Introduction In Chemistry 1211 lab the main objective was to identify the name of the unknown acid #2651145-PLF13 that was issued by the instructor. Melting point, titration of the unknown acid, calculation of equivalent weight, pKa, solubility tests, and properties of a hydrochloric acid; these procedures were used to characterize the unknown acid and then compared with known substances using GSU Chemistry department search engine. By doing this experiment he or she will develop an understanding of the properties of organic acids and differences between properties of a strong acid such hydrochloric acid. Experimental The first procedure to identify the unknown organic acid was finding the correct melting point. This was done by taking small amounts of the unknown acid.
The reaction that occurred with this step was displacement and metathesis in the form of gas formation. The balanced equation of this step looks as follows: CuSO4aq+Zns→Cus+ZnSO4(aq) Once this step was finished, the remaining copper was retrieved. First, to recover the copper HCl was added to remove all the zinc. When this happened, a yellow tint was observed in the liquid, as well as bubbling as the zinc was broken down. Once the copper dried out, it was weighed and came to a total of 240 mg.
To perform this experiment, we will utilize emission spectra, titrations, and thermal gravimetric analysis, using knowledge from Experiments 10, 4, Titrations of Na2CO3 and NAHCO3 by HCl (hydrochloric acid) will be performed to determine the concentration of HCl, as well as the number of moles of HCl present within the sample of baking soda. As a result, we will be able to determine the molar concentration of HCl by determining its equivalence point (the point on the graph where the exact amount of rectant needed to perform a reaction has been added) from graphical analysis. Na2CO3(aq.) + HCl(aq.) ==> NaHCO3(aq.)
Radu Purtuc | Chemistry 231 - Lab | Section 32 Ronnie :: team-member TECH 705, SEPARATING ACIDS AND NEUTRAL COMPOUNDS BY SOLVENT EXTRACTION - MACROSCALE EXTRACTION July 6, 2006 Lab Report INTRODUCTION Purpose: using extraction technique to separate acetanilide, p-toluic acid, and p-tert-butylphenol; then measure the melting points of each compound and comparing them to the statistical values. Background: separating acids and neutral compounds by solvent extraction is a useful technique used in practice by chemists to separate organic compounds from mixture of other compounds. It generally involve several steps, with limiting factors being the number and output purity of compounds to be extracted from source mixture. A number of specific compound solvents not inter-miscible are used to separate and dissolve compounds, and a physical transfer between solvents is employed. An example of use is cleaning compounds of impurities, where different solvents work as a molecular filter that interacts differentially with compound and impurities respectively.
The concentration is measured in molarity. Molarity is the measure of moles of solute per liter of solution. The rate law helps one find solution's reaction order. If the reaction order is zero, the graphical representation is concentration vs. time, and the slope of the line is the negative rate constant. 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.
Liquids and Solids Purpose: The goal of this experiment is to be able to identify melting/boiling points of substances. We can then use these methods to identify unknown substances because of constants in melting/boiling points. Procedure: 1. Boiling Point a. Begin by adding 1 mL of rubbing alcohol to test tube and attach a thermometer to it.
In uncompensated respiratory alkalosis, the You correctly answered: b. carbon dioxide levels of the blood are low. 3. What type of breathing results in acidosis? Your answer: b. hypoventilation Correct answer: d. hypoventilation and rebreathing 4. With renal compensation for respiratory acidosis, the pH of the urine You correctly answered: b. decreased because [H+ ] increased.
To note the endpoint of the reaction, a pH electrode probe is placed in the reactant. In understanding and finding out the results of the laboratory, it is important to know its components, find the percent composition to see how much acetic acid is in vinegar, and to find the pH solution of vinegar. Experimental Investigation One: First, be sure that the temperature and the pH electrode are set up and are connected to LoggerPro software. Rinse the probe with distilled water after you unscrew the top cap and then dry afterwards. To calibrate the
Tablet | A report based on a scientific experiment designed to investigate and compare the rates at which different forms of aspirin dissolve. | 11-11-2013 | Introduction This experiment was designed to investigate and compare the rates at which different aspirin tablets dissolve in both Water (H2O [representing saliva]) and Hydrochloric Acid (HCl [representing the stomach’s acid]). The amount of Water and Hydrochloric Acid will be kept constant between tablets, and tests. Aim To investigate and compare the rates at which different Aspirin Tablets dissolve. The different kinds of Aspirin tablets are: * Enteric Coated Tablets * Capsules * Regular Tablets * Dissolving Tablets.
William Flores-Paz Monitoring Acid-Base Titrations with a pH meter October 30, 2013 Introduction The purpose of this experiment was to record the volume of HCl and acetic acid with a NaOH with a known molarity. This data would allow us to create a graph so we could compare the two titration curves. We would then use these curves to calculate the unknown molarities. HCl + NaOH >H2O + NaCl This equation shows the relationship between the acid and the base then the reaction goes forward and they are titrated creating salt and water. 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.