We resulted that lead, silver, and copper are the strongest oxidizing agents, and that magnesium and zinc are the weak oxidizing agents. The strong oxidizing agent oxidized the weak oxidizing agent and in turn the strong oxidizing agent got reduced while oxidizing the weak agent. When a reaction occurred, the solid metal reduced the ion, and in turn made it the more reactive metal. In part two we used a solvent extraction technique to derive an activity series for the halogens. With the use of this technique we placed chlorine, bromine, and iodine into solutions containing chloride, bromide, and iodide.
Abstract The interaction at equilibrium between acids and bases during a titration can be used to determine several characteristics of the acid or the base. In this experiment 0.05 M of KHP titrate with the strong base NaOH. From the plot of pH versus the volume of sodium hydroxide added was found that acid ionization constant Ka for KHP at half point was equal to 8.3176x10-6, also the dissociation constant Kb for conjugate base of weak acid was equal to 1x10-9. This value was established by observing the pH versus volume of NaOH graph. The equivalence point of titration occurred at a volume of 31 mL 0.081M NaOH (aq).
If the reaction is first order, its graphical representation is seen as ln[A] (natural log of concentration) vs. time, and the slope of its like is also the negative rate constant. Finally, for a second order reaction the graph is shown as 1/[A] (inverse of concentration) vs. time, and the slope of its given line is the positive rate constant. By understanding the rate law and finding the value of the correct rate constant with respect to the order of the reaction, one can determine the half-life of the crystal violet. This is because the crystal violet undergoes a decay reaction with the sodium hydroxide. According to Beer's Law, the absorbance of crystal violet is proportional to its concentration.
This is used when a weak acid is being used in the reaction as it acid does not fully dissociated and there is an A- value. This is the equation used for reaction (ii) as it used ClCHCOOH as the acid. Results, Observations and Discussion: (ii) 0.25M HCl | (iii) 0.5M Cl2CHCOOH | (iv) 0.125M HCl | Time(mins) | Vol (Na2S2O3) | Time(mins) | Vol(Na2S2O3) | Time(min) | Vol (Na2S2O3) | 0 | 0.46 | 0 | 0.4 | 0 | 0.33 | 6 | 0.44 | 8 | 0.4 | 6 | 0.28 | 12 | 0.4 | 16 | 0.36 | 12 | 0.24 | 18 | 0.36 | 24 | 0.29 | 18 | 0.22 | 24 | 0.32 | 32 | 0.26 | 24 | 0.2 | 30 | 0.28 | 40 | 0.2 | 30 | 0.19 | Calculations: Finding Kobs - (ii) -dI2dt=0.005
This particular reaction is a strong acid and a strong base which means that when the reaction reaches the equivalence point, the moles of the acid and the base are equal and the solution is neutral so the pH should be around 7.0 depending on the final volume of each solution. To get this data, we will titrate an HCl solution with NaOH solution of which is a known concentration. We will record the initial and final reading of the NaOH while we record the pH of the titrated solution in the beaker. We will repeat this process with a solution of acetic acid which is a weak acid with NaOH and record the initial and final reading of NaOH and the pH of the solution in the beaker. Procedure Preview Calibrate the pH meter.
What is the identity of your unknown? Justify your conclusion by comparing the observed molecular weight and pKa values to those for all amino acids that might have been your unknown. B) Examining the effect of ionic strength on the pKa of a weak acid. Restandardize the pH meter with both pH 4 and pH 7 buffers. Why is this necessary?
ABSTRACT Isopropyltoluene isomers were synthesized through the friedel-crafts alkylation of toluene with 2-chloropropane in the presence of aluminum chloride as a catalyst. Through extraction of the distillate with water and 5% NaHCO3, followed by a fractional vacuum distillation, the desired aromatic organic compound was isolated. Infrared Spectroscopy and Gas Chromatography were used to analyze the composition, purity and to confirm the identity of the prepared product. The sample weighed approximately 2.66g, which reflected a low yield at 47%. However, from the GC the area % (also known as percent purity) was 91.8%, which indicates that a very pure product was obtained.
The result proved: Contract to the hypothesis, at pH 12, activity of enzyme Catecholase and the rate of reaction decreased. Introduction pH is a measure of the concentration of hydrogen H+ in solution so the higher concentration hydrogen ion, the lower pH. pH is one of the most important factors affect to human body. pH was divided three parts on pH scale from pH 0 to pH 14: at pH 7, solutions are neutral. pH > 7 is alkalinity environment that will bind hydrogen ion, and pH < 7 is acidic environment that will donate hydrogen ion.
Bromination of Arenes This lab demonstrated the application of adding bromine to various arenes, hydrocarbons with alternating single bonds. This process, bromination, is a mechanism which treats hydrogen as a functional group. This being the case, the rate of reaction of certain arenes can be measured and compared to that of other arenes upon the addition of the bromine. The reaction occurs when the bromine radical generates from the halide diatomic molecule, using light energy. The fact that the energy needed to break the necessary bonds falls within the visible light spectrum is the basis on which the experiment is based.
This table shows the data collected while standardizing NaOH. With finding the volume used/ final volume. Trials | Mass of KHPthl (g) | Initial volume (mL) | Final volume(mL) | Volume used(mL) | 1 | 1.02 | 0.00 | 36.10 | 36.10 | 2 | 1.01 | 0.00 | 38.5 | 38.5 | 3 | 1.00 | 0.00 | 39.1 | 39.1 | Potassium hydrogen phthalate is used for standardizing NaOH because it is slightly acidic, which is often used with NaOH and is used as a buffering