Acid-Base Titration Acetic Acid Content of Vinegar

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1 Acid-Base Titration Acetic Acid Content of Vinegar Prelab Assignment Read the entire lab. Write an objective and any hazards associated with this lab in your laboratory notebook. On a separate sheet of paper in your laboratory notebook complete data tables that you will fill in during lab. Answer the following questions in your laboratory notebook before coming to lab. 1. Complete and balance the following reactions: a. HCl + NaOH b. H 2 SO 4 + NaOH 2. Calculate the mass of NaOH required to make 1 L of a M NaOH solution. 3. Assume you are titrating 10 ml of vinegar that is 5% acetic acid, CH 3 COOH, by weight with M NaOH. How many ml of M NaOH will be required to reach the equivalence point? For the purposes of this lab assume that the end point of your titration is at the equivalence point of the titration. Assume the density of vinegar is 1 g/ml. Hint: acetic acid, and to convert from grams acetic acid to moles you divide the grams of acetic acid by the molar mass of acetic acid. 4. Briefly describe how you will know that you have reached the endpoint of your titration in this lab. In other words, exactly what will you see happen as you reach the end point of your titration?

2 Acid-Base Titration Acetic Acid Content of Vinegars Introduction Acids and Bases Acids are a class of substances that have similar chemical properties. Acids react with metals to form hydrogen gas. Acids produce carbon dioxide gas when they react with compounds containing carbonate such as limestone. Some dilute acids are common in foods, usually causing a sour taste. Citric and acetic acids are examples of weak acids found in food. You may also have strong acids, such as sulfuric acid, in your car s battery. Different acids have similar chemical properties because they contain and release H + in aqueous solution. Bases are another class of substances with similar chemical properties. One of the properties of bases is that they react with vegetable oils and fats to make soap. Bases feel slippery to the touch because concentrated bases dissolve skin. Ammonia is a common weak base found in household cleaners. Many drain openers or cleaners contain strong bases such as sodium hydroxide. Bases have similar properties because they cause hydroxide ions, OH -, to be present in aqueous solution. Indicators How can we tell if a solution is acidic or basic? One method is to use a chemical called an indicator. Indicators exhibit one color in an acidic solution and a different color in a basic solution. Common indicators include methyl red, which changes from yellow in solutions above a ph of between 4.4 and 6.2 to red as solutions decrease below this ph range, and phenolphthalein, which changes from clear in solutions below a ph of between 8 and 10 to bright pink as solutions increase above this ph range. Titrations A titration is an analytical technique used to determine the concentration of a substance in solution by adding an accurately measured volume of a solution of known concentration, called a titrant, which reacts through known stoichiometry with the substance of unknown concentration. Titrations are often carried out by adding a base of known concentration to an acid, or by adding an acid of known concentration to a base. The net ionic equation for the reaction of a strong acid with a strong base is H + (aq) + OH - (aq) H 2 O(l), and is called neutralization. At the endpoint of an acid-base titration the number of moles of acid or base added has reacted with or neutralized exactly the same number of moles of acid or base in the sample. In other words, at the end point moles acid or base added=moles acid or base in the solution of unknown concentration. The characteristics of the solution being titrated will change dramatically at this point, and a vivid color change in an appropriately selected indicator should occur. The volume of the titrant added during the titration must be carefully controlled and measured. This is done using a buret. Examine the buret carefully before use. Notice that the graduations on the buret

3 are 0.0 ml near the top and increase to 50.0 ml as you move down the buret. Recall that when reading the level of liquid in a buret, always read the lowest point on the meniscus and all readings should be taken at eye level. By interpolating (estimating the values between the markings on the buret), it is possible to determine volumes to an accuracy of 0.01 ml. The volume of titrant added at the end point of the titration is the final buret reading minus the initial buret reading. Titrant is released from the buret by turning the stop cock near the bottom tip of the buret. The stop cock is closed when it is perpendicular to the long cylinder of the buret. As you slowly turn the stop cock toward a parallel alignment with the cylinder of the buret titrant will first begin to drip then flow in a steady stream. You may wish to practice using the buret before you begin a titration. Vinegar Vinegar is a dilute solution of acetic acid in water, and is made from fruit juices. The chemical changes involved in the formation of vinegar are the fermentation of sugar to alcohol by yeast followed by the subsequent oxidation of the alcohol to acetic acid by certain bacteria. The United States Department of Agriculture specifies that the organic acid content of vinegar (expressed as acetic acid) must be at least 4 % by weight. The commercial vinegars that we will be using today all list the acetic acid content as approximately 5 %. The acetic acid content or acidity of vinegar can be calculated from the neutralization reaction of acetic acid using a base of known concentration. We will perform a titration with a M NaOH solution. Neutralization occurs when the moles of acid equals the moles base in the titration vessel. The reaction is CH 3 COOH + NaOH H 2 O + CH 3 COONa Note that in the balanced equation, one mole of acetic acid exactly neutralizes one mole of sodium hydroxide to give water and sodium acetate. To make the endpoint (where the moles of acid equal the moles of base) visible we will add phenolphthalein indicator to the unknown acid solution. Phenolphthalein is colorless in acidic solution (where it is protonated) and pink in basic solution (where the H + dissociates). You should mark the endpoint at the FIRST appearance of CONSISTENT pink color (color persists for seconds with mixing), not after you have developed a deep pink or red color. Procedure 1) Wash the buret with soap and water. After washing, thoroughly rinse the buret with tap water and then with small amounts (~2-5 ml) of distilled water. Close the stopcock and pour about 2 ml of NaOH solution into the buret using a funnel. Rotate the buret in a nearly horizontal

4 position in order to rinse the interior of the buret with base solution. Wear gloves and hold a finger over the end of the buret to rinse it. Place the buret into the buret clamp and drain the rinse solution form the buret into a small beaker (for waste). 2) Close the stopcock and use a funnel to fill the buret with base solution to between 15 and 20 ml from the top. Record the exact volume of base in your lab notebook as your initial reading. All buret readings should be made to two decimal places (for example, 1.05 ml) 3) Add 10 ml of vinegar to a 250 ml Erlenmeyer flask using a graduated cylinder. Add about 75 ml of distilled water and 5 to 6 drops of phenolphthalein indicator to the flask. Shake the bottle of phenolphthalein before use. 4) Titrate the vinegar solution by carefully adding titrant. Gently swirl the vinegar solution in the flask while titrating. Place a piece of white paper under your flask to make the color change at the endpoint easier to see. You may add titrant more quickly at first. Recall that you estimated approximately how much titrant will be required to reach the endpoint in your prelab. As you near the endpoint of your titration add titrant much more slowly drop by drop as you gently swirl the sample and carefully watch for the color change. You will see a pink spot appear where the titrant first falls into the vinegar solution as you near the end point. The pink spot will

5 disappear with swirling. When the pink color spreads to the entire solution and persists for seconds, you have reached the endpoint. If you pass the endpoint you must start over from the beginning. 5) Record the volume of titrant remaining in the buret at the endpoint. Continue to add titrant until the vinegar solution turns bright pink to verify that you have passed the endpoint. 6) Repeat the titration with another 10 ml of vinegar with 75 ml of distilled water.

6 Copy the following data sheet into your lab notebook. Data Sheet NaOH Molarity moles/l Rep 1 Rep 2 Initial buret reading Final buret reading NaOH used, ml NaOH used, L Moles of NaOH used Recall moles = M V Moles of Acetic Acid in Titration Flask (Recall that at the equivalence point moles base added = moles acid in the sample) Molarity (M moles/l) of Acetic Acid in Vinegar Grams of Acetic Acid in Vinegar (Recall that to convert moles to grams you multiply by the molar mass) Weight Percent* of Acetic Acid (Weight percent of acetic acid in vinegar is the mass of a acetic acid in a vinegar sample divided by the total mass of the sample, multiplied by 100) *Assume the density of vinegar is 1 g/ml.

7 Questions 1) Based on your results does the vinegar you titrated meet the US Department of Agriculture standards? 2) Based on your results is the percent by weight of acetic acid indicated on the label of the vinegar you titrated correct? 3) How would you design an experiment to analyze for the percentage of NH 3 (aq) in commercial ammonia? Consider the procedure you used in this lab. Be specific: list at least 5 steps in the procedure; include sample size, identity of titrant, and any indicators utilized.

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