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Acid Base Titration Lab Report

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Introduction:
The acid-base titration experiment is the use of a titrant, an analyte, and an indicator. Titration is the slow addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization, which is often indicated by a color change.1 The titrate is what is later released into a beaker or flask that is filled with the analyte and indicator. The color change happens because of the indicator. The correct shade of light pink will show when it has reached the equivalence point. Common places that use this experiment are pharmacies and doctor offices. Pharmacists use titration to achieve a desired mix of compound drugs.2 Doctors will …show more content…

If anything is added out of order, then the experiment will not react as needed. The experiment was held in two parts. The titrant was prepared first because it was what was going to be used in mass amounts for both parts. The preparation of the analyte and indicator needed to be done precisely. If anything was added out of order the color change would not happen. The titrant used was NaOH. The indicator for both parts of the experiment was phenolphthalein. Phenolphthalein is an indicator that changes color depending on the pH of the solution it is in.3 Specifically, phenolphthalein is colorless when the pH of a solution is acidic or neutral, but when the solution becomes slightly basic, phenolphthalein turns slightly pinkish, and then darker pink as the solution becomes more basic.3 This allows for a clear understanding of when the reaction has been …show more content…

All steps were followed as told till step 17 was reached.4 In step 17 to make sure the titration would be perfect the NaOH was released 10mL less than the pilot run then the rest was dispensed by drops. This insured the titrations would be a pale pink color rather than the bright pink color. To find the moles of KHP the mass was divided by the molar mass. The moles of KHP was then multiplied by the mole to mole ratio to get the moles of NaOH. The moles of NaOH was then divided by the liters of NaOH used to find the molarity, which was added to trial 2 then divided by 2 to find the average

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Standard Sodium hydroxide solution is the alkaline solution that will be used to titrate with soda water as it is a common solution that can be easily found in an ordinary school laboratory. It is a strong base. Carbonic acid is a weak acid which will react with a strong base to form a basic (pH > 7) solution. When Phenolphthalein is added to Soda water, the resultant solution is colourless. After titration with a strong base (sodium hydroxide), the solution will turn to pink as the solution becomes

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The mass of vinegar used during the experiment was 4.108 grams. It was determined that there were .003129 moles of CH3COOH in the vinegar sample. Using this information and the molar mass of CH3COOH, which was 60.05 g/mol, the mass of acetic acid in the vinegar was calculated: 4.Vinegar is a 5% aqueous solution of acetic acid. Since the mass of acetic acid within the vinegar was calculated as .18789 g in step 3, the percent of CH3COOH was calculated using the following equation: To calculate the percent error, the experimental value of 4.5% acetic acid in vinegar was subtracted by the theoretical value of 5% and divided by 5% to yield a percent error of 8.54%. The following is a copy of the calculations done using decimals: 5.The equivalence point of the titration curve measured in step 1 was 25.25 mL of NaOH.

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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.

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