ACIDS-BASE REACTIONS AND TITRATIONS

One of chemistry's best tricks is to determine the concentration of various substances. Imagine buying vinegar and sometimes the acetic acid concentration is so weak that it tastes like water, and other times it is so strong that it burns the skin off the tongue and throat. So finding concentration is an important skill.

Many substances that we use are either acidic or basic. Because acids and bases can neutralize each other, that gives us a strategy for finding the unknown concentration of an acid or a base when we know the concentration of the other one.

For example, in the last quiz, you did a problem about how lye (NaOH) and aspirin will neutralize each other. In other words, the OH- from NaOH will combine with H+ coming off of aspirin (acetylsalicylic acid) to make H2O.

Let's say we suspect the aspirin tablets do not contain 325mg of aspirin as they claim. If we trust that the NaOH is 100% lye as the lye bottle claims, we can use that to test the amount of aspirin in the tablets. One approach is to figure out equal quantities that will neutralize each other. We take 1 tablet of aspirin and see if the truly has 325mg. To know how many grams of NaOH it would take to neutralize this we have to count the aspirin molecules. So we use the molar mass of aspirin, which is 180.157 g/mole, to count the aspirin molecules. The count for NaOH needs to be the same if they are to neutralize each other. So we turn 325 milligrams of Aspirin into moles. That number of moles is the same for NaOH. Those moles get changed to grams of NaOH.

Instead of using pH paper, we could add a pH indicator such as phenolphthalein. If the color of the solution is purplish, then there was less Aspirin than NaOH meaning there was less than the claimed 325 milligrams. If the solution is clear, then there is equal or more Aspirin than NaOH.

The problem with both of these approaches is they don't tell you how much less or more is the Aspirin compared to NaOH. So we need a better approach.

An improvement was to not to just dissolve the NaOH in water and dump it into a solution of the dissolved Aspirin all at once. The idea was to add it to the solution of dissolved Aspirin a little at a time. We call this method "tritration". "Titrate" comes from "Titer/Titre" which comes from the same word as "title". A title can signify a certain quality like the title of "Premium, champion, first-class, etc". "titre" was a method used to report the quality of gold or silver. So the idea of determining the quality of gold or silver is similar to what we do now we use now to determine the quality (strength) of substance when doing titrations.

Above we calculated that 0.0720 grams of NaOH will neutralize 1 Aspirin tablet. Since 0.0720 g is too small to weigh out, we can make up What we could do is take twice that weight of NaOH (2x0.0720g), which is 0.144 grams and dissolve it in 50mL of water. We could then add this solution of NaOH to the solution of 10 dissolved Aspirin tablets. After adding 25mL, there will be 0.0720 grams of NaOH added, and all of the Aspirin should be neutralized. If it gets neutralized before 25mL, then that means there is less Aspirin than the 325mg expected. If it takes more than 25mL, then the Aspirin present is more than 325mg. The amount of mL more or less than 25mL would let us figure out the actual amount of Aspirin present.

So the problem is that the solution of 0.0000720 moles per mL (0.0720 moles per liter) of NaOH is only approximate. Is there a way to make up a solution of NaOH and then measure its concentration accurately? Yes, there is. It's by using a known amount of acid. One acid that is commonly used is called potassium hydrogen phthalate or KHP for short. This organic acid is a solid and easy to weigh out. It also doesn't absorb water so when exposed to the air, its weight doesn't change.

So the strategy is to first use the NaOH solution to neutralize a known amount of KHP. That will tell you just how much NaOH is in the solution. Then the NaOH solution with an accurately known concentration can be used to neutralize the Aspirin (acetylsalicylic acid) so we can get an accurate concentration of Aspirin.

To the left is the chemical equation for KHP releasing one hydrogen ion. That means each KHP molecule will neutralize one NaOH molecule because H+ + OH- --> HOH.

The procedure is to dissolve 0.3676 grams of KHP in about 50 mL of water and add a couple of drops of phenolphalein to tell us when all of the KHP is neutralized. The solution will turn purplish as soon as there's just a quarter drop NaOH more than what is needed to neutralize the KHP. The KHP solution is put into an Erlenmyer flask like show.

Previously we only made up 50mL of NaOH solution, but this time we want to have extra NaOH so we have enough to do tritrations several times. So let's make a liter of NaOH solution. Our target concentration before was 0.0720 moles per liter, but let's just round that up to 0.1 mole per liter. It's weight then is 0.1 moles x 40.0 grams per mole, which comes out to be 4 grams of NaOH. We weigh out about 4 grams knowing that the weight isn't accurate because NaOH absorbs water. We then dissolve that in 1 liter of water giving us approximately 0.1 moles per liter and put it in a container that has a cap or stopper. CO2 will neutralize the NaOH if left exposed to long. We pour some of this into a 50mL buret and record where the starting volume level. Remember burets have zero at the top. Let's say the level of the NaOH solution reads at the 2.42mL mark (estimated just past the 2.4 line).

We then start adding the NaOH slowly to the flask with the KHP. It's basically let it flow a drop at a time. When it gets close to the point where all of the KHP is neutralized the clear solution of KHP will start to turn purplish but then the color goes away. Each drop added will cause the purplish color to persist longer. At one point the purplish color does not go away. That's when you stop and read the level on the buret. The level has dropped to 19.96 mL mark. The difference from 2.42mL and 19.96mL is 17.54mL. That's the volume of NaOH that has neutralized all of the KHP. Now you can calculate how strong your NaOH solution really is. We know it is in the 0.l mole per liter vicinity, but this pins it down more exactly.

Below are the calculations.

Now we can return to out task of determining if these tablets truly have 325mg of Aspirin in them. We do the procedure just like with did with KHP, but this time our unknown is the Aspirin and our known is the NaOH concentration.

We place a tablet in about 50mL of water and add a couple of drops of phenolphthalein. We refill the buret with more our NaOH solution; however, this time we have an accurate concentration for the NaOH will will give us an accurate determination of the amount of acetlysalicylic acid (Aspirin) in the tablet. The top level of the NaOH solution is read to be at the 1.55mL mark (half way between 1.5 and 1.6 marks). We allow the NaOH solution to flow into the solution with the dissolved Aspirin at a drop by drop rate. As the purplish color appears we slow down the rate of the drops and then do a drop by drop addition of the NaOH solution. At the point we add a drop and the solution stays purplish (for 30 seconds), we then stop. The level is now at the 18.47 mL mark. That means 16.92 mL (18.47-1.55) of 0.1026 moles per liter NaOH solution was needed to neutralize the Aspirin.

See below for calculations

Problem 1: What is the grams of acetic acid per 100 mL of vinegar (M2)?
Problem 2: What is the % w/v of acetic acid for the above brand of vinegar?

Problem 3: What formula do you put in M2? Remember you don't include K3 (100) because that goes directly into M3. You also don't need to include any cells that have a "1" in them.

Problem 4: If A2 goes higher, does that make the final grams (M2) higher or lower?

Oxalic acid is a toxic acid. A person drank some water that had been contaminated with radiator cleaner that contained oxalic acid. The doctors need to know what the concentration was of the oxalic acid in %w/v. You do a titration and came up with the following data: Notice you need the molar mass of oxalic acid and notice that 10.00mL of the oxalic acid solution was used in the titration. Also notice that oxalic acid releases 2 H+ ions.
H₂C₂O₄ --> 2H⁺ + C₂O₄^2-

Problem 5: How many grams of oxalic acid is there per mole (G2)?

Problem 6: How many grams of oxalic acid per 100mL of the sample (M2)?

Problem 7: What is the % w/v of oxalic acid in the sample?

Here's a bottle of Milk of Magnesia (solution of magnesium hydroxide- Mg(OH)₂. The label says 8% w/v. Again, that's just the label. Does it really contain that amount?

We can use a known concentration of an acid to neutralize the magnesium hydroxide using titration methods. On hand we have a solution of 0.1124 molar (moles per liter) HCl. Like what was done with NaOH, we put the known concentraton of HCl solution into a 50mL buret. To know how big of a sample of the Milk of Magnesia to use for the titration, we need to do some preliminary calculations. Titrations are more accurate if you use about 20 or more mL of the titrant (solution in the buret). So let's figure the moles of H+ in 25 mL of the 0.1124 M HCl solution and how many mL of Milk of Magnesia would equal that. Since Mg(OH)₂ has two OH per molecule it only takes half as many moles to neutralize the H+ from HCl.

Problem 8: How many moles of HCl is in 25mL of 0.1124 M HCl solution (H2)?

Problem 9: How many mL of this 8% w/v Mg(OH)₂ is needed to neutralized those 25mL of HCl (H5)?

Problem 10: (was 8) How many grams of magnesium hydroxide per mole of magnesium hydroxide (G2)?

Problem 11: (was 9) How many grams of magnesium hydroxide per 100mL of the sample (M2 with 3 sig figs)?

Problem 12: (was 10) What is the % w/v of magnesium hydroxide in the sample (3 sig figs)?