Distillation and IR Spectroscopy CHE 361L Christian Johnson 02/17/2018 Introduction The purpose of this lab was to separate an unknown binary mixture by distillation and use IR spectroscopy along with the placement of known functional groups in order to determine the identity of the compounds. Based upon the potential unknown solutions, there are a few specific functional groups that can specifically be targeted in order to accurately depict the identity. The functional groups and specified area on the IR spectrum are located below. By directly establishing where these certain functional groups are located on the IR spectrum, the identification of the unknown can be confidently established. Each of the potential compounds have a certain feature
Water samples from the Clark Fork have been taken and will be tested using both absorption and emissions spectroscopy in order to check the levels of group IA and IIA metal ions. When electrons in an element are excited energy is released that can be measured as light. Each element releases different levels of energy that are observed as different wavelengths of light. With the proper equations (E=hv and E=hc/⋋), emission spectroscopy can be used to find the wavelength and frequency of light emitted by the excited electrons. This will help determine the types of ions present in the water sample.
Gracen Seiler April 7th, 2015 Section- 109 Investigating Stoichiometry with Sodium Salts of Carbonic Acid Introduction- This experiment is intended to help find a better understanding of chemical stoichiometry through titrations of NaHCO3 and NA2CO3 with HCl. A chemical reaction is a process that involves rearrangement of the molecular or ionic structure of a substance, as opposed to a change in physical form in a nuclear reaction. Titration is when a measured amount of solution of unknown volume is added to a known volume of a second solution until the reaction between them is complete. The objective of this experiment is reacting sodium bicarbonate (NaHCO3) and sodium carbonate (NaCO3) with hydrochloric acid (HCl) to produce sodium chloride (NaCl), water (H20) and carbon dioxide (CO2). -Use the titrations of the following chemical reactions: NaHCO3 + HCl (aq) NaCl (aq) + H2O (l) + CO2 (g) 2HCl (aq) + Na2CO3 (s) 2NaCl (aq) + H2O (l) + CO2 (g) Experimental procedure- Two Erlenmeyer flask must be labeled “unknown 1 and unknown 2”.
Objectives: The purpose of this lab is to observe the reaction of crystal violet and sodium hydroxide by looking at the relationship between concentration and time elapsed of the crystal violet. CV+ + OH- CVOH To quantitatively observe this reaction of crystal violet, the rate law is used. The rate law tells us that the rate is equal to a rate constant (k) multiplied by the concentration of crystal violet to the power of its reaction order ([CV+]p) and the concentration of hydroxide to the power of its reaction order ([OH-]q). Rate = k[CV+]p[OH-]q To fully understand the rate law, concentrations of the substances must be looked at first. The concentration is measured in molarity.
Laboratory Report Chemistry Mr. Crider Title: Validating the Gas Laws Purpose: The purpose of this lab is to validate Charles’ Law, Boyle’s Law, and I deal Gas Law by attempting experiments that prove all three Kinetic Molecular Theories are in face true. Hypothesis: If the first procedure shows a fixed amount of gas at a constant will both either increase or decrease simultaneously according to Charles’s Law. If an unknown volume of air has mass in the second procedure, then it is a form of matter because of the presence of atoms. If the third procedure has a fixed amount of gas at a constant temperature, then according to Boyle’s Law the volume of the gas will increase as the pressure of the gas decrease or vice versa. Materials: Safety Goggle Laboratory Apron 60-cm3 syringe with end cap 2 utility clamps Ring stand and ring Wire gauze 600-mL Beaker Thermometer inserted into spilt stopper Bunsen Burner Air pump w/ pressure gauge Balance 1 L Graduated Cylinder (or assume syringe vol.
Why is it important to determine these physical properties of a substance? The melting point of a solid is the point at which a solid becomes a liquid with standard atmospheric pressure. The boiling point of a liquid equals the external pressure. It is important to know these characteristics of a substance so that you can handle them in the correct manner. The boiling point and melting point can also be used to identify an unknown substance.
Subject: Separation of unknown organics by flash column chromatography Introduction Column chromatography is a process that is used as a purification technique. The purpose of this lab is to isolate desired compounds from a mixture. The goal of this experiment is to apply column chromatography to separate two compounds and analyze their purity. It will be accomplished by running the mixture to be analyzed through the top of the column tube and then find purities by a TLC plate after the mixture has been separated. Reactions: Results: Calculations: Discussion: The TLC plate had 5 circles, indicating the 5 compounds, when it was under the UV lamp.
3) Write equations to indicate what you consider to have happened in each case in which there was precipitate formed. Use ions to represent the species in the reacting solutions, but for those products that were precipitates write a formula for the compound. Place (aq) after those species in solution and (s) after the precipitates. Be sure to write the equations so that both atoms and charge are conserved. For example: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) ( AgCl(s) + Na+(aq) + NO3-(aq) 4) Rewrite the equations, leaving out the ions not involved in the reaction (spectators).
Strong electrolytes produce large numbers of ions, which results in high conductivity values. Weak electrolytes result in low conductivity, and non-electrolytes should result in no conductivity. In this experiment, you will observe several factors that determine whether or not a solution conducts, and if so, the relative magnitude of the conductivity. Thus, this simple experiment allows you to learn a great deal about different compounds and their resulting solutions. In each part of the experiment, you will be observing a different property of electrolytes.
(d) What evidence suggests that nitrate compounds are soluble in water? (e) Write the chemical formula for each precipitate that formed. Apply and Extend (f) Write a balanced chemical equation for each precipitation reaction that occurred. (g) Why is it necessary to use distilled water to prepare the solutions used in this investigation? (h) "Hard" water contains a high concentration of calcium ions.