Burette

Determination of Relative Atomic Mass of Lithium Evaluation: In general the accuracy of the experiments was good. However with practice, the accuracy could be improved; accuracy being how close the results are to the real answer. I think I have carried pit the experiment as well as I possibly could at the time with the given conditions and time period allowed. I have gained precise results from the practical. However, looking back at the analysis section, the

Mg2+ Determination using EDTA Linh Nguyen Chem 1212L – 165 Feb 08 , 2014 Purpose and Procedure: The purpose of this experiment is using Compleximetric titration and EDTA to determine the concentration of Mg2+ in solution; and also calculating the percent by mass of MgO in the unknown sample. This procedure results no significant deviations. The procedure for the experiment is from the lab manual referenced below Laboratory Experiments for Chem 1211L & 1212L (6e)

• Determine the total alkalinity of (=[HCO-3 +2[CO2-3]) by preforming a titration with the use of HCl. • Determine the Bicarbonate content (HCO-3 + OH- → CO2-3 + H2O) by preforming a titration with the use of NaOH to convert HCO3- to CO2-3. • Calculate the composition of carbonate and bicarbonate in the solution. Introduction Acid-base titrations are common laboratory practices that are used to determine the concentration of either an acid or a base, by neutralizing the substance with a known concentration

washed by water. Burette was rinsed by sodium hydroxide solution and pipette was cleaned by hydrochloric acid solution. Retort stand was set up and the white sheet of paper should be placed under the burette where the beaker was put on to easily realize the colour changes. 3. Two beakers were labeled as acid and base for each one of them. Then they were brought to the teacher and filled it up by sodium hydroxide and hydrochloric acid. The funnel was put on the top of the burette then the sodium hydroxide

gathered, about 55.0 mL was measured and placed into the burette. All of the solution did not fit into the burette. The burette was filled until the iodine solution was at the 0.0 mL mark. A table chart was created to record all the data collected during the experiment. The first data table was labeled standardized data. Only one column was needed. It was labeled run one. The rows on the table were labeled final burette volume, initial burette volume, mL of iodine solution, mg of ascorbic acid in

on this error in relation to the apparatus error of the method. In the titration, I used these available instruments to ensure my results would be as accurate as possible. Volumetric burette: This instrument was filled with the sodium hydroxide solution that would be gradually added to the vinegar solution. The burette was used instead of a measuring cylinder as it gives a finer volume

equivalence point between the acid and base where they neutralize each other. The materials used in this procedure were HCL solution, water, ring stand, burette, burette clamp, unknown concentration of NaOH, phenolphthalein, erlenmeyer flask, and graduated cylinder. To start the procedure, obtain a burette, and rinse the burette with water and check if the burette is able to release the solution. Next the ring stand must

enable me to see the colours much easier than on a tile of another colour such as red or black. Measuring cylinder This will enable me to measure out 25mlᵌ of alkali into the conical flask. Funnel A funnel will allow me to pour the acid into the burette without it spilling which will limit safety hazards. Hydrochloric acid 0.2, 0.4, 0.6, 0.8, 1.0 molar 50cmᵌ for each test. This is the acid that we are allowed to use and the highest concentration we can have is 1 molar to limit risks. Furthermore

First, wash the burette with soap using a burette brush. Rinses well with tap water and then several times with distilled water. Next, fill the burette with the desired solution above the zero mark and then drain the solution out the tip so that the level of the solution is just below the zero mark. Before beginning the titration record the initial reading on the burette. Put the tip of the burette into the titration flask, but do not let the tip touch the

HNC Applied Sciences Zakiah Ali Aim The aim of this experiment was to measure how much sodium hydroxide was used to turn the diluted vinegar pink. Materials 2 Pipettes (25cm3) Burette Volumetric flask 2 beakers Clamp stand Clip White title Funnel Conical flask Pipette filler Vinegar Deionised water 0.1mol/l sodium hydroxide 3 drops of phenolpththalein indicator Summary A standardized vinegar solution was prepared, to test how much sodium hydroxide is needed to turn the solution