Lab Report Electrical Conductivity Introduction There are some substances that are capable of conducting electricity‚ and the reason they conduct electricity is because of the type of compound the substance is. Electrolytes or any ionic compound conduct electricity and nonelectrolytes do not conduct electricity. An Ionic compound is formed from the electrical attraction between anions and cations‚ typically a metal with a non-metal‚ except hydrogen. When an ionic compound forms‚ the anion
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Thermal Conductivity of Metals and Non-metals 1. Introduction Thermal conductivity is a physical property of materials of great importance. Unlike some physical properties‚ however‚ thermal conductivity cannot be directly measured. In order to determine a material’s thermal conductivity‚ intermediate quantities must be determined from which the conductivity may be ultimately calculated. The objective of this lab was to determine the thermal conductivity of metals. To do so‚ it was necessary to study
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CHEMICAL EFFECTS OF ELECTRIC CURRENT Conductivity of Liquid Electrolysis Electroplating www.excellup.com ©2009 send your queries to enquiry@excellup.com Finish Line & Beyond The materials‚ which allow electric current to pass through them‚ are good conductors of electricity. On the other hand‚ materials‚ which do not allow electric current to pass through them easily‚ are poor conductors of electricity. You know that metals such as copper and aluminum conduct electricity whereas materials
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11/29/2012 Lab # 11 – Acid - Base Titration Introduction: The purpose of this lab is to determine the molarity (M) of an unknown HCl solution. A NaOH solution will be made and its molarity calculated. A sample of the NaOH solution will be titrated against the unknown HCl solution to calculated the volume needed to neutralize it. With these volumes the unknown molarity can be calculated. Theory: Solutions are made up of solvents and solutes. Materials known as acids when
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H3PO4 titration curve 4 2.3 H2A titration curve 5 3. Calculations 3.1 HC2H3O2 Calculations a. Exact molarity of the HC2H3O2 solution 6 b. Ka from the initial pH 6 c. Ka from the pH at halfway point 6 d. Ka from the pH at the end point 7 3.2 H3PO4 Calculations a. Exact molarity of the H3PO4 solution 7 b. Ka1 from the initial pH 7 c. Ka1 from the pH at the first halfway point 8 d. Ka2 from the pH
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Title : Preparation of a standard solution Aim To prepare a standard solution of potassium hydrogenphthalate which will later be used to standardize sodium hydroxide solution‚ NaOH. Research question How does different molarity of potassium hydrogen phthalate solution which is prepared by dilution process influence the volume of sodium hydroxide‚ NaOH used during titration process until the colourless phenolphthalein indicator solution turns pink where the volume of potassium hydrogenphthalate used
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Questions: 1. Why is a conical flask‚ rather than a beaker‚ used in the experiment? – To allow easy mixing of solutions by swirling. 2. Why is the funnel removed from the burette after adding the acid solution? – so that the drops from the funnel will not fall into the burette. 3. In using a burette‚ why is it important to (a) rinse it with a little of the solution it is going to contain? – to remove any residual water and so avoid dilution of the acid solution when it is poured into the burette
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Experiment 5- Standardization of NaOH and determination of Molarity of an unknown Acid Objectives 1. Preparation and standardization of a 0.1M NaOH solution 2. To learn the technique of titration 3. Determination of the concentration of an unknown diprotic acid. Introduction Titration can be traced to the origins of volumetric analysis‚ which began in the late eighteenth century. Study of analytical chemistry began in France and the first burette was made by Francois Antoine Henri
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Salle University-Dasmarinas Dasmarinas‚ Cavite Philippines Abstract ____________________________________________________________ ________________ The electrical conductivity of electrolytes and non-electrolytes activity demonstrated the physical propertiesand the conductivity of some solution. Electrical conductivity apparatusare dipped into a liquid in a beaker. Whenthe liquid contains significant concentrations of ions‚ the ions more between the electrodes to complete the circuit(which
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1.2 Exercise 2 - solutions Using molarities and concentrations 1. Calculate the number of moles of H2SO4 in 50 cm3 of a 0.50 moldm-3 solution. 2. Calculate the number of moles of FeSO4 in 25 cm3 of a 0.2 moldm-3 solution. 3. Calculate the mass of KMnO4 in 25 cm3 of a 0.02 moldm-3 solution. 4. Calculate the mass of Pb(NO3)2 in 30 cm3 of a 0.1 moldm-3 solution. 5. What is the molarity of 1.06g of H2SO4 in 250 cm3 of solution? 6. What is the molarity of 15.0 g of CuSO4.5H2O in 250 cm3 of solution
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