Objectives 1. To separate a mixture of an acid and a neutral compound into its component by extraction. 2. To determine the melting point and the yield of the benzoic acid and the unknown sample. 3. To determine the unknown sample whether is is 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
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Simple Equilibria 1. Identify the acid/base and their conjugate base/acid‚ and which definition you use to determine(Bronsted‚ Arrhenius or Lewis): a. HCO3- + H+ ↔ H2CO3 Base conj acid: Bronsted b. HCO3- ↔ CO32- + H+ Acid conj base : Arrhenius c. CH3NH2 + H2O ↔ CH3NH3+ + OHBase acid conj acid conj base : Lewis d. C6H5OH + H2O ↔ C6H5O- + H3O+ Acid base conj base conj acid : Lewis‚ Arrhenius‚ Bronsted e. H2O + H2O ↔ H3O + + OHAcid base conj acid conj base - 2. Assuming Kw = 1x10-14
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Enthalpy of Neutralization Introduction Energy changes always accompany chemical reactions. If energy‚ in the form of heat‚ is liberated the reaction is exothermic and if energy is absorbed the reaction is endothermic. Thermochemistry is concerned with the measurement of the amount of heat evolved or absorbed. The heat (or enthalpy) of neutralization (∆H) is the heat evolved when an acid and a base react to form a salt plus water. Eq. 1 HNO2(aq) + NAOH(aq) → NaNO2(aq) + H2O(l) + Q Q in the
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Experiment Title: Acid-Base Titration Abstract: Vinegar is a common household item containing acetic acid as well as some other chemicals. This experiment is designed to determine the molar concentration of acetic acid in a sample of vinegar by titrating it with a standard solution of NaOH. CH3COOH(aq) + NaOH(aq) -> CH3COONa(aq) + H2O(l) By adding the sodium hydroxide‚ which is a basic solution‚ to the acetic acid‚ which is an acidic solution‚ a neutralization reaction occurs. An indicator
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Experiment 2 Acid/Base Titration John J. Purdue CHM 321 – Fall 2012 TA: Scott Cole Section 1 September 4‚ 2012 Unknown Concentration: X.XX ± X.XX M (@95% confidence interval) (adapted from a report prepared by N. Skrynnikov‚ 2009) Abstract The concentration of an unknown acid (HA) solution was determined by titration with a standardized solution of sodium hydroxide. The standardization of NaOH was done by titration with a solid acid sample‚ potassium hydrogen phthalate (KHP)‚ and phenolphthalein
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Introduction: In this lab‚ we measured the acid-base strengths of seven separate organic compounds. The lab was painless to perform‚ it consisted of adding a small amount of one of the organic compounds to a well‚ and testing the pH via testing paper. The color of the paper was then analyzed to determine what the pH of the compound was. The structures were benzenesulfonic acid‚ benzoic acid‚ benzyl alcohol‚ benzylamine‚ p-cresol‚ and p-toluidine. My initial hypothesis about the acidity/basicity
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A. Title – Acid-Base Extraction with Separatory Funnel B. Introduction – The main objective of the experiment was the extract an acid‚ a base‚ and a neutral compound from a 2:1:1 compound of benzoic acid‚ p-nitroaniline‚ and azobenzene. In theory‚ an extraction technique based on phase distribution should allow two immiscible solvents to separate with a portion of the solute distributed into each. Using a separatory funnel‚ acids were extracted with bases (NaOH)‚ and bases were extracted
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For my project‚ I had to create my own acid-base indicator and find out what happens when it is placed in an acidic solution (vinegar) and a basic solution (dissolved baking soda). I chose my indicator to be a fruit because fruits can be very effective at determining how acidic or basic a substance is. My fruit was a blueberry‚ but I couldn’t use raw blueberries because it’s not going to give me the best results. I had to make blueberry juice. I did this by placing several blueberries in a blender
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Lab Report: Acid and Base Indicator Lab The title of my lab report is “Acid and Base Indicator Lab” this lab is testing what household solutions area bases depending on what color they changed. You have to use the pH balance scale to determine Acid‚ Base‚ and Neutral. On this lab we used 7 different solutions to determine if it’s either base‚ acid‚ and neutral. These are ammonia‚ vinegar; drain cleaner‚ soft drink‚ baking soda‚ detergent‚ and lemon juice are the solutions that are going to be
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Acid-Base Strengths of Organic Compounds By: Chris Frankmore Due Date: February 15‚ 2011 Resonance Benzenesulfonic Acid Benzoic Acid Benzyl Alcohol Benzylamine P-Cresol P-Toluidine Acid/Base | Structure | pH | Why It is a strong/weak acid/base | Benzenesulfonic Acid | | 1 | This is a strong acid because it has a pH of 1. Another reason why this is a strong acid is that its conjugate base has strong resonance stabilization
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