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Cleveland State University Experiment # 7 “Studying the pH of Strong Acid, Weak Acid, Salt and Buffer Solutions” Mohammed Muntaser Mahmoud Najjar Bryan Saiski Andrea Rivera R.Lama General Chemistry II Lab 267: Section # 2 Date: March 29, 2011
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Muntaser 1 INTRODUCTION: The main theory behind this experiment is that by measuring the -Equations: Equation 1: A=2.00-log(%T) Equation 2: A=[FeSCN 2+ ] / ([Fe 3+ ][SCN - ]) Equation 3: A= log( I t / I o ) Equation 6: Beer Lambert Law / -Objective: The goal of this experiment is to compare calculated and measured pHs of a series of hydrochloric acid and acetic acid solutions. The acid dissociation constant of acetic acid can be calculated based on the pH measurements. By measuring the pH of the various salt solutions, the hydrolysis constants of ammonium chloride can be calculated. After these procedures are completed, the measurements and calculations of the pHs of the same buffer solution mixed with HCl solution and mixed with the NaOH solution, distilled water, and distilled water mixed with HCl solution and mixed with NaOH solution can be compared. Materials & Equipment -2 solutions -10mL and 50mL graduated cylinder -stirring rod -Several test tubes - Spectrophotometer -test tube stand -Distilled water. -Bottle water -beaker -Pipet. -Curvet -gloves - Goggles -paper towel -flask PROCEDURE:
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This note was uploaded on 03/28/2011 for the course CHEM 101 taught by Professor Mundell during the Spring '07 term at Cleveland State.

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