ABSTRACT
The experiment aims to find the concentration of acetic acid in the vinegar sample by titrating it to a standardized NaOH solution, a base solution. A standardized 0.100 M NaOH solution was prepared from an available concentration of NaOH specifically a 1.00 M NaOH. The volume of the standardized solution (titrant) used which is 0.100 L was calculated using the M 1 V 1 = M 2 V 2 relationship. It was then gradually added to the vinegar solution until the acid-base reaction was completely neutralized. To regulate the reaction, phenolphthalein, an acid-base indicator, was added beforehand to the vinegar (analyte). The indicator will change its color, signaling that the end point is obtained and the volume of NaOH used can now be
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Titration is an analytical method used in the laboratory to determine the concentration of an unknown solution using a solution of accurately known concentration referred as the standard solution. Since the volumes of both solutions and the concentration of the standard solution are clearly identified, it is possible to calculate the concentration of unknown solution. The standard solution is gradually added to the unknown solution until the equivalence point, a point at which the moles of an acid is equivalent to the moles of the base, is attained. (Chang, …show more content…
The process reaches an endpoint when the two solutions completely and exactly neutralized each other. However, in determining the neutralization time by speculating the change in color, one must be critical and careful enough to get accurate and precise data. In conducting this experiment, some possible errors affect the accuracy of the data. The first possible source of error encountered is in the miscalculation in preparing the titrant. Excess or lesser amounts of 1.00 M NaOH can lead to inappropriate standardization. Consequently, an incorrect standard solution prepared yielded to the wrong number of moles of NaOH which consequently give us wrong data. Another issue arose with the amount of the indicator used. Since drops are the measurement associated with the amount of phenolphthalein, it is quite difficult to obtain an accurate amount. A slight error in the indicator can shift the endpoint and consequently affects the volume of the obtained NaOH. Lastly, the final source of error of this experiment is misjudging the color of the indicator near the endpoint. The color change is very intricate that even a small amount of the standard solution can produce different shades of the color. With these uncertainties, a 23.3 % error was committed given that the theoretical molar concentration of acetic acid in the the vinegar sample is
The average HCl concentration of the three trails is = 0.098 M 2. Question 2: Experiment 2: The acidity and vinegar, the type of vinegar we used was Kroger distilled white vinegar, and the acidity of the vinegar was 5% Trails Dilution of original vinegar solution. Volume of
In the first part of the experiment, Part A, the standard solutions were prepared. As a whole, the experiment was conducted by four people, however, for Part A, the group was split in two to prepare the two different solutions. Calibrations curves were created for the standard solutions of both Red 40 and Blue 1. Each solution was treated with a serial 2-fold dilution to gain different concentrations of each solution.
After obtaining an homogeneous mixture, the flask was placed in an ice bath during five minutes next to a graduated cylinder containing 5.0 mL of concentrated sulfuric acid. The temperature of the ice bath was recorded to be 1.1 °C. Likewise, a second graduated cylinder containing 1.8 mL of nitric acid and 2.5 mL of sulfuric acid was immersed in the cold ice bath to keep the three different solutions at the same temperature. Thereafter, the cold 5.0 mL of H2SO4 were added to the erlenmeyer flask containing the acetanilide solution, which remained in the cold water for approximately another 4 minutes.
Glacial acetic acid and acetic anhydride were added to the mixture while refluxing, which converted the lime colored solution into a clear mixture. The flask was cooled in an ice bath and the solution
3. Upon adding 20 drops of NaOH, a white precipitate was formed signifying acidic impurity. In the second NaOH mixture, about 20 drops were administered and no precipitate formed indicating that the ample is more pure than before. Data: Weight of flask = 75.10 grams Weight of the flask with solids =
Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.
Conclusion: Based on the results of molarity from Trials 1, 2, and 3, it is concluded that our experimental for each trial is .410M NaOH, .410M NaOH, and .450M NaOH. The actual molarity of the NaOH concentration used was found to be 1.5M NaOH. The percent error of the results resulted in 72%. The large error may have occurred due to over titration of the NaOH, as the color of the solution in the flask was a darker pink in comparison for the needed faint pink. Discussion of Theory:
Commercial vinegar, Yamaha brand 0.1 mol/dm3, NaOH soloution Phenolpthalein indicator soloution (50.00 ± 0.5 cm3 ) cm3 burrete (250.00 ± 0.5 cm3) volumetric flask a (250 cm3± 0.5 cm3)
Its pH is greater than 7 and turns red litmus paper into blue. Acid- base neutralization is done by adding an acid to a base or a base to an acid until the substance has equal hydrogen and hydroxide ions. This is used to determine unknown concentration of a
Practical I: Acid-base equilibrium & pH of solutions Aims/Objectives: 1. To determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3.
Introduction Buffer is a solution that resists a change in pH when bases or acid are added. Solutions that are acidic contain high concentrations of hydrogen ions (H+) and have pH values less than seven. Buffer usually consist of a weak acid, and its conjugate base or a weak base and its conjugate acid. The function of buffer is to resist the changes in hydrogen ion concentration as a result of internal and environmental factor. This buffer experiment is important so that we relies the important of buffer in our life.
Materials Required: 1. Pellets of Sodium Hydroxide (NaOH) 2. Phenolphthalein solution (1%) 3. Potassium acid phthalate (KHC8H4O4) 4. Graduated cylinder - 10 mL 5.
The average result obtained was 22.5% and is close to it’s literal value. This experiment had also proven to have shown effective transfer of solids and liquids as values of 1st and 2nd results, namely 22% and 23% respectively, were similar thereby showing consistency in results. Phenolphthalein indicator was proven to be more suitable as an indicator as compared to Methyl Orange in this experiment. This is because Phenolphthalein the pH values of HCl involved in this experiment were in range of the pH values that bring about colour change in the Phenolphthalein indicators. (Approximate pH ranges for color change: 8.0-9.8) Low pH values are preferred for Methyl Orange.
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.
That caused a new initial reading of NaOH on the burette (see Table1 & 2). The drops were caused because the burette was not tightened enough at the bottom to avoid it from being hard to release the basic solution for titrating the acid. The volume of the acid used for each titration was 25ml. The volume of the solution was then calculated by subtracting the initial volume from the final volume. We then calculated the average volume at each temperature.