Solution (Henderson – Hasselbach Equation) [pic] [pic] Buffer Solution after the Addition of Acid or Base [pic] [pic] [pic] [pic] In this experiment‚ the experimenters prepared solutions of HOAc‚ NaHOAc‚ NH3‚ NH4Cl‚ NaOH and HCl.
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Bunsen burner Drying oven or light Beaker tongs 10-ml graduated cylinder Filtering funnel Rinse bottle with deionized water Whatman #1 filter paper 1.8 to 2.2 grams CuSO45H2O 250-ml beaker *10 ml of 6.0 M NaOH solution * For 100 ml of a 6.0 Molar solution of NaOH‚ Using a 100-ml volumetric flask‚ dissolve
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Thermodynamics Lab Introduction: Thermodynamics is the study of energy which can exist in many forms‚ such as heat‚ light‚ chemical energy‚ and electrical energy. The variables that thermodynamics can be used to define include temperature‚ internal energy‚ entropy‚ and pressure. Temperature‚ relating to thermodynamics‚ is the measure of kinetic energy in the particles of a substance. Light is usually linked to absorbance and emission in thermodynamics while pressure‚ linked with volume‚ can do
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Lung Capacity in this lab‚ I learned about lung capacity and CO2 production. Lung capacity simply means the maximum amount of air you can take into your lungs. Lung capacity and CO2 production closely relate to the respiratory system. The respiratory system is the system in which oxygen goes into your body and carbon dioxide comes out; In short it’s breathing. The structures involved in the respiratory system are mouth/nose‚ mucus/cilia‚ pharynx‚ larynx‚ bronchi‚ bronchioles‚ alveoli‚ pleura‚ and
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bases). After ranking the pH of these solutions‚ you will then test your predictions in the laboratory. 1. Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO‚ HCl‚ HCN‚ NaOH‚ NH3‚ NaCN‚ KNO3‚ H2SO4‚ NH4Cl‚ H2SO3‚ NaHCO3‚ Na3PO4 and CH3COOH. In order of increasing pH: H2SO4: This is because the first hydrogen is strong and completely ionizes and the second is weak and ionizes very minutely
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Ocean County College Department of Chemistry Chem 180 Lab 5: Ionic Reactions Submitted by Abstract: The purpose of this experiment is to work with aqueous solutions of ionic substances. Aqueous solutions are those solutions in which water is the solvent. When ionic substances are dissolved in water‚ the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates. The goal of this experiment is to study the nature of ionic reactions‚ write balanced
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Determination of % Composition of Pennies Using Redox and Double Displacement (Precipitation) Reactions Introduction: Oxidation involves the gain of electrons of hydrogen or the loss of oxygen or decrease in oxidation state. If zinc completely reacts with HCL‚ then the theoretical yield of copper should be equivalent to the actual yield. Purpose: In this lab‚ we will determine the percent composition of a modern (post-1982) penny by using a strong acid to react and dissolve the zinc
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IDENTIFICATION OF AMINO ACIDS BY MEANS OF TITRATION CURVE ABSTRACT The aim of the experiment was to identify an unknown amino acid through acid-base titrations which was prepared in water to form an acidic solution. Each group prepared unknown amino acid hydrochloride. The pre-prepared basic solution was slowly added to the amino acid solution and pH change was closely observed using the pH meter. During these titrations the amino acid converted from cation to zwitterion to anion; zwitterion
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reacted with the air‚ and this would decrease the volume of acid which actually mixed with the base‚ resulting in an increased heat of neutralization. A second source of error was that in the experiment where HCl and NaOH were being mixed‚ one drop of NaOH was lost by accident which the NaOH solution was being poured into the calorimeter. This would result in too much acid solution‚ which means that not all of the acid completely reacted with the base. This‚ also‚ would increase the heat of
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p. 1 Megan Ly Chemistry 231L February 20‚ 2013 SOLUBILITY Purpose: To better comprehend solubility behavior by investigating the solubility of various substances in different solvents‚ looking at miscible and immiscible pairs of liquids‚ and observing the solubility of organic acids and bases. Reference:
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