Flame Tests – Identifying cations Abstract: My objective of this experiment is to identify cations present in water samples. To do this I will be doing 7 experiments using different types of metal ions. To do this I will clan the flame test wire by dipping it into acid, then heat nichrome wire in a Bunsen flame until no colour is visible in the flame. Then dip the wire into acid, then into salt solutions and hold wire in edge of flame and finally note the colour of the flame, then repeating this for all the salt solutions. Introduction: This report is based upon my hypothesis taken out in an experiment.
Aim: | The aim of this experiment is to analyse a sample of vinegar and determine it’s concentration. | | | Hypothesis: | It’s expected that the aceatic acid will have the concentration of 0.1mol as this is the molarity of the NaOH as they have a 1:1 ratio of moles as it states in their chemical equations. | | | Apparatus: | * 1 x retort stand * 1 x retort burette clamp * 1 x burette * 1 x pipette * 1 x glass funnel * 2 x Conical Flasks * Sheet of filter paper * 200mL of 0.1 mol L-1 NaOH * 200mL of acetic acid of unknown concentration | | | Procedure: | 1. WARNING: Wear safety glasses and gloves! 2.
Part Two: 1: The purpose of this experiment was to remove the contaminants from the impure Acetanilide and see how much of the crystals we could recover through the recrystallization process. 2: Chemicals and equip: Acetanilide, 600 ml beaker, 250 ml beaker, hot plate, filter paper, decolorizing charcoal, stemless funnel, vacuum filtration apparatus, and clamps. 3: In this experiment we took 6 grams of impure acetanilide and put it through a recrystallization process to filter out the impurities. We let our solution dissolve into a solvent that included hot water and decolorizing charcoal. We then let it boil and become one substance.
Experiment 4: Using Buffers Name: Andrew Duval Lab Partners: None Location: My House Course Number: Chem 112 Date: July 28, 2013 Abstract: This lab aims to teach us about the use of buffers, or in this case vinegar. Buffers are used to control the pH of a solution, because they are able to able to absorb strong acid or bases. Because of this fact, we can add acid or basic mixtures and control the outcome of the pH by also mixing a buffer in there as well. In this lab we will be adding 0.1M and 6M HCL and NaOH to a two mixtures. One mixture will contain vinegar, and the other will contain distilled water.
Recrystallization of the Benzoic Acid Antonio Roki CHE 311L: Organic Chemistry I Section #2 September 14, 2012 Recrystallization of the Benzoic Acid Summary: The purpose of this experiment was to determine if the process of the Recrystallization is the good method of purification of the solid substance based on its different solubility values. This experiment conducted the purification of the Benzoic acid. The melting point range of the impure Benzoic acid was determined to be 86- 108 °C. Melting point was measured one more time after the process of the purification and was determined to be 111-117 °C. The melting point ranges of the impure and pure benzoic acid seemed reasonable.
In this experiment we will determine the percent composition of the NaHCO_3 and the contaminates in the solution. Experiment 1 – Titration of NaHCO_3 with HCl. Titration allows for the equilibration of the unknown substance with an acid. The amount of acid required to neutralize the unknown will give data on the amount of base present. The titration between NaHCO_3 and HCl will determine the percent composition of NaHCO_3 in the Athenium Baking Soda.
Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined. Procedure: 1) Using the graduated cylinder add 10.0 mL of water into the Erlenmeyer flask. 2) Add 5.0 mL of HCl into the flask using another graduated cylinder because acid goes into water when mixing them. 3) Add three drops of phenolphthalein indicator into the flask. 4) Swirl the flask in circular movements to mix the substances.
Synthesis of Acetylsalicylic Acid (Aspirin) AINI A.G (2012xxxxxx) 19.03.13 (TUES) Abstract Acetylsalicylic acid was obtained from esterification reaction between salicylic acid and acetic anhydride in 97.40% yield. The product was tested for its purity by ferric chloride test and then identified by its melting point Results and Discussion Acetylsalicylic acid was obtained in 97.40% yield by allowing esterification reaction to occur between salicylic acid and acetic anhydride. Recrystallization of the crude acetylsalicylic acid gave white crystals, m.p. 101-107 0C (lit. 135-1360C ).
Separation of a Mixture of Solids Purpose To become familiar with separating a mixture of solids, as well as to become familiar with separation techniques dependant on the chemical make-up of a substance. Data Separation Flowchart Initial Mixture (iron fillings, table salt, benzoic acid, sand) | | | | | | | | | | | Put mixture in a cup and hold the magnet over it. | | | | | | | | | Mixture - iron fillings (table salt, benzoic acid, sand) | | | | | | | | | | | Boil mixture to dissolve table salt and hopefully benzoic acid. | | | | | | | | Filter out water with table salt (and hopefully benzoic acid) | | | | | | | | | | | | | | | | | | | | | | | | Mixture - iron fillings and sand (table salt and benzoic acid | | Data Table 1: Experiment Data | | Grams | Percent of mixture | Iron filings | 1.6 | 23.8% | Sand | 1.7 | 25.0% | Table salt | 1.7 | 25.0% | Benzoic acid | 1.7 | 25.0% | Total | 6.7 | 98.8% | Hands-on Labs, Inc Observations I observed that while decanting the sand-table salt-benzoic acid mixture that it appeared that some of the sand may have been decanted out of the beaker as well. I also observed that while filtering the benzoic acid-salt mixture that some of the mixture stuck to the sides of the filter and may not have been filtered properly.
CHE 131 Spring 2008 Experiment 4 - Determination of acetic acid in vinegar Preliminary Reading: Chang, 9th ed., section 4.7, pp. 150-153 Introduction: The principal component of vinegar (besides water) is acetic acid, HC2H3O2, a weak acid. In this experiment you will determine the concentration of acetic acid in a vinegar sample by titrating the acetic acid with the strong base sodium hydroxide, NaOH. The stoichiometry of the neutralization reaction is as follows: Molecular: Net Ionic: Neutralization: HC2H3O2(aq) + NaOH(aq) → NaC2H3O2(aq) + H2O HC2H3O2(aq) + OH¯ (aq) → C2H3O2+ (aq) + H2O H+(aq) + OH¯(aq) → H2O(aq) (1) (2) (3) Definition: The end point (also known as the equivalence point) of a titration occurs when the initial number of moles of H+ from the acid has been exactly neutralized by an equal number of moles of OH¯ ion from the sodium hydroxide: moles H+ = moles OH¯ (4) The only species present at the end point are the products, sodium acetate and water. For reasons that are beyond the scope of the material covered so far (but which will be covered in CHE 132), the solution is very slightly basic at the end point of a weak acid-strong base titration.