Billy Kong Chem&163 Lab Report 1 Analysis of Acids‚ Bases‚ pH and Salt Purpose: Explore various methods for determining the characteristics of acid/base solution. The goal of this experiment include the investigation of various acid/base indicators‚ calculating the change of pH with concentration‚ change of pH due to the addition of salt and different between strong and weak acids/bases. Safety and Disposal: Use extreme caution when handling concentrated acids and bases. Dispose of all
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flask and add about one spatula of solid calcium hydroxide. Stopper the flask and shake well for one minute. Leave to stand for at least 24 hours. Titrate 10cm3 samples against 0.05 mol dm-3 hydrochloric acid solution using methyl orange as an indicator. Obtain enough results to calculate an accurate average‚ and then calculate the number of moles of calcium hydroxide solution in 1 dm3 of solution. RAW DATA Titration number | Final volume Ca(OH)2 (cm3) ±0.1ml | Initial volume Ca(OH)2 (cm3)
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CH 125 INORGANIC CHEMISTRY FOR MICROBIOLOGY Laboratory Manual 2013 Edition By Brian Clark‚ Marco Castillo & Patrick Chan CENTENNIAL COLLEGE OF APPLIED ARTS & TECHNOLOGY‚ SCARBOROUGH‚ ONTARIO Preliminary Laboratory Information - CH 125 The following safety information is provided to the student in order to ensure that all students and college staff working in the laboratory are aware of common industrial laboratory safety practices. Laboratory
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or base1. Titration starts with a beaker or Erlenmeyer flask containing a very precise volume of the known concentration solution and a small amount of indicator‚ which is put underneath a burette containing the solution with unknown concentration1. Small drops of the titrant are then added to the known solution and indicator until the indicator changes which means the endpoint has been reached. Single drops of the titrant can sometimes make a permanent or temporary change in the indicator2.
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Name: _____________________ Date: _____________ Student Exploration: pH Analysis Vocabulary: acid‚ acidic‚ alkaline‚ base‚ indicator‚ neutral‚ pH Prior Knowledge Questions (Do these BEFORE using the Gizmo.) 1. Acids are substances that produce hydrogen ions (H+) when dissolved in water. Lemon juice is an example of an acid. A. What does lemon juice taste like? __Sour.______________________________ B. What does it feel like if lemon juice gets in your eye? ___It
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Oxidation Reduction Titrations: The Indirect Iodimetric Analysis Ascorbic Acid Unknown Number 69 I: Purpose: To determine the percent weight of Ascorbic Acid in unknown sample. This was to be done by the means of an indirect iodimetric analysis. In an iodometric analysis‚ the oxidizing agent can be determined by a different means than titrating directly with standard iodide‚ because a high concentration of I- is needed to form the I3- complex. In this type of analysis‚ excess iodide is added to
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THE UNIVERSITY OF THE WEST INDIES □ Supplemental/Summer School □ Examinations of December /April/May □ /July □ 2009 Originating Campus: Cave Hill □ Mona St. Augustine □ Mode: On Campus By Distance □ Semester l Semester II Course Code and Title: CHEM1901 - INTRODUCTORY CHEMISTRY A Date: Duration: Time: 2 Hours. Paper No: 1 Materials required: Answer booklet: Calculator: (where applicable) Multiple Choice answer sheets: Programmable □ □ numerical
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Flask #1 7.8 Dark pink‚ fast change Flask #2 7.85 Light pink‚ fast change Flask #3 7.9 Light pink‚ slow change Mean Volume NaOH: 7.85 mL SD: 0.05 RSD: 0.64% Standardization of 0.1M NaOH Quantity of KHP added to 100mL H20‚ Phenolphthalein indicator then titrated
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put into the flask. Water was then added to the same flask. Then phenolphthalein indicator solution was added before we began titrating by adding more drops of the NaOH solution while swirling the flask until a pink color remained. The liquid levels were recorded on both burets. Part B: Solid unknown acid was added to a flask with water and swirled until almost fully dissolved. Then phenolphthalein indicator was added. With standardized NaOH solution we titrated and recorded the initial and
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chemistry. This reaction is also widely known as neutralization. In this experiment‚ we used titration technique which involves accurately measuring the volume of a solution required to react with another reagent. An indicator must be used to determine the end point of the titration. The indicator used can change colors at different pH values. OBJECTIVE To determine the concentration of sulphuric acid (H2SO4) using titration technique CHEMICALS NaOH solution‚ approximately 0.2 M‚ dilute sulphuric
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