Thiosulphate Of Acetic Acid H2so4 And Standardizing Naoh Using Titration Technique Essay

1. To titrate a hydrochloric acid solution of “unknown” concentration with standardized 0.5M sodium hydroxide.

The results showed the molarity of the NaOH solution. This experiment was completed twice and a new average molarity

8. Repeat step 7 with H2SO4, except that you should use a 10 mL graduated cylinder of H2SO4 and adding 15 mL water.

The purpose of this experiment was to determine the pKa, Ka, and molar mass of an unknown acid (#14). The pKa was found to be 3.88, the Ka was found to be 1.318 x 10 -4, and the molar mass was found to be 171.9 g/mol.

Approximately 3.4 grams of K2HPO4 was weighed on a triple beam balance and dissolved in 100.00 mL of DI water by diluting to the mark in a volumetric flask. Similarly, 2.4 grams of NaHPO4 was weighed on triple beam balance and dissolved in 100.00 mL of DI water by diluting to the mark in a volumetric flask.

During a titration the pH of the solution will be monitored using a pH meter from that we get a titration curve. The titration curve is then used to determine the equivalent molecular weight and Ka value of the unknown weak acid, from that we are

One milliliter of 6.00-M phosphoric acid was placed into a 125-mL Erlenmeyer flask using a volumetric pipette. Using a slightly larger pipette, six milliliters of 3.00-M sodium hydroxide was transferred into a 50-mL beaker. Then a disposable pipette was used to slowly mix the sodium hydroxide into the phosphoric acid while the solution was swirled around. Then both the beaker and flask were rinsed with 2-mL of deionized water and set aside. A clean and dry evaporating dish was weighed with watch glass on a scale. Then the solution was poured into the dish and the watch glass was placed on top. The solution was then heated with a Bunsen burner to allow for the water to boil off to reveal a dry white solid. After the dish cooled to room temperature it was once again weighed and the new mass was recorded.

Simultaneously, 0.5 mL of methyl benzoate was filled in an Erlenmeyer flask and this flask was put in another ice bath. 1 mL of H2SO4 was put drop by drop into the flask using glass pipettes. Then, the H2SO4 acid was transferred to the HNO3 acid drop by drop, because the stronger acid should be poured to the weaker acid. This was done while keeping the test tubes in the ice bath for 10 mins as the ice bath prevents over heating because the reaction between the acids is extremely exothermic.

The purpose of this two-part experiment was to “determine the mass percent of sodium hypochlorite in a commercial chlorine bleach sample” (lab website). Titration is used in this lab twice. In Part one, students will use the solution of KIO3 primary standard and use this solution to standardize a solution containing sodium thiosulfate. When the KI is added to the solution, it forms a brown/yellow color. Then students used titration to add Na2SO3 to make the color go from brown/yellow to colorless. In the second part of the lab, students used the standardized Na2SO3 solution to determine the mass percent of sodium hypochlorite in the commercial chlorine bleach. Students used titration to the standard solution of Na2SO3 to

Unlike other solutions that can be accurately weighted, NaOH tends to draw water from the air and become hydrated. This part of the experiment helped us calculate the exact concentration of NaOH via titration, and understand the importance of knowing that some compounds are easily affected when exposed to their surroundings. The endpoint was expected to take longer, a usage of approximately 10 mL to 15 mL, but the results showed otherwise. This proved the hypothesis wrong as well, titrating NaOH used less than or equal to 5.0 mL of NaOH. The calculations were revised multiple times by the mentors and by the professor, but no error was found.

The experimental value for the neutralization of NaOH and H2SO4 was closest to the theoretical value, in trial 3, with an percent error of 30.9%. All experimental values calculated were relatively high. This accounts for the heat loss through the coffee cup calorimeter, and the extrapolation of the data to find the maximum

An ice bath was prepared in a large beaker and a small cotton ball was obtained. 0.5 g of acetanilide, 0.9 g of NaBr, 3mL of ethanol and 2.5 mL acetic acid was measured and gathered into 50mL beakers. In a fume hood, the measured amounts of acetanilide, NaBr, ethanol and acetic acid were mixed in a 25mL Erlenmeyer flask with a stir bar. The flask was plugged with the cotton ball and placed in an ice bath on top of a stir plate. The stir feature was turned on a medium speed. 7mL of bleach was obtained and was slowly added to the stirring flask in the ice bath. Once all the bleach was added, stirring continued for another 2 minutes and then the flask was removed from the ice bath and left to warm up to room temperature. 0.8mL of saturated sodium thiosulfate solution and 0.5mL of NaOH solution were collected in small beakers. The two solutions were added to the flask at room temperature. The flask was gently stirred. Vacuum filtration was used to remove the crude product. The product was weighed and a melting point was taken. The crude product was placed into a clean 25mL Erlenmeyer flask. A large beaker with 50/50 ethanol/water

HCl is known as Hydrogen chloride in its gas state, but when in the presence of water, it is known as hydrochloric acid(PubChem). Hydrochloric acid is extremely corrosive and has uses in both laboratories and industrial settings(PubChem). This acid can cause short term complications such as irritation to the eyes and nose or it can leave long term effects like dermatitis and chronic bronchitis (PubChem). Sodium hydroxide is a base that neutralizes acids and when in liquid form it has a higher density than water (PubChem). The compound is used in various textile industries (PubChem). NaOH can be corrosive to metals and is toxic if ingested (PubChem).

Sodium hydrogen carbonate was added to the solution until it becomes neutral. Ph paper was used for this test to determine its ph value.

The method of titration was discovered in late 1800’s by a french pioneer name Francois Antoine Henri Descroizilles. Titration is a process used to find concentration of an unknown compound. This process is used in labs to find information need in everyday life.For instance, titration is used during blood test and urine test to determine the concentration