The property or power of conducting heat, electricity, or sound” and is used as such in chemistry (Dictionary, 2014). In the medical field however, specialists are now trying to use carbon nanotubes (CNT’s) to aid in the absorption of medicines used to treat terminal illnesses, it is also used in gels, EKG, EEG and other testing supplies (Shao, 2013). The lab test today is going to help determine whether a substance is Conductive and the type of bond in portrays—ionic, polar covalent, or non-polar covalent, with a series of tests and results using an array of samples. If water is used as a solvent then sodium chloride, calcium sulfate, potassium aluminum sulfate, potassium nitrate, ammonium nitrate, copper (II) nitrate, and sucrose will be dissolved because they are soluble solids with ionic and polar bonds placed into a polar covalent liquid. Glycerin and ethanol will be miscible in water as well due to their polar bonds.
Add a quarter spatula of copper (II) oxide and warm the solution gently to the 4th test tube and record observations. 7. To the 5th test tube, add 3cm3 of ethanol a couple of drops of conc, sulphuric acid and warm gently. Pour the resulting mixture into 30cm3 of sodium carbonate solution to remove excess acid and smell and record observations. Experiment 2 Time | Observations | 5 minutes | Bubbled like sugar | Once salt water was added | Turned soapy white and thick | Equation: METHOD 1) Put 2 cm3 of castor oil into a 250 cm3 beaker and add 10 cm3 of 5mol.dm-3 sodium hydroxide from a measuring cylinder.
In the first part, five 100 mL flasks of 5 mL ligand solution, 5 mL 2 M sodium acetate, 4 mL 3 M NH2OH, and 1-5 mL Fe2+ solution are diluted with water. The absorption spectrum for varying concentrations of Fe2+ are measured using a spectrophotometer and the data is graphed in Excel. The slope of the line is ε in the Beer-Lambart equation A = εcl. In the second part of the experiment, eleven flasks containing diluted stock solutions of Fe2+ and ligand are mixed with 5 mL 2 M sodium acetate and 4 mL 3 M NH2OH and diluted with water. The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel.
Separation of the components of Extra-Strength Excedrin I: Acid-Base extraction Introduction The purpose of this experiment is to analyze the purity of Extra-Strength Excedrin® by utilizing thin-layer chromatography and determine the percent recoveries of its components. Three active ingredients will be extracted and collected from two tablets of Extra-Strength Excedrin® by utilizing acid-base extraction method. Three active ingredients of Extra-Strength Excedrin® are acetylsalicylic acid(aspirin), acetaminophen and caffeine, and their structures are: In addition, there is a binding material, which binds other three components together. These compounds can be separated by acid-base extraction because of their different acidities. A binding material can be separated by dissolving the tablet in ether since three active ingredients are soluble.
Halides Lab: Background information: Halide ions are reactive and useful. Salts are positively charged ions (metals) combined with any negative ions (nonmetal), and when placed in a solution (water) it separates into the cations and anions that made it up. The Purpose of this lab is to find out how the Halides react with the indicators, and to determine the identity of the two unknown solutions (A and B). Color of solutions prior to experiment: NaF | NaCI | KBr | KI | Unknown A | Unknown B | clear | clear | clear | clear | clear | clear | Color of indicator prior to experiment: 5% Bleach (NaOCI) | 0.2 M Na2S2O3 | 0.1 M AgNO3 | 0.5 M Ca(NO3)2 | clear | clear | clear | clear | Halide solutions | NaF | NaCI | KBr | KI | unknown A | unknown B | Test 1: Ca(NO3)2 | Cloudy White (Nothing) | Clear | Nothing | light yellow (Nothing) | Nothing | Nothing | Test 2, Part A: AgNO3 | clear (Nothing) | Milky White | Gold (Cloudy yellow) | milky green (Cloudy yellow) | turned white, film developed on top layer | Milky | Test 2, Part B: add Na2S2O3 to test tube from part A | Dark Orange/brown | Clear | Dark Gold(precipitate yellow then clear) | milky green (no change) | white precipitation, settled on bottom | Milky | Test 3: NaOCI (Bleach) | Clear (Nothing) | Nothing | Nothing | Orange (Clear) | Nothing | Orange | Unknown A is identified as NaCI (Sodium Chloride), because in test#1 the solution turned a cloudy white color when Ca(NO3)2 (Calcium nitrate) was added. In the first part of test#2, when AgNO3 (Silver nitrate) is added, the solution turned white, with a thin layer of film developing on the surface.
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.
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.
ABSTRACT: The lab of “observations of chemical changes” was to observe the changes that occur in chemical reactions and attempt to interpret these changes. In these experiments it taught me how to interpret chemical reactions with acids and bases. Also, how one chemical can have many different reactions when combined with other chemicals and how to interpret each reaction as what it could mean. I discovered not only how to measure out a well-balanced chemical combination to receive a reaction but to know how to test for acids and bases using a few different methods. Other tests also included in this experiment were testing for Sodium Bicarbonate, and Starch.
In this lab you will use a method called visible spectroscopy to determine the concentration of a solution of CoCl2. This method relies on the fact that colored solutions will
NH4+ Heat 5mL of the test solution in a beaker. Test the gas evolved with damp red litmus paper. The damp red litmus turns blue Ammonia gas. - 4. Ag+ Add HCl(aq) to original solution.