Objectives: The purpose of this lab is to observe the reaction of crystal violet and sodium hydroxide by looking at the relationship between concentration and time elapsed of the crystal violet. CV+ + OH- CVOH To quantitatively observe this reaction of crystal violet, the rate law is used. The rate law tells us that the rate is equal to a rate constant (k) multiplied by the concentration of crystal violet to the power of its reaction order ([CV+]p) and the concentration of hydroxide to the power of its reaction order ([OH-]q). Rate = k[CV+]p[OH-]q To fully understand the rate law, concentrations of the substances must be looked at first. The concentration is measured in molarity.
William Flores-Paz Monitoring Acid-Base Titrations with a pH meter October 30, 2013 Introduction The purpose of this experiment was to record the volume of HCl and acetic acid with a NaOH with a known molarity. This data would allow us to create a graph so we could compare the two titration curves. We would then use these curves to calculate the unknown molarities. HCl + NaOH >H2O + NaCl This equation shows the relationship between the acid and the base then the reaction goes forward and they are titrated creating salt and water. This particular reaction is a strong acid and a strong base which means that when the reaction reaches the equivalence point, the moles of the acid and the base are equal and the solution is neutral so the pH should be around 7.0 depending on the final volume of each solution.
EXTRACTION: DETERMINATION OF ITS EFFICIENCY AND CALCULATION OF THE DISTRIBUTION COEFFICIENT Group#4: Wassim Abdel Naby and Bianca Francisco Bachelor of Science degree in Chemistry De La Salle University ABSTRACT The objective of this experiment is to demonstrate the concepts of extraction and to calculate the distribution coefficient. In the process of extraction, amount of acetic acid was the one to be determined, and this was done through the process of titration, indicator used was phenolphthalein and the titrant used was Sodium hydroxide. First, 20 ml aliquot portion of diluted acetic acid in a 125 mL Erlenmeyer flask titrated with Sodium hydroxide. Next, the second flask containing another 20 mL of acetic acid extracted by 20 mL portion toluene, this was done twice due to over titration in the first trial. Lastly, the third 20 mL aliquot portion acetic acid underwent the same procedures with flask 2 but this time with two 10 mL portions of toluene.
And limiting reagent which is the reactant that is completely consumed when a reaction is run to completion. III. Summary of Procedure In this lab the first procedure was to measure the initial temperature of NaOCl and of Na2S2O3 and measure it with a thermometer and then record it. The same thermometer is used for measuring both solutions, but the thermometer should be washed with distilled water after the using it in one solution. Afterwards a small amount of NaOCl was added to the graduated cylinder.
Purpose: The purpose of this lab is to investigate whether mass is gained or lost during a chemical reaction. Hypothesis: It will be found out that the mass is neither gained nor lost during a chemical reaction but transferred. Materials: * Safety goggles * Erlenmeyer flask * Balance * Graduated Cylinder * Beaker * Iron (III) chloride solution * Copper (II) sulphate solution * Sodium bicarbonate * Test tubes (small, and large) * Rubber Stopper * Tweezers * Paper towel * Scoopula * Sodium hydroxide solution * Hydrochloric acid Procedure: 1. 5ml of iron (III) chloride was measured and placed in the Erlenmeyer flask. 2.
The piece of metal is then taken out of the boiling water and placed in a calorimeter which contains room temperature water. The heat that was absorbed by the metal is measured by the temperature change the metal causes in the room temperature water. James Joule was one of the first to determine the mechanical equivalent of heat. He did this in the 1870s using a calorimeter of his own invention. The energy (or heat) unit of the Joule was named after him.
The balanced equations for this reaction shows that the molar ratio of magnesium reacted to hydrogen gas produced is 1:1. Therefore, by determining the mass of magnesium that reacts and the number of moles that this mass is equal to, you will also be able to determine the number of moles of hydrogen gas produced. The volume of hydrogen gas produced will be measured directly on the scale of a gas-measuring tube. The gas laws of Boyle and Charles will be used to correct this volume, measured under laboratory conditions, to the volume the sample of gas would occupy at STP. The collected data (number of moles and volumes at STP) will be used to calculate that molar volume of the hydrogen gas.
| Chemistry Coursework | How does the concentration of Hydrochloric Acid affect the rate of reaction between Hydrochloric Acid and Sodium Thiosulfate? | | | Initial Planning The aim of my coursework is to investigate the variables that increase the rate of reaction. There are several equations that can be investigated. The main 3 equations are: 1) Hydrochloric Acid + Marble Chips Calcium Chloride + Water +Carbon Dioxide 2HCl (aq) + CaCO3 (s) CaCl2 (aq) + H2O (l) + CO2 (g) 2) Hydrochloric Acid + Magnesium Magnesium Chloride + Hydrogen 2HCl (aq) + Mg (s) MgCl2 (aq) + H2 (g) 3) Hydrochloric Acid + Sodium Thiosulfate Sodium Chloride + Sulfur Dioxide + Sulfur + Water HCl (aq) + Na2S2O3 (aq) NaCl (aq) + SO2 (g) + S (s) + H2O (l) In equation 1, the CO2 produced is monitored over a certain period of time. The more CO2 produced over this time, the higher the rate of reaction.
HN Chemistry BP Elevation Lab April 23, 2013 II. Introduction A. In this lab, Boling point Elevation was taught. Boiling point elevation is a colligative property that deals with the amount of particles in solution and how fast it boils. When an electrolyte or non electrolyte is introduced the effectiveness of the Boiling point changes.