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`
`SENJU EXHIBIT 2099
`LUPIN v SENJU
`IPR2015-01105
`
`

`
`© Rob Lewis and Wynne Evans 1997,2001
`
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`as the authors of this work in accordance with the
`Copyright, Designs and Patents Act 1988.
`First edition 1997
`Reprinted twice
`Second edition 2001
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`

`
`Solutions and Solubility
`
`contents
`
`Objectives
`
`11.1
`11.2
`
`11.3
`
`Solubility
`
`Dynamic nature of
`dissolution
`
`Solubility of
`sparingly soluble
`ionic compounds
`Distribution ofa
`solute between two
`solvents
`
`Solubility of gases
`in water
`
`Osmosis
`Colloids
`
`170
`
`176
`
`182
`
`183
`
`187
`190
`
`Revision questions
`
`192
`
`>Examines solvent miscibility and immisclbilityl
`
`>Explains the idea of solubility product
`
`>Looks at distribution ratios and gas solubility
`
`>Discusses osmosis and its applications
`
`blntroduces colloids
`
`,. Solubility
`
`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, the
`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 the
`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 71). 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 polarsulastance dissolves, it dissolves only in polar solvents.
`
`2. lfa n0n—poll:1rsubstmice dissolves, it dissolves only in n0n—p0lar 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
`
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`

`
`§1L1PmmmoHmmmmsmwms—mommof
`sing polarity with heptane the least polar and water
`most polar
`
`SOLUBILITY
`
`Formula
`
`CH3(CH2)5CH3
`CH3(CH2)4CH:-1
`CeH12
`ccn
`CeH5CH3
`C2H5OC2H5
`cH2cn
`CH3CH(OH)CH3
`C4H80
`cncg
`CH3CH2OH
`CH3COOC2H5
`CH3COCH3
`CH3OH
`CH3CN
`CH3SOCH3
`H20
`
`Density at
`25 '’c/g cm"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
`
`chloromethane
`’
`an-2-ol
`trahydrofu ran
`ich|oromethane“
`hanoi5 (absolute)
`hyl ethanoatee
`opanone7
`ethanols
`hanenltrileg
`methyl sulfoxide
`ater
`
`ernative names: ‘Carbon tetrachloride, 2Toluene, 3Diethyl ether, 4Chloroform,
`thyl alcohol, 6Ethyl acetate, 7Acetone, “Methyl alcohol, 9Acetonitrile.
`
`lvents in Table 11.1 was obtained in this way. Ofthe common solvents, water is the
`0st polar and the hydrocarbons heptane and hexane the least polar.
`
`iscibility
`
`,
`
`when two solvents are mixed, a single layer (consisting of a solution of the two
`) is produced, the solvents are said to be miscible. lftwo layers are produced
`d both layers consist ofpure solvent, the liquids are said to be immiscible (Fig. 11.1).
`No 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
`yd water produces two phases.
`[Table 11.2 shows which pairs of common solvents are miscible, with 0 denoting
`miscibility. For example, the table shows that water is immiscible with tri-
`loromethane and with ethyl ethanoate.
`
`artially miscible solvents
`
`W solvents are truly immiscible, and even though two liquids may not appear to
`ix, there will still be a tiny amount of each solvent present in the other layer. Table
`-3 shows the solubilities oforganic solvents in water, and ofwater in organic sol~
`ms. The units ofthe solubilities are grains oforganic solvent per 100 g ofsaturated
`ater, and grams ofwater per 100 g ofsaturated organic solvent.
`
`.1, Tetrachloromethane
`
`Fig. 11.1 Three immiscible
`liquids—tetrachloromethane,
`mercury and water: mercury
`(density 13.6 gcm’3 at 25°C)
`sinks to the bottom;
`tetrachloromethane (density
`1.6 g cm‘3) occupies the
`middle position; and water
`(density 1.0 gcm ’3) floats on
`top.
`
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