| Initial volume of NaOH in burette (ml) ±0.05 | Final Volume of NaOH in burette (ml) ±0.05 | Final – initial Burette Reading (Volume of NaOH used) (ml) ±0.1 | Qualitative Observations | Phenolphthalein | 0.00 | 0.90 | 0.9 | At first when the base was being dropped into the vinegar there wasn’t a color change‚ however when the solutions came close to full titration‚ the solution would turn pink and once mixed would turn clear again | | 0.90 | 2.30 | 1.4 | | | 2.30 | 3.20 | 0.9 | |
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Sulfa Drugs: Preparation of Sulfanilamide Introduction The purpose of this experiment is to prepare sulfanilamide from p-Acetamidobenzenesulfonyl chloride. This will be done using reflux‚ vacuum filtration‚ and melting point determination. Experiment Scheme6 Figure 1. Reaction equation.6 A hot water bath was prepared in a fume hood using a 250-mL beaker. 2.5 g of p-acetamidobenzenesulfonyl chloride was placed into a 50 mL Erlenmeyer flask and 11 mL of dilute ammonium hydroxide solution
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oscillator model. In addition‚ the specific molecular vibration nodes are visualized using computational chemistry software. Introduction The Lewis acid-base is defined simply: acids accept electrons‚ and bases donate electrons. Lewis acids and bases are important in inorganic syntheses because bonds are usually formed between an electron-deficient Lewis base and electron-rich Lewis acid in the absence of compounds that are unable to donate protons. There are two types of boron-hydrogen bonds‚ in which
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chemical reactions between twelve different basic compounds. Each reaction revealed chemical properties consisting of color change‚ CO2 gas formation‚ and/or precipitate formation. Certain reactions made it possible to distinguish between an acid and a base. Through the results of this experiment‚ chemical properties observed in the reactions could be used to associate similar chemical substances and properties in household products. Experiment and Observations: The first step in this experiment was
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light shade of pink when it was in a solution with a pH of 7. Neutralization reactions occur when an acid is mixed with a base. The product of this reaction is a salt and water. These reactions are double displacement reactions‚ because the cation of the base mixes with the anion from the acid‚ forming a base‚ and the hydrogen from the acid mixes with the anion from the base‚ forming water. In this reaction‚ the sodium ion from the sodium hydroxide attracts to the acetate ion from the acetic acid
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Procedure The procedure stated in Chem 2120 experiment 6 Williamson Ether Synthesis of Phenacetin laboratory manual was followed without any major changes. Data and results Compound Amount used MW (g/mol) Moles Stoichiometry/Comments acetaminophen 0.354 g 151.16 2.34 x 10-3 limiting reagent ethyl iodide 0.3mL 155.97 3.75 x 10-3 1.6 equiv ’s sodium ethoxide 2.6mL 68.05 3.3 x 10-2 catalyst‚ reaction solvent crude product obtained: phenacetin 0.32g
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utilizes reaction(s) characteristic of a given chemical species and interprets the obtained results using a deductive thought process. Qualitative analysis of cations requires an extensive knowledge of various aspects of chemistry including acid-base equilibria‚ complex ion equilibria‚ solubility‚ etc. However‚ in the deductive process‚ common sense and logic can be as helpful as a knowledge of the chemistry involved. In this lab you will be working with a solution containing a mixture of cations
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| | 1 | 2 | 3 | Final Volume/cm³ (±0.1cm³) | 27.5 | 27.3 | 27.4 | Initial Volume/cm³ (±0.1cm³) | 0.0 | 0.0 | 0.0 | Volume of acid required/cm³ (±0.2cm³) | 27.5 | 27.3 | 27.4 | Colours of solutions: acid‚ base‚ and phenolphthalein were all initially colourless. The base turned dark pink when phenolphthalein was added to it. Add the end point the trials were colourless. Table showing titration of CH3COOH unknown concentration against NaOH Burette Reading/cm³±0.1cm³ | Trial | |
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________________________ Internal Assessment Criteria Aspect 1 Aspect 2 Aspect 3 Total DCP CE Aim: The aim of this practical is to plot and investigate the pH titration curves for the titration of a strong acid with a strong base and of a weak acid with a strong base‚ and find Ka of the weak acid. Procedure: Part I 1. Pour 30 ml of the HCl solution of unknown concentration in a 100 ml beaker. 2. Add a stirring magnet. 3. Place the beaker on the magnetic heater and activate the rotating motor
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Preparation of Sodium Chloride through titration Abstract: acid-base titration is a technique commonly used to determine the moles of acid in a sample by adding a known volume of strong base of a known concentration. The strong base provides the hydroxide ion‚ to react quantitatively with the acid. The point at which the acid is completely and exactly consumed the known quantity of base is called the equivalence end point and is signalled by a colour change in the solution (end point). This colour
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