Chemistry
`
`Second edition
`
`ROB LEWIS AND WYNNE EVANS
`
`Page 1 of 4
`
`SENJU EXHIBIT 2099
`LUPIN v. SENJU
`IPR2015-01097
`
`

`
`All rights reserved. No reproduction, copy or transmission of
`this publication may be made without written pemnission.
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`* ©Rob Lewis and Wynne Evans 1997, 2001
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`No paragraph ofthis publication may be reproduced, copied or
`transmitted save with written permission or in accordance with
`the provisions of the Copyright, Designs and Patents Act 1988,
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`The authors have asserted their rights to be identified
`as the authors of this work in accordance with the
`Copyright, Designs and Patents Act 1988.
`
`First edition 1997
`Reprinted twice
`Second edition 2001
`Published by
`PALGRAVE
`Houndmills, Basingstoke, Hampshire RG21 6XS and
`175 Fifth Avenue, New York, N.Y. 10010
`Companies and representatives throughout the world
`
`PALGRAVE is the new global academic imprint of St. Martin's Press LLC
`Scholarly and Reference Division and Palgrave Publishers Ltd (formerly
`Macmillan Press Ltd).
`
`ISBN 0-333-96257-5
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`A catalogue record for this book is available
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`Typeset by Footnote Graphics, Warminster, Wilts
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`Page 2 of 4
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`

`
`Solutions and Solubility
`
`Contents
`
`Objectives
`
`11.1 Solubility
`11.2 Dynamic nature of
`dissolution
`11.3 Solubility of
`sparingly soluble
`ionic compounds
`11.4 Distribution of a
`solute between two
`solvents
`11.5 Solubility of gases
`in water
`11.6 Osmosis
`11.7 Colloids
`
`170
`
`~Examines solvent miscibility and immiscibility·
`
`~Explains the idea of solubility product
`
`176
`
`~Looks at distribution ratios and gas solubility
`
`176
`
`~Discusses osmosis and its applications
`
`~Introduces colloids
`
`182
`
`183
`
`187
`
`190
`
`Solubility
`
`Revision questions 192 A solution is a mixture consisting of a solvent (the 'dissolver') and the solute (the
`substance that is being dissolved). For example, if we dissolve sugar in water,
`water is the solvent, the sugar the solute and the sugary water is the solution. If we
`keep adding sugar to some water, a point will be reached when the water will not be
`able to hold any more sugar. The solution is now said to be saturated. Adding more
`sugar simply results in sugar settling on the bottom of the container. Raising
`temperature of the solution allows the water to hold more sugar before it becomes
`saturated. Many solids, like sugar, are more soluble at higher temperatures, although
`the reverse usually applies to gases, which are less soluble in hot water than in cold
`water.
`
`Rules of solubility
`The word 'polar' was introduced in Unit 5 (see page 7l ). A polar substance is a
`substance that contains ions or consists of polar molecules. A polar solvent is a
`solvent which consists of polar molecules.
`We start by reminding ourselves of the following:
`
`1. If a polar substance dissolves, it dissolves only in polar solvents.
`2. If a non-polar substance dissolves, it dissolves only in non-polar solvents.
`
`These generalizations are summarized in the rule like dissolves like. Solvents may be
`placed in order of polarity by testing their solubility in each other. The order of
`
`Page 3 of 4
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`

`
`11.1 Polarity of common solvents
`in order of
`polarity with heptane the least polar and water
`polar
`
`SOLUBILITY
`
`171
`
`Formula
`
`CH 3(CH 2)5 CH 3
`CH3 (CH2)4CH 3
`C6H12
`CCI 4
`C6H5 CH 3
`C2HsOC2Hs
`CH2CI2
`CH 3CH(OH)CH 3
`C4H80
`CHCI3
`CH 3 CH 20H
`CH 3 COOC2 H5
`CH 3 COCH 3
`CH 3 0H
`CH 3CN
`CH 3 SOCH 3
`H20
`
`Density at
`2s•c;gcm~ 3
`
`. 0.68
`0.66
`0.77
`1.58
`0.86
`0.71
`1.32
`0.78
`0.89
`1.48
`0.79
`0.90
`0.79
`0.79
`0.78
`1.10
`1.00
`
`names: iCarbon tetrachloride, 2Toluene. 3 Diethyl ether, 4 Chloroform.
`alcohol, 6 Ethyl acetate, 7Acetone, 8Methyl alcohol, 9Acetonitrile.
`
`in Table 11.1 was obtained in this way. Of the common solvents, water is the
`polar and the hydrocarbons heptane and hexane the least polar.
`
`when two solvents are mixed, a single layer (consisting of a solution of the two
`) is produced, the solvents are said to be miscible. If two layers are produced
`both layers consist of pure solvent, the liquids are said to be immiscible (Fig. 11.1).
`layers are produced, the solvent with the lowest density floats on the top.
`The word 'layer' is often replaced by the word phase. Thus, a mixture of hexane
`water produces two phases.
`Table 11.2 shows which pairs of common solvents are miscible, with • denoting
`For example, the table shows that water is immiscible with tri(cid:173)
`and with ethyl ethanoate.
`
`miscible solvents
`solvents are truly immiscible, and even though two liquids may not appear to
`there will still be a tiny amount of each solvent present in the other layer. Table
`.3 shows the solubilities of organic solvents in water, and of water in organic sol(cid:173)
`The units of the solubilities are grains of organic solvent per 100 g of saturated
`, and grams of water per 100 g of saturated organic solvent.
`
`Water
`
`Tetrachloromethane
`
`Mercury
`
`Fig. 11.1 Three immiscible
`liquids-tetrachloromethane,
`mercury and water: mercury
`(density 13.6gcm- 3 at 25°C)
`sinks to the bottom:
`tetrachloromethane (density
`1.6 g cm- 3 ) occupies the
`middle position; and water
`(density l.Ogcm~· 3) floats on
`top.
`
`Page 4 of 4