Acid-Base Titration Lab Report

My results yielded a high Average Molarity .270M . The ideal would be around 1.000M . Deviation was ± 1.20

We know that that the end point of the titration is reached when, after drop after careful drop of NaOH, the solution in the flask retains its pale pink color while swirling for about 30

4. To utilize the titration results to calculate the molarity of the hydrochloric acid and the

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

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

Then MnO4- was added drop wise until the pink color persisted for 15 seconds to signal the equivalence point had officially been reached. The reason why the pink color signaled the equivalence point is because MnO4- was an indictor for the titration. After the titration was finished the final volume of the buret was recorded, which came out to be 21.45 mL. All the previous steps were then done a second time. The data that was yielded from this second trial was .406 grams for the mass of ferrous ammonium sulfate, 9.21 mL for the initial volume, and 23.60 mL for the final volume.

Using Graph 1: The Volume of Titrant Added in order to reach the Endpoint and the Corresponding pH Values, observe the vertical line of each titration and see the points in which the horizontal lines intersect it. These points give the

The third part of the lab consisted of understanding the acid-base titration of the KTOF that would help understand how much pH is within the solid. When using the ion exchange column, it is important to know if the column is acidic or not when it is calculated through the Logger pro. The pH experiment uses an ion exchange column to change a solution into an eluent solution to change a compound of the KTOF. First, 0.0466g and 0.0507g of KTOF was weighed on an analytical balance. After the KTOF was weighed, the ion exchange column was rinsed with 10 mL of distilled water to determine the pH of the column.

Titration can be used to standardize a solution. In this experiment, sodium hydroxide was used to titrate KHP solution. Using the results of the titration, the exact concentration of NaOH was calculated to three significant figures. As see in data table A.1, the volume of NaOH used in trial one is 25.95 mL, and moles of KHP is 0.003501 mol. Using this information, the molarity of NaOH was found by using the formula, Mass of sample x (1 mole/ atomic mass), in Table A.2.

In this experiment, a redox reaction occurred. An oxidation-reduction reaction (redox) is a type of chemical reaction that involves a transfer of electrons between two solutions. The chemical being oxidized is losing electrons and the chemical being reduced is gaining electrons. In this case KMnO4 is losing electrons and Oxalic Acid is gaining electrons. KMnO4 can titrate a or reduce Oxalic acid. Titration is the technique used to find the unknown concentration of one solution based on the concentration of a known solution. In equation 2, the molar relationship between the 2 is shown, it is 2 KMnO4 to 5 Oxalic Acid. The molar ratio relationship is useful because it shows how much of a certain product is needed to help a reaction occur and which chemical is limiting reagent. The experiment was started by preparing a titrating strength KMnO4 solution from stock to a less concentrated KMnO4. Equation one shows how this was done. The KMnO4 needed to be diluted, if it had not been diluted, then it would be way too hard to get an accurate reading of the Oxalic Acid used. Without being diluted the Oxalic Acid would be strong. The next step was to standardize the KMnO4 solution. It was calculated that 37.5 mL of Oxalic Acid could titrate 15 mL of KMnO4. To determine the exact molarity of a solution a standardization needs to happen. In this experiment the standardization found how much Oxalic acid was needed. Through the controlled variable, the fact that 37.5 Oxalic acid could be titrated by 15 mL of KMnO4, the percent of the

Collect to 2 large beakers both large beakers are to be filled with hot water (labtutor). Then obtain seven conical tubes these will be used to collect the levels of gas, you will also need test tube a stopper and a plastic tube (labtutor). You want to fill the conical tube to at least 50 ml of water (Cressy). Take the four conical tubes filled with water and place two in each beaker, to do this you must invert the tube and cover the release hole as to not lose any water (Cressy). Then place the beakers with the tubes in the bath so they can be at the same temperature as the bath (Cressy). Next mark all of your test tubes in number order to be sure which tube contains what concentrations and pH (Cressy). Having mixed a solution to the specifications of 2.5 ml of glucose in all tubes, 3 ml of yeast in 2 tubes of pH 5, 2 tubes of pH 9, and the single pH 7 tube, the remaining two tubes will contain no yeast as they will be negative controls. Next add 2 ml of pH buffer 3 tubes will receive pH of 5, three will receive a pH of 9 and a single tube of pH 7. Finally add pure water to make sure all test tubes have 10 ml of solution. When making the solutions

Before the commencement of the practical, all necessary glassware and measurement tools were rinsed appropriately. The pipette was rinsed three times with vinegar solution, whereas the volumetric flask was rinsed three times with distilled water. 20mL of the vinegar solution was measured and transferred to the volumetric flask, where it was diluted with distilled water by filling the flask to the 200mL graduation line. A 20ml aliquot of the aforementioned solution was extracted from the volumetric flask via the volumetric pipette and subsequently transferred to the conical flask. Three drops of phenolphthalein indicator were then added. The burette was filled with the provided NaOH solution of 0.1M, with volume measurements taken from the bottom of the meniscus. The conical flask was placed under the burette, from which a rough titration of the vinegar solution began. Titrations halted once a permanent color change was visible in the conical flask. This process was repeated until three concordant titre values were obtained.

The purpose of this lab was to use process titration to find concentration of an aqueous solution of Hcl(aq) , using KOH(aq) as the titrant.

e. Just prior to titrating the flask, add four drops of Eriochrome Black T indicator solution. Continue stirring for another 30