Experiment 10. Acid Base Titration

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1 Experiment 10 Acid Base Titration Definitions: Titration A technique to accurately and precisely measure something, most often acids or bases Acids Most acids are molecules that behave as if they were ionic compounds in which the cation is the hydrogen cation, H + (which happens to be a proton). When acids dissolve in water, they release an H + cation (hydrogen ion), which binds to water. Reminder: Acids sometimes undergo a name change when they are dissolved in water, e.g. Hydrogen chloride becomes hydrochloric acid. Bases A soluble compound containing the OH - anion (hydroxide) is called a base. Note: NH 3 is a special case. NH 3 dissolves in water, but is also thought to react slightly with water to also produce some hydroxide anion: NH 3 + H 2 O + NH 4 + OH -. Concentration: Molarity The ratio of the number of moles to a fixed volume, the liter, is given the name: Molarity (M) Molarity (M) = moles of solute / liters of solution M = mol / L Neutralization Reactions: Acid Base Titration Acid-Base reactions (H + + OH - H 2 O) are also called Neutralization Reactions

2 We use neutralization reactions to determine the concentration of an unknown acid or base The procedure of neutralization is called a titration. With this procedure we carefully add just enough acid solution to neutralize a known volume of a base solution - Or visa versa A dye such as phenolphthalein, that changes color when the [H + ] 1 x 10-7 M, is employed in the solution to indicate when neutrality has been reached. The dye, phenolphthalein changes from colorless to a pink color as soon as any excess OH - occurs. The change may require only a single drop (50 µl) of your acid solution Reading a Buret:

3 Must read with proper line of sight to avoid parallax error Example Calculation: What volume of a M HCl solution is required to neutralize 25.0 ml of a M NaOH solution? Solution: 1. Label the knowns and unknowns, e.g.: What volume (V1) of M HCl (M1) solution is required to neutralize 25.0 ml (V2) of a M NaOH (M2) solution? 2. Substitute into the following equation and solve for V 1 : M 1 x V 1 = M 2 x V 2 (0.100 M HCl) (V 1 ) = (0.350 M NaOH) ( 25 ml) V 1 = [(0.350 M NaOH) (25 ml)] / M HCl V 1 = 87.5 ml Today s experiment: HCl concentration = moles / liter = Moles / L

4 Careful technique is critical to good results Grading will be based on accuracy in determining an unknown base solution Equipment: Two separate check out steps: 1. Check out two burets and a buret clamp You will also need a spare waste beaker Must work with great care at all times to avoid breaking off the glass tips during: Cleaning Handling Titration Check burets for cleanliness Rinse with water. No water droplets on inside Use small beakers for adding water for rinsing Wash with soap and buret brush if water beads up Note: Measurements are to hundredths of a ml, and a single drop of water 50 µl or 5 hundredths of a ml. Extra water droplets adhering to the walls of the cylinder can significantly affect accuracy. Rinse burets Rinse with tap water several times including the stopcock and tip Final rinse with deionized water Check to be sure stopcocks are secure 2. Check out reagents: Exchange a clean 250 ml Florence flask and a 250 ml beaker for the reagents in comparable containers Note: The Florence flask contains 250 ml of the unknown NaOH. The same solution will be employed next week, so use it sparingly and appropriately. Write your name on the Florence flask with a Sharpie. When done, seal the flask with Parafilm and store in a designated cupboard.

5 Burets: Final preparation Complete two careful 5 ml rinses with the reagent prior to filling each buret Red buret for acids Blue buret for bases Titration Measurements Measures volume to one hundredths of a milliliter Use small funnels for adding reagents to burets Add reagents to just below the 0 ml mark Run some reagent out to fill the stopcock and tip Trick to reading the meniscus: hold something behind the cylinder Accurately read / record the initial volume reading. Starting at an exact number is not important. Accurately reading the number is. Part I Add approximately 20 ml of HCl and then accurately read the volume reading. This will be recorded at the initial HCl reading. Add two drops of phenolphthalein Begin titrating with your unknown NaOH solution, swirling the flask as needed As the volume of NaOH approaches the HCl volume, slow the addition to about a drop every 5 seconds while continuing to swirl the flask Neutralization is completed with the clear solution turns permanently slightly pink with the addition of a single drop. Record your final volume as the final reading Complete your calculations of the NaOH concentration and bring to the instructor for review before completing your remaining runs Part II Check burets for cleanliness Rinse with water. No water droplets on inside Use small beakers for adding water for rinsing Wash with soap and buret brush if water beads up

6 Note: Measurements are to hundredths of a ml, and a single drop of water 50 µl or 5 hundredths of a ml. Extra water droplets adhering to the walls of the cylinder can significantly affect accuracy. Rinse burets Rinse with tap water several times including the stopcock and tip Final rinse with deionized water Check to be sure stopcocks are secure Unknown Acid Concentration Today, you will be given an unknown acetic acid (HC 2 H 3 O 2 ) solution. There are several different possible unknown solutions. You will be graded on how close your experimental value comes to the true value of your unknown. Record your locker number on your Part II worksheet. Note that the data sheet for Part II is the reverse of that for Part I (acid and base parts have been reversed) The calculations are also reversed: M a V a = M b V b. This time you are solving for M a. Note that this week, your unknown will require anywhere from ml of your standard NaOH solution, depending on which unknown you have. You may wish to make a rough cut of how much NaOH you will need by taking a couple of ml of unknown and titrating it to get into the range of NaOH you will need. Then you can make adjustments as to how much acid and base you will need for your accurate titration. You will use the NaOH value you determined from Part I. Check your returned Part I for any corrections you may need to incorporate. Be watchful of how much of your NaOH you use. You should have enough for approximately 4 titrations of the unknown acid concentration. M a V a = M b V b Calculation of mass percent: Mass % = g solute / g solution

7 Molarity = moles HC 2 H 3 O 2 / L solution Molar mass of HC 2 H 3 O 2 = g. Mass % acetic acid = g HC 2 H 3 O 2 / g solution (Assume the density of the solution is 1.00g / ml) Assume the density of the solution is 1.00g / ml (this will work up to three sig figs). Mass % acetic acid = (moles HC 2 H 3 O 2 / L) x (conversion moles to g) x (conversion L solution to g).

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