Acid dissociation constant

Effect of Bunker Fuel Use over Extended Periods of Time Introduction The South Australian Government is considering the regulation of Bunker Fuel in Port Adelaide, but it is facing a lot of pressure from shipping companies not to do so. In the future the SA Government plans on getting more cruise ships to come to Adelaide. The Government want to know how the increased uses of Bunker Fuel in Port Adelaide will affect the climate, and nearby residents. This report, will be looking at how the use

In the following experiment, fluorescence methods and techniques will be used to determine the detection limit and the concentration of quinine in tonic water. As shown in the graph of the quinine standard samples, the concentration was on average was 350 ppm. This concentration is incorrect, since it did not factor in the max emission and the emission at smaller concentrations. Despite the error in the calibration data, the pH data was able to be observed and assesse the relationship of pH to emission

Abstract Spectrophotometry is the process by which the light energy absorbed by colored compounds, is determined and used for quantitative and qualitative analyses. We use this process to often produce a standard curve, and use that to compare absorbance with different factors. In Experiment 3.1-3.4, spectrophotometry is used to produce the absorbance spectrums for the basic and acidic forms of PNP, to determine the pKa of PNP, and to develop standard curves for determination of unknown concentration

The purpose of this lab was to construct a titration curve by titrating Formic acid using a standardized sodium hydroxide (NaOH) and a pH meter through potentiometric titration. After the data for the rest of the class is collected, compare and contrast the equivalence points to see how the concentrations of the various acids affected the acids weakness and strength. Methods: Obtain 0.020 M of Formic Acid (HCCOOH). Calibrate the pH meter using the instructions for calibrating the pH meter

Objective: The objective of this experiment is to use acid-base extraction techniques to separate a mixture of organic compounds based on acidity and/or basicity. After the three compounds are separated we will recover them into their salt forms and then purify them by recrystallization and identify them by their melting points. Procedure: Extraction of Carboxylic Acid A pre-weighed (0.315g) mixture of Carboxylic acid, a phenol, and neutral substance was placed into a reaction tube (tube 1)

In some cases chemistry can pertain to acids and bases. These components are very useful when it comes to trying to figure out reac-tion stoichiometry, ionization constants, RICE tables, making buffer solutions, and stabilizing pH solutions. Acid equations include HA as the acid and H2O as the base. One example of an acid reacting with a base can be seen in Equation 1. Equation 1. HA(aq) + H2O(l)  H3O+(aq) + A-(aq) The Bronsted-Lowry theory connects acids as being a proton donor and bases as

M KCl solution containing 5 mM Fe(CN)63-/4-. Inset of Fig. 3B: Equivalent circuit applied to fit impedance measurements, where: Rs is the resistance of electrolyte solution; Rct is the charge transfer resistance, W is warburg impedance and CPE is constant phase element. 3.5. Electrocatalytic oxidation of nitrite on the modified electrode The electrocatalytic activity of the β-Ni(OH)2@CDs/GCE toward nitrite was studied by recording cyclic voltammograms from the range of potential 0.3 to 1.1 V in the

Objective The purpose of this lab was to perform acid base titrations using a pH electrode to monitor the equivalence point. Standardized NaOH was titrated with HCl and acetic acid using phenolphthalein as the indicator. Each titration was analyzed by the following plots to determine the equivalence point volume: pH vs volume, first and second derivative plot and Gran plot. Methods The pH meter and glass electrode were calibrated using buffers of pH 7 and 4. 25.00 mL of HCl solution was transferred

of a weak acid and its conjugate base required to prepare the buffer solutions of specific pH. Examine pH behavior of buffer solutions using previously studied methods of measuring pH. Reinforce the proper use of volumetric glassware in preparation of solutions of a required concentration. Practice with titration technique in the determination of a buffer capacity. Introduction: A buffer solution is one that is resistant to change in pH value when small amounts of a strong acid or base are

Introduction: Acid Rain, or more specifically, acid precipitation, is an environmental phenomena. It is composed of sulfuric acid and nitric acid, in addition to water, which come to be due to the interactions between the water and atmospheric pollutants, such as sulfur oxide and nitric oxide. This combination of strong acids in water is known to be detrimental to the environment, infrastructure, and the health of people. Due to the water cycle, other water bodies, such as lakes and streams, are