PH indicator

Craig Mathews, and Ross Mather. T.A. Maia Popova, Professor Yasmin Jessa. 144 Section C. October 15, 2014. Abstract: While the goal of this lab was mainly to be able to perform an acid-base titration. Complete a traditional titration and then and a pH electrode titration. Calculate the molarity of citric acid from the titration volume of NaOH. Calculations should be fairly close in average and the ending point should coincide with the equivalence point. All while effectively being able to compare

Discussion: The purpose of this lab was to calculate the amount of calcium in Kirkland Signature’s Calcium 600mg +D3 through the processes of vacuum filtration and acid-base titration. These two methods were effective in determining the amount of calcium in the calcium supplement with an error of +/- 0.05 g; the amount of calcium stated on the label was 600 mg. The reactions that occurred during the process of vacuum filtration were: CaCO3 (s) + 2HCl(aq) → CaCl2 (aq) +CO2 (g) + H2O(l) CaCl2(aq)

appropriate indicator is vital in performing a successful titration reaction because the end point and equivalence point must be as close as possible. The indicator phenolphthalein was chosen for both parts B and C as in both titrations it was a weak-acid and strong base titration. Oxalic acid and acetic acid are both weak acids, whereas NaOH is a strong base. At equivalence points, the resulting solutions contain CCOONa and only. Therefore, salt hydrolysis occurs in part B and the PH at equivalence

stomach. Original Procedure Test the pH of the vinegar and each antacid. Place 5 drops of each antacid on the wax paper and mix in 5 drops of vinegar in each. Test the pH of the mixture. When we got the same results for all three mixtures (pH: 4), we decided to modify our procedure. Modified Procedure Instead of mixing a few drops of each substance, we decided to mix 5 mL of the antacid with 5 mL of the vinegar. Data (Original Experiment) Vinegar pH: 2 Gaviscon Extra Strength Mylanta Maximum

Experiment 11B consisted of synthesizing methyl orange, a synthetic dye, and testing this dye’s coloring quality and effectiveness as a pH indicator. Methyl orange is an acid-base indicator. In a pH of greater than 4.4, it becomes a yellow solution with a negatively charged sulfonate ion. When submerged into a solution with a pH less than 3.2, the dipolar red ion (helianthin) predominates. Methyl orange is a type of azo dye, which is commonly found in food, fabric, paint, and other brightly colored

titration procedure involved the addition of NaOH to another solution: KHP (primary standard) in Part A and HCl in Part B. This process involved the addition of a strong base to a strong acid, so the titration curve started at a low pH (acidic) and ended at a high pH (basic). The titration of a primary standard, KHP, was used to help determine the unknown concentration

specifically, titration is often used in the making of medicine and different types of drugs for medical use2. The titrant, or known solution, is usually added to a known quantity of the unknown solution, the analyte, until the reaction is complete5. An indicator is used to demonstrate when the reaction is finished, the endpoint. The neutralization reaction for when a strong acid, HCl, is titrated with NaOH is1:

chemically equal amounts of the acid and base have been mixed and neutralized each other. Neutralization between a strong acid and base such as HCl and NaOH will result in a solution with a pH of 7.0. If the final solution does not have a pH of 7.0 errors that might have occurred include misjudging of color indicator, using a contaminated

titration. In a clean 25 mL volumetric flask, measure out 0.0020 mole of acetic acid. Make sure to use all the digits on the balance. Add water to line indicated on the flask. In 125-mL Erlenmeyer flask, add the mixture and 3 drops of phenolphthalein indicator solution. Use sodium hydroxide to titrate the solution until the color turns pink. Wait for at least 30 seconds to see if the pink color continues. Record the volume of 0.1 M NaOH solution used. In 125-mL Erlenmeyer flask, rinse very well with

determine the pKa of a common acid-base indicator and color dye, bromothymol blue. Acid-base indicators are usually weak acid or base that change color with various pH levels in a solution, giving one specific color for acidic solutions (HIn) and another color for basic solutions (In^-). In the case of bromothymol blue, a weak acid, the reagent turns yellow in the presence of an acidic solution and turns blue in the presence of a basic solution. As the pH of the solution containing bromothymol blue