibrium is favored. The reactant in this case are H P 04 to minus and acetic acid H C two h 302 so they both could serve his acids. If you go to the table 17 1, you will find that they are both listed as acids in the table. The one that is going to service the acid in the chemical reaction will be the one that is the stronger of the two acids. So it turns out that acetic acid is a stronger acid than H P 04 to minus. So this will service the acid and donate ah hydrogen ion to H P 04 to minus producing h two peel four minus and the acetate an ion. So now what we have to do is compare the conjugate acid that was created, the strength of the conjugate acid that was created to the strength of the acid that reacted in order to determine the side that equilibrium favors. It turns out that H to peel for minus is the weaker of the two acids. And because equilibrium always favors the side that has the weaker acid, then this equilibrium will favor the product side, producing more product than there is reactant once equilibrium is reached.