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CHEM 1125Q Chapter Notes - Chapter 11: Semipermeable Membrane, Starch, Ebullioscopic Constant

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peachhippopotamus235

29 Mar 2017

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Solutions are defined as homogeneous mixtures of two or more substances. Often, one component of a solution is present at a significantly greater concentration, in which case it is called the solvent. The other components of the solution present in relatively lesser concentrations are called solutes. The subscript aq in the equation signifies that those molecules are solutes and are therefore individually dispersed throughout the aqueous solution (water is the solvent). Water is used so often as a solvent that the word solution has come to imply an aqueous solution to many people. However, almost any gas, liquid, or solid can act as a solvent. Many alloys are solid solutions of one metal dissolved in another. They are homogeneous; that is, after a solution is mixed, it has the same composition at all points throughout (its composition is uniform). The physical state of a solution, solid, liquid, or gas, is typically the same as that of the solvent.

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Related Questions

Experiment 10 Colligative Properties Introduction A pinch of wa make boiling water hotter. A handful will clear the snow from your steps. Every day we the physical properties of materials around us, but often don't know why we use these particular s or what chemistry is involved. Modifying the temperature of phase changes, by adding a second chemical to the pure solvent are examples of manipulating the Colligative Properties of a solution. this lab, we will study how varying the concentration and type of a salt affects the point of a solution. Colligative properties are properties of a solution containing 2 or more components. Typically, the primary is the solvent and the other called the such as color or hardness, properties depend on the number of particles of astute in the not the identity of the In many cases, the rokute will determine the number of solute particles (degree of ionization, solubility, etc,) in the solvent, but a colligative property does not depend upon the nature of the particles. Two colligative properties commonly encountered are boiling point elevation and freezing point depression (the temperature of of a is lower than of pure solvent). We will be studying boiling point elevation in this Most of the previous work that you have done with solutions has involved units of molarity, M, or moles of solute per liter of solution. Boiling point elevation calculations (as well as those for freezing point depression) or moles of solute per kilogram of solvent. boili change of temperature. When the temperature of a solution changes, the volume of the solution also changes. Since molarity depends on a change in wil the solution's molarity. Molality depends on the mass of the solvent. and thus is independent of temperature. n't Hoff Factor salt into and the of moles inorganic salts in an aque the based on the addition of the number dissociates, the total number of particles in the solution will be of cations and anions produced from the dissociation. Thus; Nacion Na Choaa (2moles of particles) Cacbrs Ca +2ch (3moles of particles) The quantity of particles produced per mole of solute is called the van'tHoff factor and is given the symbol, i, If 1 mole of sodium chloride were completely dissociated, iwould be 2. This theory works very well for dilute solutions and non-electrolytes (i 1, no dissociation at all since nonelectrolytes not ionize), For does not always apply to more concentrated solutions. Thus, when there are a large number of particles in a solution, they have a tendency to recombine as the salt and you don't get 100% dissociation. example, at a NaCl concentration of 0.1M, iwill be 1.81 (90% dissociation) rather than 2 (100%). Boiling Point Elevation solute causes the solution to boil at a higher When a solution is heated, the presence of a non-volatile point of the pure liquid and the temperature than the pure The difference between the boiling boiling point of the solution is: 169

If you could answer the rest of Question 1 from the 6th and 7th picture and then Question 3 from the 8th and 9th picture

11 Oxidation-Reduction Reactions Introduction We encounter oxi uction reactions every day Examples include the combustion of coal natural gas, oil, and gasoline, the operation of automobile's battery and the sains by a Although there are a variety of oxidation-reduction reactions .when you compare a number of you can some common featu Each these of simultaneous oxidation and reduction because electrons are lost by one atom and gained by another one. Moreover, the reactants include an agent and a reducing agent always lost agent and gained by the oxidizing agent (Ebbing/Gammon, Section 4.5) Purpose You will begin by preparing aqueous solutions of three halogens: Cl2, Bra, and Iz. You will prepare these substances in solution from stoichiometric quantities of certain oxidizing and agents. By observing the effect ofthese halogens on the corresponding halides (CI,Br, and you will be able the halogens according to their oxidizing strengths and the halides according to their reducing strengths. Your subsequent observations on the reactions of two halides, Br and I with two common oxidizing agents will enable you to rank the latter according to their oxidizing strengths. You will also find that the products obtained from an oxidation-reduction reaction in an acidic solution can differ markedly from those obtained in a basic solution. Finally, and most important, you will write a balanced equation for each reaction that you have observed The Halogens and the Halides You will deal with halogens and halides in each part ofthis experiment. A brief description of some of their properties will enable you to understand some of your observations more easily. The halogens are found in Group VIIA of the periodic table. The members of this group are fluorine (F) chlorine (CI, bromine (B), iodine (i) and astatine these elements belong to the same 12, group, have many similar properties. For example, their elemental diatomic (F2.cl. Br2, they Atal, and each of them is an oxidizing agent. This experiment uses only Cl, Bra, and Iz, however, because F is such a strong oxidizing agent that special conditions are required for its study and because astatine is radioactive. Aqueous solutions ofcl, be prepared either by dissolving these elements in water or by generating them in Br, reactions. Aqueous solutions of these halogens are solution as products of certain oxidation-reduction respectively. Each called chlorine water, brominee and iodine thickness solution. has its own characteristic color, depending on the concentration and red-brown to water is colorless to yellow; bromine water is yellow to red-brown; and iodine water is brown These halogens are also soluble in cyclohexane (C6H12, a substance that is itselfinsoluble in water. layer When cyclohexane is added to an aqueous solution of a halogen, two layers are formed. The upper is cyclohexane, because it is insoluble and less dense than water. A portion of the halogen passes from the aqueous layer to the upper cyclohexane layer (a process called extraction). A characteristic color is then imparted to this layer. The color ofa halogen in cyclohexane differs somewhat from its color in an aqueous solution, as you will discover during the experiment. be scanned, copied or duplicated or possed toa publicly accessible webwie, iawhole or in Cengage Leaming All Rights Resened c 2013

Exp 25. pH Measurements-Buffers and Their Properties.

I need help in the calculations for part C finding the pKa in 1,2, and 3. Thanks!

Experiment 25 pH Measurements- Buffers and Their Properties ne of the is its concentration of hydrogen ion. The pecies, on they, the H,O ion) has a great effect on the solubility of many isorganic and ora tions. It is important H ion (or. more more important properties of an aqueous solution conplex metallic cations found in solutions, and on the rates of many chemical reac- of hydrogen ion and understand its effect on solution propertics that we know how to measure the concentration For convenience, the concentration of H" as molarity. The frequendly ex ãion is frequently expressed as the pH of the solution rather than pH of a solution is defined by the following equation: the equation, 4. If the [H to the base 10. If (H'l is 1 x 104 moles per liter, the pH of the solution is, by is 10-? M, the pH is 1.3. tion will always be obeyed: described in terms of pH. In aqueous solutions the following equilibrium rela- In distillecd water [H Soler t lequals IOH 1. so, by Equation 2, IH"] must be I X 10 M. Therefore,the pH of distilled will have a pH 7; if H 1 IOH1. the solution is basic and its pH >7. A solution with a pÅ of 10 will have or 1 Ã 10-4 M. We measure the pH of a solution experimentally in two ways. In the first of these we use a chemical an indicator, which is sensitive to pH. These substances have colors that change over a relatively short two pH units) and can, when properly chosen, be used to determine roughly the pH of a solu- called H range on. Two very common indicators are litmus, usually used on paper, and phenolphthalein, the most common indicator in acid-base titrations. Litmus changes from red to blue as the pH of a solution goes from about 6 to about 8. Phenolphthalein changes from colorless to red as the pH goes from 8 to 10. A given indicator is useful for determining pH only in the region in which it changes color. Indicators are available for measure- ment of pH in all the important ranges of acidity and basicity. By matching the color of a suitable indicator in a solution of known pH with that in an unknown solution, one can determine the pH of the unknown to within about 0.3 pH units. The other method for finding pH is with a device called a pH meter. In this device two electrodes, one of which is sensitive to [H'], are immersed in a solution. The potential between the two electrodes is related to the pH. The pH meter is designed so that the scale will directly furnish the pH of the solution. A pH meter gives much more precise measurement of pH than does a typical indicator and is ordinarily used when an accurate determination of pH is needed Some acids and bases undergo substantial ionization in water, and are called strong because of their essentially complete ionization in reasonably dilute solutions. Other acids and bases, because of incomplete ionization (often far less than even 1% in 0.1 M solution), are called weak Hydrochloric acid, HCl, and sodium hydroxide, NaOH, are typical examples of a strong acid and a strong base. Acetic acid, HCH,0, and ammonia, NH, are classic examples of a weak acid and a weak base. A weak acid will ionize according to the Law of Chemical Equilibrium HB(aq)H'(a) B (aq) 3)