Acid dissociation constant

determine the dissociation constant, Ka, of Acetic Acid. In order to do so, sodium hydroxide is titrated into a sample of acetic acid and the equivalence point is determined. Part two of the experiment consists of tested the dissociation constant. Acetic acid is mixed with sodium acetate. Part three of the experiment consists of adding acid or bases into the buffer solution and observing the changes that occur. The independent variable in this experiment is the titration of acetic acid being titrated

Determining the Equivalent Mass and Dissociation Constant of an Unknown Weak Acid by Titrimetry Ka Chun Wong, and James Ross, Ph.D. East Los Angeles, Chemistry Department, 1301 Avenida Cesar Chavez, Monterey Park, CA 91754 Abstract Chemistry 102 is the study of kinetics – equilibrium constant. When it comes to the study of acid-base, equilibrium constant plays an important role that tells how much of the H+ ion will be released into the solution. In this lab, the method of titrimetry was performed

Date Performed: September 9 ,2011 SPECTROPHOTOMETRIC DETERMINATION OF THE ACID DISSOCIATION CONSTANT OF METHYL RED M.C. Caligagan ,M.N.Q. Tolentino and M.Q. Clores Institute of Chemistry, College of Science University of the Philippines, Diliman, Quezon City, Philippines Received :September 21,2011 ABSTRACT This experiment aims to determine the acid dissociation constant value of Methyl Red by means of spectrophotometry. Ten samples were spectrophotometrically analyzed under a UV-Vis

strong base (NaOH) against a weak acid (Histidine monohydrochoride ) enables us to know of properties of the weak acid (histidine). Such properties include the pKa of the acid and the pH range of the buffering capacity. One way to relate pH to pka would be through the Henderson – Hasselbalch equation as stated below. pH = pKa + log ([Conjugate Base]/[Acid]) Using this equation and the mid-point of the buffering capacity of the acid, we will be

temperature and equilibrium constant in weak acids Topic/Purpose The topic of the investigation is equilibria of weak acids, using ethanoic acid. The purpose of the investigation is to determine the relationship between temperature and the equilibrium/dissociation constant of weak acids, by calculating the K_a value of ethanoic acid at various temperatures. Aim The aim of the investigation is to determine whether the relationship between temperature and the equilibrium constant is linear or exponential

29 EXPERIMENT 3. ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this experiment a solution of hydrochloric acid is prepared, standardized against pure sodium carbonate, and used to determine the percentage of carbonate in a sample. An aqueous solution of hydrochloric acid is almost completely dissociated into hydrated protons and chloride ions. Therefore, in a titration with hydrochloric acid the active titrant species is

to determine a weak acid and its acid dissociation constant (Ka) through a process of an acid-base titration. A sample of the unknown weak acid was made into a 100 mL solution, where 20 mL was take out for titration; phenolphthalein was added in as the indicator. NaOH, as the titrant, is dripped into the weak acid solution until a slight change in coloration (from clear to pink) was noted. At this point in time, the titrated solution is diluted with 20 mL more of the weak acid; the pH is then measured

INTRODUCTION For this experiment, a weak acid-buffer titration will be performed. While acids produce hydronium ions in water, bases produce hydroxide ions. To determine how strong an acid or base is, levels of dissociation are observed. While a strong acid or base entirely dissociates in solution, a weak acid or base only partially dissociates in solution. The extent to which a weak acid dissociates in an aqueous solution can be denoted by the constant, Ka, which stands for the ratio in products

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 and biochemistry. Apart from the carboxylic acids, the carboxyl group also parents a large family of related compounds called carboxylic acid derivatives (amides, esters, thioesters, acyl halides

The purpose of Experiment 3 was to determine the pKa of a common acid-base indicator and color dye, bromothymol blue. Acid-base indicators are usually weak acid or base that change color with various pH levels in a solution, giving one specific color for acidic solutions (HIn) and another color for basic solutions (In^-). In the case of bromothymol blue, a weak acid, the reagent turns yellow in the presence of an acidic solution and turns blue in the presence of a basic solution. As the pH of the