Titration Lab Report

In this test, primary halides precipitate the fastest while secondary halides need to be heated in order for a reaction to occur. Comparison of the rates of precipitation of the obtained product to standard 1° and 2° bromide solutions will show whether the product is a primary or secondary

In direct titrations, the number of moles of acid can be easily derived by simply manipulating with the values of acid and base given in the experiment. In back titration, excessive volumes of acid are always added. Of which, only a certain quantity would be neutralised. The number of moles of acid is eventually derived from titrating this excess acid with a strong base and using mole fractions to calculate. The quantity of acid neutralised is obtained by subtracting the moles of acid given at the start of the experiment, with the moles of acid titrated.

It was shown that the intramolecular conversion of the MOPh-CO2 complex was the most responsible for the products distribution of the Kolbe-Schmitt reaction. It was observed that the mechanism of the carboxylation reaction of lithium phenoxide was significantly different from those of other alkali metal phenoxides however, there was a resemblance between the mechanisms of the carboxylation reactions of lithium phenoxides and sodium

I can now calculate the density  (aka the concentration), of them before and after. Then I can take the change in density over the change in time to determine the rate of chemical reaction. This is because a chemical reaction will affect a solution’s concentration, and to determine the rate, I just need to factor time into the scenario. Furthermore, I can do this multiple times, all with different concentrations of HCl and different amounts of calcium carbonate (as it is diluted in water, and water has a different mass than the acid), to determine how the original concentration of HCl affects the rate.

Exercise 1 1. Suppose a household product label says it contains sodium hydrogen carbonate (sodium bicarbonate). Using your results from Data Table 1 as a guide, how would you test this material for the presence of sodium bicarbonate? B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript33 Words

A limiting reactant is the reactant that limits the amount of product that can be produced in a reaction. An excess reactant is the opposite, or the reactant that remains after a chemical reaction is performed and the limiting reactant runs out (Stoichiometry: Limiting). The stoichiometry calculations determining what should happen can be found in the calculations section. The solid should form calcium carbonate. The uses for calcium carbonate are as a filler and coating pigment in paper, plastics, paints, and coatings.

ABSTRACT The experiment aims to find the concentration of acetic acid in the vinegar sample by titrating it to a standardized NaOH solution, a base solution. A standardized 0.100 M NaOH solution was prepared from an available concentration of NaOH specifically a 1.00 M NaOH. The volume of the standardized solution (titrant) used which is 0.100 L was calculated using the M 1 V 1 = M 2 V 2 relationship.

All the mobile ions get attached to the opposite charge of the stationary phase resin molecules. This happens when the right buffer conditions are applied. When this kind of conditions are successful where ions are completely attached to the resin, then equilibrium is said to have reached. Sample Application –The sample is loaded inside the column using a syringe, typically. The neutral proteins or the one with similar charge as the resin will get eluted and the ones with the opposite charge get attached to the resin

Discussion: End point in this acid-base titration experiment refers to the point where the chemical reaction has reached its conclusion and no additional titrant should be added. The end point of this experiment can be obtained when the indicator used changes colour. For example colourless to light pink when phenolphthalein is used and red to orange and subsequently yellow when methyl orange is used. Equivalence point, also known as stoichiometric point in an acid-base titration refers to the point where the reacting acid and base is in equal proportions. In the graph plotted, pH against volume of NaOH, the graph becomes nearly vertical at the equivalence point.

Pre- lab preparation To perform this investigation, a number of the solutions were needed to be prepared in advance. The following is the preparation process - Preparing the stock solution-The stock solution of Salicylic acid needed to be prepared well in advance before the experiment began. To do so, 1.73g of Salicylic Acid was weighed using the weighing balance. After Salicylic acid was weighed, it was transferred to a standard flask of 100cm3 and, 100cm3 of pure Ethanol (C2H5OH), was poured into the standard flask that contained the Salicylic acid.

In this lab, three unknown compounds were separated from a mixture and identified by melting point. Unknown mixture #124 has components of acid, base and neutral compound. The compounds were identified by melting point and matched up with the known melting points from a given list. In order to identify the compound it was important to separate by dissolving the mixture in an organic solvent which was not soluble in water, and then extracting the solution first with HCl, and then dilute sodium hydroxide solution. From the separation mixture, the aqueous layer were obtained and labeled as TT-1 (base), TT-2(acid) and TT-3 (neutral) in three different test tubes for later recovery.

The second step is about finding the theoretical yield, which will help to determine the correct amount of Ca(OH)2 can be made in chemical reaction. However, before doing this, it’s necessary to find whether CaCl2 or NaOH is a limiting reagent. For each test, the limiting reagent is found by multiplying the number of moles of the reactant by 1 mole of Ca(OH)2 and dividing then by a number of moles of reactant from the reaction. The lowest answer in each test will be the limiting reagent. To find a theoretical yield, the limiting reagent was multiplied by the molar mass of Ca(OH)2 and

Purpose The purpose of this experiment was to evaluate the stoichiometric relationship between the testing agents and to identify the products formed. The relationship was found by completing three acid and base neutralization reactions using phosphoric acid, which is a triprotic acid, with different volumes of sodium hydroxide. Introduction Procedure Phosphoric acid solution with a volume of 1.00 mL and a molarity of 6.00 M was transferred into a 125-mL Erlenmeyer flask using a volumetric pipette.

The objective of the lab was to understand the Law of Conservation of Mass. The Law of Conservation of Mass states that matter can be changed from one form into another, mixtures can be separated or made, and pure substances can be decomposed, but the total amount of mass remains constant. For example, from our experiment in the lab, we observed mass of the mixture of aqueous Sodium Sulfide and aqueous Zinc chloride turned white color. After the filtration, and all the water was evaporated, we measured the mass very close to what we had started at the beginning. The error in mass occurred because of the remained residue (solute) in the beaker.

Introduction: The unknown acid molarity will be determining by titration method. Titration is a process depends on concentration of known solution to another solution until the solute in the another solution completely react. Standard solution is the solution of known concentration that used in titration. In this experiment, NaOH was the titrant (base) however, the two analyte which used were HCl and H2SO4.