Depression of Aqueous Solutions Abstract: The purpose of this lab was to find the freezing point depression of 0.5M aqueous solution NaCl‚ distilled water‚ 0.5M aqueous solution of CaCl2‚ and unknown solution A. However‚ the teacher gave us values to do our experiment. Introduction: The objective of this lab is to understand how a solute depresses the freezing point of a solvent; also to comprehend the process of super cooling and to measure the freezing point of solutions and solvents
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4.1 & 4.2: General properties of aqueous solutions and Precipitation Reactions: 1. (Brown 4.11) When asked what causes electrolyte solutions to conduct electricity‚ a student responds that it is due to the movement of electrons through the solution. Is the student correct? If not‚ what is the correct response? 2. (Brown 4.15) Specify what ions are present in solution upon dissolving each of the following in water: a. ZnCl2 c. (NH4)2SO4 b. HNO3 d. Ca(OH)2 3. (Brown 4.16 ) Specify
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The Ionic Lattice In most ionic compounds‚ the anions are much larger than the cations‚ and it is the anions which form the crystal array. The smaller cations reside in the holes between the anions. Basic Concepts: 1. Ions are assumed to be charged‚ incompressible‚ nonpolarizable spheres. 2. Ions try to surround themselves with as many ions of opposite charge as closely as possible. Usually in the packing arrangement‚ the cation is just large enough to allow te anions to surround it without
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Chemistry December 14‚ 2010 Conductivity of Ionic solutions Introduction This lab report is about the conductivity of ionic solutions. In class we have been discussing wether all ionic solutions conduct equally well. If an solvent solution conducts electricity‚ then it must contain ions. So measuring the conductance of solutions can tell you whether the solutes in the solution are dissociated into ions. (Conductivity) Any type of solution‚ even ionic solutions‚ provide resistance to the flow of current
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Purpose: To observe the reactions of specific aqueous solutions with specific aqueous reagents. Introduction: A solution is as a homogeneous mixture containing two or more substances. Reagents are added to solutions to create a chemical reaction or added to see if anything occurs. Reagents can be added to solutions to see if there is a presence of other substances. For example‚ iodine added to a lead solution. Iodine would be the reagent and would cause a chemical reaction confirming the presence
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Chapter 1: Introduction Chapter 1: Introduction Ionic liquids (ILs) can be viewed as a new and remarkable class of solvent. They are also a type of materials that have a long and useful history‚ where the earliest material that meets the current definition of IL was observed in the mid-19th century when a separate liquid phase called the “red oil” was observed in Friedel-Crafts reaction [17]. Over the following years‚ there has been a rapid growing of interest in ILs due to the realization
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1114) CHEMICAL BONDING MOKAN A/L VELAN (SCPNG0000019030) SANDEEP SINGH JASPREET SINGH TABLE OF CONTENT Contents IONIC BOND 2 METALLIC BOND 9 The "Sea of Electrons" Theory 14 Conductors‚ Insulators and Semiconductors 16 25 IONIC BOND Ionic bond is formed when electron transferred from a valence shell of an atom to the valence shell of another atom. Ionic bond involves electron transfer across two atoms. The atom which donates the electron is called cation which is a positive
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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 equations‚ and to write net ionic equations for
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Abstract: When ionic compounds are dissolved in water‚ they break apart into ions. In this lab the opportunity to mix two ionic solutions and observe the results was given. Some ions will remain dissolved and uncombined in the solution even when they are mixed with other ions. When other ions are mixed‚ they form compounds that appear as cloudy or grainy precipitates. The objective of this lab was to observe the formation of compounds and to write the names and formulas of ionic compounds. It is
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Ionic compounds are formed when a metal and a non-metal join together. When sodium metal is dropped into a gas jar of chlorine gas the elements react violently to form a new compound called sodium chloride joined by ionic bonds. To understand how this process works‚ we must grasp an understanding of what an ion is and what an ionic bond is. An ion is an atom that has an electric charge and is created when an atom (or a group) gain or loses electrons. (It has an electric charge due to the imbalance
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