Ethanoic Acid Lab Report

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Aim: The purpose of the experiment is to prepare solutions and buffers according to different volumes, different concentrations and measure their pH values.

Introduction: Acids are chemical compounds that release hydrogen ions when dissolved on the water. A strong acid is any acid that can be ionize completely in solutions. This implies it gives the highest number of hydrogen ions or protons when positioned in a solution. Ions are charged particles. When the concentration of hydrogen ions is higher, there is lower pH. Strong acids are fully ionized however weak acids are just partly ionized in a solution. As an example, ethanoic acid is a weak acid but hydrochloric acid is a strong one. Bases produce hydroxide ions in an aqueous solution. Strong bases dissolve 100% into the cation and OH- . The hydroxides of the Group I and II metals generally are can be accepted strong bases. These bases fully dissolve in solutions of 0.01 M or less. On the other hand, a weak acid is an acid that give off only some of its hydrogen atoms into the solution, dissolves partially. pH is a numeric scale that represents the acidity or basicity of a solution. A pH scale consist of numbers from 1 to 14. Seven represents the middle (neutral) point. Numbers below 7
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With the formula of C1xV1 = C2xV2, 30 ml of NaCl solution required and from the equation of molarite = mol / liter (5=n / 0.05) 0.25 mols of solid NaCl taken for the experiment. 1 mol NaCl equals to 58.44 grams so 0.25 mol NaCl equals to 14.75 grams. But we could have taken 14.79 NaCl. As a first step, 0.25 mol of NaCl was combined with 30 ml of water, then 20 ml of water was added. There are two process for the adding water because if we put water in one step, the total volume could be affected and it could have been higher than 50. Then, magnetic stirrer was used for mixed the 5M 50 ml NaCl, and 20 ml distilled water was added on

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