Abstract In this experiment, the reaction kinetics of the hydrolysis of t-butyl chloride, (CH3)3CCl, was studied. The experiment was to determine the rate constant of the reaction, as well as the effects of solvent composition on the rate of reaction. A 50/50 V/V isopropanol/water solvent mixture was prepared and 1cm3 of (CH3)3CCl was added. At specific instances, aliquots of the reaction mixture were withdrawn and quenched with acetone. In addition, phenolphthalein was added as an indicator.
Eventually using the NaOH and the acid’s consumed moles, the equivalent mass will be determined. Procedure: Part 2: Obtain 45mL of NaOH, and then weigh 0.3-0.4g of the unknown acid (KH2PO4). Dissolve the acid into 20.00mL water. Record the buret readings, and slowly titrate the NaOH into
In the next steps the density of water between 30-40 °C, 40-50 °C and 50-60 °C was measured. Then our results ρ vs T and also density vs temperature values given in the Steam Tables were plotted on the same graph in order to compare. In the second part the density of water was measured by density bottle. The densities obtained from the experiment are 995, 992.5, 991, 990 kg/m3 for the first part and
In this experiment I set up a lab that examined how 5 different concentrations of HCL (each concentration differing by 5ml of HCL) reacted with CaCO3 and performed three trials for each concentration of HCL, I then found then average of the results and used the averages to form an accurate graph comparing the rate of reaction for each concentration of HCL when mixed with CaCO3 chips. In this experiment I placed 5g of CaCO3 chips in a conical flask and then mixed the different concentrations of HCL with the calcium carbonate. As soon as all of the acid was poured in I attached a delivery tube to the conical flask and watched the CO2 form in upside down graduated cylinder (see diagram). The reaction observed
The most ideal in preparation of sodium alginate is by adding the powder to agitated water rather than vice verso to avoid formation of clumps. Alginic acid can be in two conditions which are water soluble or insoluble. That is relying upon the type of the related salt. The salts of sodium, other alkali metals and ammonia are soluble, though the salts of polyvalent cations such as calcium are water insoluble except for magnesium. The polymer of alginate itself is anionic which is negatively charged.
However, the reason that acetyl was not bound in the ortho position was because the para position demonstrated the least amount of steric hindrance. In other lab procedures, benzoic acid is sometimes substituted for anisole in the Friedel-Craft acylation. However, the reason benzoic acid
The solubility of CVD-ILs with CA and TA is less than CVD. This observation could be related with pH of final solution. pHs of final solution for CVD-ILs in HCl 0.2 M are 2.5-3 for IL-CA and IL-TA. According to the pKa of CA and TA (Table 1), they are partially in non-ionized form and synthesized ionic liquid cannot increase the CVD’s solubility against of the ionic liquid’s solubility in acetate buffer solution. Nevertheless a high concentration of chloride ion in solution because of fully ionization of counter-ions, the solubility improved in compared with CVD.
The most common are precipitation and complexation. In a precipitation reaction, an ion in solution reacts with an added reagent to form a solid. Whether a solid will form from a given reaction can be predicted by the solubility product constant (Ksp) of the solid under the given conditions. Solubility product constants are the equilibrium constants for the dissolution of an "insoluble" ionic solid in water. A low Ksp implies that the compound does not dissolve to an appreciable degree in water.
The product (Cu(OH)2) was unstable and could reform Cu2+ and OH- ions due to its high solubility. This result can cause difficulties on separating Cu from the other metals in the AMD. Therefore, additional treatment, such as sulfidization, is required to prevent the occurrence of the reformation process
After testing the burret reading, the next step was to start the experiment by preparing approximately 0.1 M NaOH solution. First calculate the amount of 6.0 M NaOH stock solution needed to prepare 500 mL of 0.1 M NaOH solution. A 10.00-mL graduated cylinder was used to measure the the calculated amount of 6.0 M NaOH, and then filled to the top with deionized water. The 10.00 mL was then poured into a 500 mL plastic bottle. The 10.00 mL graduated cylinder was refilled with deionized water and was poured into the same 500 mL plastic bottle.