Solutions Solubility. Chapter 14

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1 Copyright 2004 by Houghton Mifflin Company. Solutions Chapter 14 All rights reserved. 1 Solutions Solutions are homogeneous mixtures Solvent substance present in the largest amount Solute is the dissolved substance Aqueous solutions solvent is water Alloys solutions that contain metal solutes and solvent 2 When ionic compounds dissolve in water they dissociate into ions solvated - when solute particles are surrounded by solvent molecules hydrated - ions become surrounded by water molecules 3

2 4 Covalent molecules that are small and have polar groups tend to be soluble in water The ability to H-bond with water enhances solubility Would you expect each of the following to dissolve in water? Sucrose: Typical petroleum molecule: 5 When one substance (solute) dissolves in another (solvent) it is said to be soluble Salt is soluble in water Bromine is soluble in methylene chloride When one substance does not dissolve in another they are said to be insoluble Oil is insoluble in Water There is usually a limit to the solubility of one substance in another Gases are always soluble in each other Some liquids are always mutually soluble 6

3 7 Molecules that are similar in structure tend to form solutions Like dissolves like The solubility of the solute in the solvent depends on the temperature Liquids: increased solubility at higher temps Gases: decreased solubility at higher temps The solubility of gases depends on the pressure Higher pressure = Larger solubility 14.2 Solution Composition A concentrated sol n has a high proportion of solute to sol n A dilute sol n has a low proportion of solute to sol n A saturated solution has the maximum amount of solute that will dissolve in the solvent Depends on temp An unsaturated sol n has less than the saturation limit A supersaturated sol n has more than the saturation limit Unstable Solution Composition Solutions have variable composition To describe a solution accurately, you need to describe the components and their relative amounts Concentration = amount of solute in a given amount of solution 9

4 Mass Percent mass solute Mass % = mass solution x 100 % = grams of solute per 100 g of solution 5.0% NaCl has 5.0 g of NaCl in every 100 g of solution Mass of Solution = Mass of Solute + Mass of Solvent 14.3 Mass Percent mass solute Mass % = mass solution x 100 What is the percent of calcium chloride in a solution made by mixing 2.50 g of the salt with 50.0 g of water? Molarity moles of solute per 1 liter of solution M = molarity = moles of solute L of solution = mol L Calculate the molarity of a solution prepared by dissolving 2.80 g of solid magnesium chloride in enough water to make 135 ml of solution describes how sol n was made, not how it exists moles MgCl 2 added to make 135 ml sol n M Mg 2+ and M Cl - 12

5 Molarity M = molarity = moles of solute L of solution = mol L Calculate the mass of solute needed to make ml of M iron(iii) chloride solution 14.4 Molarity Standard solution: a sol n whose concentration is accurately known Dilution Dilution is adding solvent to decrease the concentration of a solution The amount of solute stays the same, but the concentration decreases M 1 x V 1 = M 2 x V 2 15

6 Solution Stoichiometry M x V = n Calculate the mass of sodium chloride required to precipitate all the silver(i) ions from 1.50 L of a M AgNO 3 sol n 14.6 Solution Stoichiometry What volume of M sodium hydroxide must be used to precipitate all of the copper(ii) ions in 43.1 ml of a M copper(ii) nitrate solution? 17 Acid-Base reactions Titration: used to determine the concentration of an unknown acid or base add just enough acid solution to neutralize a known volume of a base solution or visa versa requires an indicator a substance that is a different color in acid or in base 18

7 19 Titration Indicator: potassium hydrogenphthalate (KHP) KHC 8 H 4 O 4 pink in acid, colorless as a base acid KHP + base Titration: Ê ( ml) 10-3 L ˆ Ê mol Á Á Ë ml Ë L H 3 O M HCl V initial =23.89 ml H 3 O + + OH - 2 H 2 O ˆ Ê 1 mol OH - ˆ Ê 1 ˆ Ê ml ˆ Á Á Á = M44 M OH - Ë 1 mol H 3 O + Ë ml Ë 10-3 L V final =35.11 ml KHP ml NaOH 20 What is the concentration of an acetic acid solution, if ml of it requires ml of M sodium hydroxide? 21

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