Determination of Acetic Acid in Vinegar using a pH Electrode Bryan Nuno Group: (Black) 212 Peter Ruggles Introduction: In the first investigation of the lab, the objective was to take the different household items and determine the pH of each of them. In investigation two, the objective was to use acetic acid in distilled white vinegar and find the percent composition of it. In the first investigation of the laboratory, it was important to find whether the household items were basic or acidic. To continue through the experiment, a temperature probe and pH electrode was used. It would be classified as a base, if the number given by the probe was higher than seven.
Esterfication Abstract: Through the process of esterification, carboxylic acid was reacted with an alcohol in order to produce an ester and water as the products. An acid called benzoic acid was reacted with an alcohol identified as ethanol. Through the use of heat and a catalyst, which in this case was sulphuric acid, an ester in the form of ethyl benzoate was produced along with water. The cherry odour comes from the ester called ethyl benzoate. Theory: The purpose of this lab is to achieve a specific odour through the process of esterification where carboxylic acid and alcohol react to produce an ester and water with the assistance of heat and a catalyst such as sulphuric acid.
Skip questions B, C, D, E and F in the lab manual, and answer these instead: A. What is the average % acetic acid in your vinegar sample? Standard vinegar is 5% acetic acid.How does your result compare with the standard? G. A 5.0 mL sample of vinegar was titrated with 7.2 mL of 0.55 M NaOH(aq). If the density of the vinegar solution is 1.00 g/mL, what is the mass percent of acetic acid present?
Results Sheet, Experiment 13 Brand of Vinegar used:________________ Acetic Acid % from bottle label_____________ | Initial NaOH Reading(estimate to 0.1 mL) | Final NaOH Reading(estimate to 0.1 mL) | Volume NaOH used(Final – Initial) | Trial 1 | 9.5 | 1.3 | 8.2 | Trial 2 | 9.6 | 1.4 | 8.2 | Trial 3 | 9.7 | 1.4 | 8.3 | Average Volume of NaOH used | 8.2 | Calculations: Normality of the acetic acid: .82 Mass of acetic acid: 49.2 % acetic acid (divide the grams, above, by the volume you used to get g/L): 4.92 Answer questions A-G in the lab manual: A. What is the average % acetic acid in your vinegar sample? Standard vinegar is 5% acetic acid. How does your result compare with the standard? The average was 4.92 which is pretty close comparably to the standard.
Record them. 3) Measure the temperature of the vinegar in the beaker using a thermometer. Record it. 4) Drop the tablet of alka-seltzer into the beaker of vinegar. Record ur observations.
Exploring enzymes through Lactex. Problem: Does pH affect the results of Lactex? Independent Variable: pH value Dependent Variable: Glucose Control: Lactex enzyme Hypothesis: I think pH will cause the result of Lactex to change. Materials: · Soap (basic) · Antacid (basic) · Soda (acidic) · Vinegar (acidic) · pH test strips · eye dropper · Cow’s milk Experimental Design: 1. Set up plastic cups 2.
Amylase breaks down amylase and amylopectin (which are starches found commonly in foods such as pasta) and converts some of the starch maltose (a disaccharide.) It’s good to chew food so that the saliva can mix with the food and begin the digestive process. Amylase continues to break down starches until the food reaches the stomach where stomach acid neutralizes amylase. After food passes through the stomach and entering the small intestine, the pancreas is signaled to make pancreatic amylase. This amylase converts the remaining starch into maltose.
In your experiment, is the light corn syrup in the dialysis tubing hypertonic or hypotonic to the water? hypertpnicressure B. 0.302 grams of an antibiotic was dissolved in 500 mL of water at 23.6°C. The solution has an osmotic pressure of 8.34 mm Hg. What is the molar mass of the antibiotic?
Radu Purtuc | Chemistry 231 - Lab | Section 32 Ronnie :: team-member TECH 705, SEPARATING ACIDS AND NEUTRAL COMPOUNDS BY SOLVENT EXTRACTION - MACROSCALE EXTRACTION July 6, 2006 Lab Report INTRODUCTION Purpose: using extraction technique to separate acetanilide, p-toluic acid, and p-tert-butylphenol; then measure the melting points of each compound and comparing them to the statistical values. Background: separating acids and neutral compounds by solvent extraction is a useful technique used in practice by chemists to separate organic compounds from mixture of other compounds. It generally involve several steps, with limiting factors being the number and output purity of compounds to be extracted from source mixture. A number of specific compound solvents not inter-miscible are used to separate and dissolve compounds, and a physical transfer between solvents is employed. An example of use is cleaning compounds of impurities, where different solvents work as a molecular filter that interacts differentially with compound and impurities respectively.
According to the Bronsted- Lowry Model, aids donate an H+ ion to another substance, while bases can accept an H+ ion. On the other hand, the Arrehenius Model states that acids produce H+ ions and bases produce OH ions when submerged in water. The hypotheses made states that all of the household substances are acidic for the following reasons: vinegar, due to its common use as a cleaning agent, to break down grime, as well as detergent, for its use in removing stains from clothing. Soda was determined to be acidic, because it destroys the enamel on teeth, along with ammonia, a powerful cleaning agent known for breaking down dirt. Drain cleaner unclogs drains by breaking down the substances caught in the drain due to its acidic quality.