In order to find the equivalent weight a titration of the unknown acid had to be conducted. Equivalent weight is the weight of the substance in grams divided by the average molarity of the sodium hydroxide solution times the volume from the titration in liters. If the molarity of your sodium hydroxide solution were too low then the equivalent weight would be off significantly. In order to calculate a decent molarity a short series of titrating was conducted using KHP. Find the molarity is essential to numerous amounts of future procedures such as equivalent weigh.
The capsule will soften but not completely dissolve in the water, however will dissolve in the Hydrochloric Acid. The Tablet will slowly dissolve in water, however more rapidly in Hydrochloric Acid – however loosely comparable to the dissolving tablet. Equipment * Water * 2M Hydrochloric Acid * Test Tubes or Beakers * Stopwatch * 2 x Aspirin Enteric Coated Tablets * 2 x Aspirin Capsule * 2 x Regular Aspirin Tablets * 2 x Dissolving Aspirin Tablets * Safety Glasse * (Recommended) Gloves for handling Hydrochloric Acid Safety Precautions * 2M Hydrochloric Acid will burn both skin and clothing * Always wear eye protection while handling Hydrochloric Acid * Avoid contact with
Lab #09: Is the Substance Ionic or Covalent? Purpose: To identify compounds as ionic or covalent based on their properties. We will do this by testing melting point, conductivity, and solubility. Hypothesis: Draw a chart in which you will predict what your results will look like for the three different tests for an ionic compound and a covalent compound. We will fill this table in
The purpose of washing the test tubes thoroughly is so the chemicals don’t cross contaminate and affect the outcome of another section of the lab. Hypothesis: 1. If a substance contains lipids then when rubbed onto a paper bag a transparent or opaque spot will appear. 2. Is a substance contains starches then when iodine solution is added to the substance it will change from yellow-brown to blue-black.
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.
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 synthesis of NaCl further identified the ionic compound by reacting sodium hydroxide and hydrochloric acid and obtaining solid sodium chloride. The synthesized compound formed was used to perform another flame test and the chloride anion test, which further solidified the identification of NaCl as the ionic compound. Introduction The purpose of the experiment was to identify unknown ionic compound
Make sure the rubber stopper is securely in place since gas can easily leak out. Collecting the gaseous product: Prepare the gas collection bottle by positioning the bottle so that its mouth is. directly over the hole at the bottom of the trough; this is where the gas will enter the bottle. After the reaction, slide a square of glass over the mouth of the bottle while the bottle is still under water. Keeping the glass fixed to the mouth, raise the collection bottle and invert.
Use a small clamp to secure the pipet and the ring stand while placing a clean collection vial below the stem to collect the filtered extract. | The extract after being filtered prevented the
Then the content of the chloride in the original salt is then calculated using stoichiometry (Chemistry Department, 2014). Theory: Gravimetric analysis is the measurement of mass, which by definition is categorized into four types however the use of one is only necessary in this experiment, which is precipitation (Gravimetric Analysis, 2012). Therefore the goal is to determine the original amount of ion. This is by isolating the ion in solution by a precipitation reaction, filtering and washing the precipitate free of pollutants, then the conversion of that precipitate to a product of the unknown sample given (Gravimetric Analysis, 2012).Therefore determining the quantitative of that substance by the precipitation reaction. The equation of the precipitate proceeds as follow if followed by the criteria given.