Qualitative Cation Tests Peter Jeschofnig‚ Ph.D. Version 42-0194-00-01 Lab Report Assistant This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions‚ diagrams if needed‚ and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing
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Trimethylmethanol or 1‚2‚4‚5-Tetrachlorobenzene. Introduction Extraction is a process of transferring a solute from one solvent to another. It is usually used to separate one or more components from a mixture. Diethyl ether‚ dichloromethane (methylene chloride)‚ trichloromethane (chloroform)‚ pentane‚ hexane‚ petroleum ether are some of the solvents commonly used for extracting aqueous solutions. Petroleum ether and ligroin are mixtures of hydrocarbons whereas the other liquids mentioned earlier are pure
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2 drops of sodium phosphate solution into five vertical wells under column number 1. Place 2 drops of sodium iodide solution into five vertical wells under 2. Place 2 drops of sodium sulfate solution into five vertical wells under 3. Place 2 drops of sodium chloride solution into five vertical wells under 4. Place 2 drops of sodium bicarbonate solution into five vertical wells under 5. Place 2 drops ofcarbonate solution into five vertical wells under 6. Place 2 drops of sodium hydroxide solution
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are four halide salts used in this experiment that are found in the human body. Sodium fluoride is poisonous‚ but has been traced to be beneficial to humans in the prevention of tooth decay. Sodium chloride is added to many of our foods to increase flavor. Sodium chloride is important for many life processes‚ but too much intake is linked to high blood pressure. Sodium bromide is distributed throughout body tissues. Sodium iodine controls cell growth. The principal oxidation number of the halogens is
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|Neither Ionic |Not measured |Yes | | In this lab‚ the neutralization of of an acid and a base was observed. 20 drops of sodium hydroxide were added to an evaporating dish‚ followed by a drop of phenolphthalein indicator. The solution turned pink when the indicator was included. Quantitative Neutralization was used by adding drops of hydrochloric acid one by one to a sodium hydroxide-phenolphthalein solution. After a certain number of drops were added‚
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Unit 18 B Study Guide 1. Find the solubility (in mol/L) of lead(II) chloride (PbCl2) at 25oC. Ksp = 1.62e–5. A) 1.59e–2 B) 2.53e–2 C) 6.64e–17 D) 2.01e–3 E) 2.01e–2 2. The two salts AgX and AgY have very similar solubilities in water. It is known that the salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY? A) Nothing. B) HY is stronger than HX. C) HX is stronger than HY. D) The acids have equal strengths. E)
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Performed: 02/05/2013 Submitted: 02/06/2013 Section 1: Title Physical and Chemical Properties Section 2: Purpose This labs is intended to help me investigate chemical and physical properties of pure substances. Section 3: Procedure In this experiment‚ I observed substances in their natural state‚ and recorded their apparent physical properties. I then tested the substances to determine how they react when their natural environments were altered. The pure substances were tested to see
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Desiree Trujillo March 6th‚ 2013 Lab # 3 Chemistry 101 Physical & Chemical Properties Purpose To examine the physical and chemical properties of multiple natural chemical substances‚ and to determine which changes are chemical and which are physical. Data Solubility or Reaction | SubstanceName | Color | Odor | Effectof Heat | ColdH2O | HotH2O | LitmusTest | DiluteHCl | DiluteNaOH | Mg | Silver
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the right (product) side. This is why temperature has to be on the reactants side (endothermic) in order for this shift to be possible. 5) If you add NaCl into the hydrated Cobalt (II) ion equilibrium‚ the concentration of the chloride ions would increase and some sodium ions would be formed. Because of this‚ the concentration of reactants increases which causes the equilibrium system to move to the right (products) side. Therefore‚ the solution turns purple. 6) Cr2O72- + 2OH- ↔ 2CrO42- + H2O
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25cm3 Of Sodium Carbonate of an unknown Concentration Using Methyl Orange Indicator. Pipette Solution | Sodium Carbonate | Mol/dm3 | Burette Solution | Hydrochloric Acid | 0.12Mol/dm3 | Indicator | Methyl Orange | | | | Trial 1 | Trial 2 | Trial 3 | Burette readings | Final/cm3 ± 0.05 | 14.80 | 14.50 | 14.60 | | Initial/cm3 ±0.05 | 0.00 | 0.00 | 0.00 | Volume Used (titre)/cm3±0.10 | | 14.80 | 14.50 | 14.60 | Mean Titre/cm3 ±0.05 | | 14.63 | * The sodium chloride and hydrochloric
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