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`MYLAN INST. EXHIBIT 1119 PAGE 1
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`MYLAN INST. EXHIBIT 1119 PAGE 1
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`MYLAN INST. EXHIBIT 1119 PAGE 1
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`

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`Address editorial correspondence to
`
`D . C. Heath and C o m p a n y
`
`125 Spring Street
`L e x i n g t o n , M A 0 2 1 7 3
`
`Acquisitions E d i t o r : K e n t P o r t e r H a m a n n
`Project Consultant: R i c h a r d E. M o r e l
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`Designer: K e n n e t h H o l l m a n
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`A r t E d i t o r : G a r y Crespo
`Photo Researcher: M a r k Corsey
`T e x t Permissions E d i t o r : M a r g a r e t R o l l
`
`C o p y r i g h t © 1993 b y D . C . H e a t h and C o m p a n y .
`Previous editions c o p y r i g h t © 1989, 1986 by D . C . H e a t h and C o m p a n y .
`
`A l l
`
`.
`rights reserved. N o part o f
`
`1 an
`.
`this p u b l i c a t i o n m a y be r e p r o d u c e d ort r a n s m i t t e d o r any
`
`i n c l u d i n g p h o t o c o p y , r e c o r d i n g , blisher.
`f o r m o r b y any means, electronic o r m e c h a n i c a l ,
`i n f o r m a t i o n storage o r
`retrieval s y s t e m , w i t h o u t p e r m i s s i o n in w r i t i n g from the pu
`
`Published s i m u l t a n e o u s l y in Canada.
`
`Printed in the U n i t e d States o f A m e r i c a .
`
`International Standard B o o k N u m b e r : 0 - 6 6 9 - 3 2 4 6 2 - 0
`
`L i b r a r y o f Congress C a t a l o g N u m b e r : 92-70801
`
`1 0 9 8 7 6
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`MYLAN INST. EXHIBIT 1119 PAGE 2
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`MYLAN INST. EXHIBIT 1119 PAGE 2
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`¥ 2 8 ? Chopter Four Types of Chemical Reactions and Solution Stoichiometry
`
`5+
`
`@
`
`8 -
`
`O
`
`105°
`
`3t
`
`4.1 Water,
`
`the Common Solvent
`
`Purpose
`
`* To show why the polar nature of water makes it on effective Solvent
`
`Water is one o f the most important substances on earth. Iti s essential for SUStain.
`it also affects our lives in many indireg,
`ing the reactions that keep us alive, but
`ways. Water helps moderate the earth?s temperature;
`it cools automobile engines,
`nuclear power plants, and many industrial processes;
`it provides a means of trans.
`portation on the earth?s surface and a medium f o r the growth o f a myriad ofCrea.
`tures we use as food; and much more.
`One of
`the most valuable properties of water is its ability to dissolvemany
`different substances. For example, salt disappears when you sprinkle it
`into the
`water used to cook vegetables, as does sugar when you add it to your iced tea. In
`each case the ??disappearing?? substance is obviously still present?you can taste it,
`solid dissolves? To understand this process, we need to
`What happens whena
`c o n s i d e r the nature o f water. L i q u i d water consists o f a c o l l e c t i o n o f H , 0 mole-
`cules. A n i n d i v i d u a l H , O molecule is ??bent?? o r V - s h a p e d , w i t h an H ? O ? }
`
`angle o f a p p r o x i m a t e l y 105 degrees:
`
`105°
`s
`
`e
`
`The O ? H bonds in the water molecule are covalent bonds formed by electron
`sharing between the oxygen and hydrogen atoms. However, the electrons of the
`bond are not shared equally between these atoms. For reasons we will discuss in
`later chapters, oxygen has a greater attraction for electrons than does hydrogen. If
`the electrons were shared equally between the two atoms, both would be electrically
`neutral because, on average, the number of electrons around each would equal the
`number of protons in that nucleus. However, because the oxygen atom hasa greater
`attraction for electrons, the shared electrons tend to spend more time close to the
`oxygen than to either of the hydrogens. Thus the oxygen atom gains a slight excess
`of negative charge, and the hydrogen atoms become slightly positive. This is shown
`in Fig. 4.1, where 6 (delta) indicates a partial charge (less than one unit of charge)-
`Because of this unequal charge distribution, water is said to be a polar molecule. It
`is this polarity that gives water its great abilit
`a n
`y to dissolve compounds.
`A schematic o f an ionic solid dissolvin
`g in water is shown in Fig. 4.2. Note that
`wn
`the ??positive ends?? of the water molecules are attracted to the negatively charged
`anions and that the ??negative ends? are attracted to the positively charged cations.
`This process is called hydration. The hydration o f its ions tends to causeas a l t t0
`?fall apart?? in the water, or to dissolve. The Strong forces present among the
`positive and negative ions of the solid are replaced by strong water?ion interactions.
`It
`is very important to recognize that when ionic substances (salts) dissolve in
`they break up into the individual cations and anions. For instance, whet
`water,
`the resulting solution contains
`ammonium nitrate (NH4NO3) dissolves in water,
`N H , ? and NO3~ ions moving around independently. This process can be repre
`sented as
`
`:
`
`i
`Figure 4.1
`(a) The water molecule is polar.
`(b) A space-filling model o f
`the
`water molecule.
`
`Hy
`NH,4NO3(s) 2 2 ? . , N H 4 * ( a q ) + NO37(aq)
`
`;
`
`where (aq) designates that the ions are hydrated by unspecified numbers of
`molecules.
`
`ee
`
`wate
`
`?_?
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`MYLAN INST. EXHIBIT 1119 PAGE 3
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`MYLAN INST. EXHIBIT 1119 PAGE 3
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`4.1 Water, the Common Solvent
`
`1 2 9
`
`Cx? 9 3 )
`
`aston
`
`Figure 4.2
`
`Polar w a t e r molecules interact
`w i t h the positive a n d negative
`ions o f a salt, assisting in t h e
`dissolving process.
`
`The solubility o f ionic substances in water varies greatly. F o r examples o o n
`chloride is quite soluble in water, whereas silver chloride(Contains
`°. a n
`om-
`ions) is only very slightly soluble. Thedifferences int h e o m ities °
`t o n e o l
`pounds in water typically depend on the relative attractions °
`the fons ie a l
`ae
`(these forces hold the solid together) andtheattractions of
`s , Tubilit Ne a complex
`cules (which cause the solid to disperse [dissolve] in water). Solubility
`P
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`MYLAN INST. EXHIBIT 1119 PAGE 4
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`MYLAN INST. EXHIBIT 1119 PAGE 4
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`

`

`1 3 0
`
`Chapter Four Types of Chemical Reactions and SolutionStoichiometry
`
`F i g u r e
`
`4 3
`
`(a) T h e e t h a n o l m o l e c u l e c o n t a i n s
`a p o l a r O ? H bond similar to
`those in the water molecule.
`(6) The p o l a r water m o l e c u l e
`interacts strongly with the polar
`O ? H bond in ethanol. This is a
`case of ?like dissolving like.?
`
`(a)
`
`r a
`
`.
`
`p o m bond
`
`0 }
`
`y
`
`oD
`
`3
`
`Sy,
`
`©
`
`®)
`
`in Chapter 1. However,
`topic that we will explore in much more detail
`the mog
`important thing to remember at this point is that when an ionic solid does dissolve in
`water, the ions become hydrated and are dispersed (move around independently)
`Water also dissolves many nonionic substances. Ethanol (C2H5OH), for exam.
`ple, is very soluble in water. Wine, beer, and mixedd r i n k s are AQUEOUS solutions of
`ethanol and other substances. Why is ethanol so soluble in water? The answer lies in
`the structure o f the alcohol molecules, which is shown in Fig. 4.3(a). Themolecule
`contains a polar O ? H bond like those in water, which makes it very compatible
`is represented in Fig. 4.3(b),
`with water. The interaction of water with ethanol
`Many substances do not dissolve in water. Pure water w i l l not,
`for example,
`dissolve animal fat, because fat molecules are nonpolar and do not interacteffec.
`In general, polar and ionic substances are ex.
`tively with polar water molecules.
`pected to be more soluble in water than nonpolar substances. ??Like dissolves like?
`is a useful rule for predicting solubility. We w i l l explore the basis for this generali-
`zation when we discuss the details o f solution formation in Chapter 11.
`
`4.2 The Nature of Aqueous Solutions: Strong
`and Weak Electrolytes
`
`Purpose
`
`° To c h a r a c t e r i z e strong electrolytes, w e a k e l e c t r o l y t e s , and
`nonelectrolytes.
`
`As we discussed in Chapter 2, a solution is a homogeneous mixture.
`It isthe
`same throughout (the first sip of a cup o f coffee is the same as the last), but it
`composition can be varied by changing the amount o f dissolved substances (one ca"
`In this section we w i l l consider what happens when?
`make weak or strong coffee).
`wit
`the solvent.
`is dissolved in liquid water,
`the solute,
`substance,
`One useful property for characterizing a solution is its electrical conduct!¥! "
`its ability to conduct an electric current. This characteristic can be checkedcont?
`I f the solution in on
`niently by using an apparatus like the one shown in Fig. 4.4.
`the bulb lights. Pure water is not an electric
`container conducts electricity,
`c
`ductor. However, some aqueous solutions conduct current very efficiently. -l t
`b u l b shines v e r y b r i g h t l y ;
`these s o l u t i o n s contain s t r o n g e l e c t r o l y t e s . Other c o f
`tions conduct only a small current, and the bulb glows dimly; these solutions ?
`to flow, and the
`tain weak electrolytes. Some solutions permit no current
`
`remains unlit;
`
`these solutions contain nonelectrolytes.
`
`ee
`
`?
`
`An electrolyte is a substance that
`when dissolved in water produces a
`solution that can conduct electricity.
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`MYLAN INST. EXHIBIT 1119 PAGE 5
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`MYLAN INST. EXHIBIT 1119 PAGE 5
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