Avogadro constant

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

The purpose of this lab is to explore the effects of enzyme concentration, substrate concentration, temperature, and inhibitors on reaction rate, respectively. To test each of these factors, four activities were completed. The enzyme from Turnip Extract and the substrate Peroxide were tested. The turnip extract was tested at the following concentrations: .5ml, 1.0ml, and 2.0ml. Peroxide was tested at the following concentrations: 0.1ml, 0.2ml, and 0.4ml. In order to understand the effect of temperature

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

Objectives: To employ the Henderson-Hasselbalch equation for calculations of amounts 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

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

have a low Ka value, the Ka value is the tendency of the acid to dissociate: Ka= [H+] [A-] [HA] Ka is the acid dissociation constant and [HA] is the concentration of the weak acid . Strong acids usually completely dissociate and has a Ka value greater than 1. Weak acids don’t dissociate completely and have a Ka value much smaller than 1. pKa values are often used for weak acids

The combination of a carbonyl (C=O) group and hydroxyl (−OH) group on the same carbon atom results in the formation of a carboxyl (−COOH) functional group. Compounds containing at least one carboxyl functional group are commonly known as carboxylic acids, and have the general molecular formula CnH2n+1COOH. Carboxylic acids with two or more carboxyl groups are called dicarboxylic acids, tricarboxylic acids, etc. The carboxyl group is one of the most frequently occurring functional groups in chemistry

We then tested our predictions by performing TLC plate where three known amino acids were spotted against the three unknown buffers at the individual fraction numbers to produce a constant solvent migration distance of 3.06. Fraction number 5 migrated at the distance of 2.25 to produce Rf of .74 this closely resembles the Rf of Aspartic acid of .82. Fraction number of 9 migrated at the distance of ¬¬3.00 to produce Rf of ¬¬.98 this

First, we started testing solutions such as Water, Sodium Phosphate (Buffer), and Sodium Chloride. The two control solutions that were used in experiment were HCl which is an acid and NaOH which is a base. The purpose of the two controls is to test and determine if NaCl is a buffer or not. When HCl was added to NaCl the pH decreased from 7.60 to 2.53 pH. The comparison of the pH change of NaCl and Na3PO4, shows that when adding acid to Na3PO4, pH did not change dramatically as it did with NaCl, only

Extraction Aleigha Spaulding Joseph Osazee 10-6-15 Abstract: This report presents the percentage recoveries found when using the solid-liquid and liquid-liquid extraction techniques to extract a strong acid, weak acid, base, and neutral compound from a mixture. During the solid-liquid section of the experiment, 0.5 M NaHCO , 0.5 M NaOH, 0.5 M HCl, and distilled water are used to dissolve and separate the acid, phenol, and amine solutions from the mixture, leaving the neutral compound