Introduction to Chemistry Laboratory: A Lesson on Tools‚ Techniques and Measurements PURPOSE: The purpose of this set of experiments (3 total) is to become familiar with the common types of laboratory glassware and equipment‚ and how to obtain and analyze data from these items. LEARNING OBJECTIVES: By the end of this experiment‚ the student should be able to demonstrate the following proficiencies: 1. Know which glassware (beakers‚ burettes‚ pipettes‚ graduated cylinders‚ flasks‚ etc) should
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CHEM 17 Expt.2-Coupled Reactions 4/18/12 Results and Discussions: One way to obtain products from a non-spontaneous process that is exhibited in this experiment is by “coupling” two reactions. The principle of Coupled Reactions is based on a simple concept: we can use a thermodynamically favorable (spontaneous) reaction to drive an unfavorable one. One step is allowed to supply enough free energy for the other to occur. A coupled reaction is a system wherein a non-spontaneous
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Experiment 5 COMMON ION EFFECT MALUBAY‚ Justin Damian PADRILLAN‚ Hazel Rose CD2‚ Group 5 Ms. Sarah Sibug 6 April 2013 ------------------------------------------------- ------------------------------------------------- I. ABSTRACT The common ion effect occurs when a given ion is added to an equilibrium mixture that already contains that ion‚ and the position of equilibrium shifts away from forming more of it. This paper is a follow-up of the experiment which aims to determine the common-ion effect
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CHEMISTRY 17 1ST LONG EXAM REVIEWER I. ELECTRONIC STRUCTURE OF ATOMS -arrangement of atoms’ electrons -the number of electrons in an atom -distribution of electrons around the nucleus and their energies • ATOMS *Billiard Ball Model (JOHN DALTON) *Plum Pudding Model (JOSEPH J. THOMPSON) *RUTHERFORD’s Model of Atom -atoms are tiny‚ hard‚ indivisible spheres -electrons (negative charge) occupy the atom - Atom is mostly empty space with a dense nucleus • PROBLEMS with Rutherford’s Model
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Acidic vs. Alkaline Introduction: Potential of hydrogen‚ or pH‚ is a scale used to express the acidity or alkalinity of a solution. The scale ranges from 0 to 14‚ below seven represents acidity‚ seven is neutral‚ and more than seven is basic. Acid-base indicators show whether the solution is acidic or alkaline. They do this by reacting with the solution‚ seen as a color change‚ as the concentration of hydrogen (H+) or hydroxide (OH-) ions changes in an aqueous solution. Different indicators
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EXPERIMENT 1: Proteins -polypeptides compose of > 50 amino acids Functions 1. Enzymes or subunits of enzymes-enhancing the rates of reactions 2. Structural or Mechanical roles 3. Immune response roles 4. Storage and transport of substances 5. Source of amino acids for organisms that cannot synthesize amino acids naturally ISOLATION- disruption of cell membranes to release cell contents; separation for other contaminants 1. CENTRIFUGATION 2. SALTING OUT-water
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INTERNATIONAL BACCALAURÉAT BACHILLERATO c BACCALAUREATE INTERNATIONAL INTERNACIONAL MARKSCHEME May 2002 CHEMISTRY Standard Level Paper 3 12 pages M02/420/S(3)M+ –5– Subject Details: M02/420/S(3)M+ Chemistry SL Paper 3 Markscheme General ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! ! Each marking point is usually shown on a separate line or lines. Alternative answers are separated by a slash (/) – this means that either answer is acceptable. Words underlined are essential for the mark. Material
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Vanden Eynden CHM2510 AU13 Practice Midterm Exam #2 CHM2510 Practice Midterm Exam #2 This exam is designed to give you a small glimpse as to the format of the exams I write. The content of the exam has no direct correlation to the difficulty of the actual exam you will take. Use this exam as another problem set so you can get a little more practice in where multiple chapters are combined into one document. It would greatly benefit you to try doing this exam first WITHOUT ANY NOTES
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XV. GIMNAZIJA International Baccalaureate Department Group 4 – Chemistry SL Lab no.2: Acid-base titration Student: Caterina Rende Dominis Teacher: Zrinka Toplićan Date: 19 November 2012 Data Collection and Processing (DCP) Aspect 1: Recording raw data Table 1 Table showing raw data collected from titration Known measurements 25 mL of diluted acid 0‚100 M of NaOH solution Measurement Number | V of alkali needed to neutralize acid /mL/ (±0.01 mL)
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Spectrophotometric determination of the equilibrium constant of a reaction K.F.P. Boado Department of Chemical Engineering‚ College of Engineering University of the Philippines‚ Diliman‚ Quezon City‚ Philippines 4 March 2015 Jade Nazareno ABSTRACT The experiment aims to determine the Keq of the formation of Fe(SCN)2+ through the use of UV-Vis spectrophotometry. The solutions used in the study were allowed to equilibrate days before calibration in a UV-Vis spectrophotometer which determined the absorbance
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