Conjugate acid - Wikipedia, the free encyclopedia
`
`Pagelof6
`
`Conjugate acid
`
`From Wikipcdia, the free encyclopedia
`
`A conjugate acid, within the Bremsted-Lowry acid-base theory, is a species formed by the reception of
`a proton (H+) by a base-in other words, it is a base with a hydrogen ion added to it. On the other hand,
`a conjugate base is merely what is left after an acid has donated a proton in a chemical reaction. Hence,
`a conjugate base is a species formed by the removal of a proton from an acidY1
`
`In summary, this can be represented as the following chemical reaction:
`
`Jobannes Nicolaus Bmnsted (left)
`and Martin Lowry (right).
`
`Acid + Base -.= Conjugate Base+ Conjugate Acid
`
`Johannes Nicolaus Bmnsted and Martin Lowry introduced the
`Bmnsted-Lowry theory, which proposed that any compound that
`can transfer a proton to any other compound is an acid, and the
`compound that accepts the proton is a base. A proton is a nuclear
`particle with a unit positive electrical charge; it is represented by
`the symbol H+ because it constitutes the nucleus of a hydrogen
`atom,(2] that is, a hydrogen cation.
`
`A cation can be a conjugate acid, and an anion can be a conjugate
`base, depending on which substance is involved and which acid
`-base theory is the viewpoint.
`['''"'""'"'''"'''"'"''''''''''"''''"''''"''''"'''''''''"'"'''"'"'''''''''''''''''''' ........................ .
`
`I Contents
`
`II_
`
`l Acid-base reactions
`'
`•
` ..
`• 2 Strength of conjugates
`• 3 Identifying conjugate acid-base pairs
`I
`• 4 Applications
`• 5 Table of acids and their conjugate bases l
`• 6 Table of bases and their conjugate acids I
`• 7 See also
`!
`• 8 References
`:
`I
`!-----·-·--··-------··---·------··--·-·---··········-··-·----·---·----·-_j
`Acid-base reactions
`
`1!
`
`In an acid-base reaction, an acid plus a base reacts to form a conjugate base plus a conjugate acid:
`
`Conjugates are formed when an acid loses a hydrogen proton or a base gains a hydrogen proton. Refer to
`the follo:ying figure:
`
`https :1/en.wikipedia.org/wiki/Conjugate _acid
`
`7/8/2016
`
`Petitioner - Catalanet Pharma Solutions
`Ex. 1017, Pg. 1 of 6
`
`

`

`Conjugate acid - Wikipedia, the free encyclopedia
`
`Page 2 of6
`
`Jl
`ti--...
`~,N/
`
`I H
`
`Acid
`
`Conjng11l~ Add
`
`We say that the water molecule is the conjugate acid of the hydroxide ion after the latter received the
`hydrogen proton donated by ammonium. On the other hand, ammonia is the conjugate base for the acid
`ammonium after ammonium has donated a hydrogen ion towards the production of the water molecule.
`We can also refer to OH- as a conjugate base of H 20, since the water molecule donates a proton towards
`the production ofNH! in the reverse reaction, which is the predominating process in nature due to the .
`strength of the base NH3 over the hydroxide ion. Based on this information, it is clear that the terms
`"Acid", "Base", "conjugate acid", and "conjugate base" are not fixed for a certain chemical species; but
`are interchangeable according to the reaction taking place.
`
`Strength of conjugates
`
`The strength of a conjugate acid is directly proportional to its dissociation constant. If a conjugate acid is
`strong, its dissociation will have a higher equilibrium constant and the products of the reaction will be
`favored. The strength of a conjugate base can be seen as the tendency of the species to "pull" hydrogen
`protons towards itself. If a conjugate base is classified as strong, it will "hold on" to the hydrogen proton
`when in solution and its acid will not dissociate.
`
`If a chemical species is classified as a weak acid, its conjugate base will be strong in nature. This can be
`observed in ammonia's (relatively strong base) reaction with water. The reaction proceeds until most of
`the ammonia has been transformed to ammonium. This shift to the right in the chemical equilibrium of
`the reaction means that ammonium does not dissociate easily in water (weak acid), and its conjugate
`base is stronger than the hydroxide ion.
`
`On the other hand, if a species is classified as a strong acid, its conjugate base will be weak in nature. An
`example of this case would be the dissociation of Hydrochloric acid HCl in water. Since HCl is a strong
`acid (it dissociates to a great extent), its conjugate base (Cr) will be a weak conjugate base. Therefore,
`in this system, most H+ will be in the form of a Hydronium ion H30+ instead of attached to a Cl anion
`and the conjugate base will be weaker than a water molecule.
`
`https :I /en. wikipedia.org/wiki/Conjugate _acid
`
`7/8/2016
`
`Petitioner - Catalanet Pharma Solutions
`Ex. 1017, Pg. 2 of 6
`
`

`

`Conjugate acid - Wikipedia, the free encyclopedia
`
`Page 3 of6
`
`To summarize, the stronger the acid or base, the weaker the conjugate and vice versa.
`
`Identifying conjugate acid-base pairs
`
`The acid and conjugate base as well as the base and conjugate acid are known as conjugate pairs. When
`finding a conjugate acid or base, it is important to look at the reactants of the chemical equation. In this
`case, the reactants are the acids and bases, and the acid corresponds to the conjugate base on the product
`side of the chemical equation; as does the base to the conjugate acid on the product side of the equation.
`
`To identify the conjugate acid, look for the pair of compounds that are related. The acid-base reaction
`can be viewed in a before and after sense. The before is the reactant side of the equation, the after is the
`product side of the equation. The conjugate acid in the after side of an equation gains a hydrogen ion, so
`in the before side of the equation the compound that has one less hydrogen ion of the conjugate acid is
`the base. The conjugate base in the after side of the equation lost a hydrogen ion, so in the before side of
`the equation the compound that has one more hydrogen ion of the conjugate base is the acid.
`
`Consider the following acid-base reaction:
`
`Nitric acid (HN03) is an acid because it donates a proton to the water molecule and its conjugate base is
`nitrate (NO~). The water molecule acts as a base because it receives the Hydrogen Proton and its
`conjugate acid is the hydronium ion (H30 \
`
`;.·, .~·,.,._.,..,.,..,...~ . ..,.,._~.,., ,...,..~ ,_.,.,..,._ ~···· •' • .._.,.,._, ... ,,.,.~,·N"'•'•'•'•'-'"-'"-'>~'•'..,,.., .. ,..,,..,., '·"?··· ,.,._ . ...,....,.,.,,..,~,_..._.•,,,,.._ . ..,.,v_.,....,.,,.,.,....., ,--·~··'• ,,.._.., ~~· ..•. •. ~--... .-.• ,,_"·'• ..... o.•...r,.n.; ,.,,,......, • .....-.,..~·~.-.-.-.-.-.. .... _..,.,...-~...,. ~ ..,,..,,....,., .... .,.,.,~
`
`;. ::.,::~_::::::~~=~~~~~~~~::.~--~~·,~,:h ... ~,~:I::~.~~-~-J::~~~~:]~~~~i~i~!~~!~~~[~~?~i~i~.~~~~~~~
`! H3o +
`! HCI02 +H2o -+ c1o~ + H3o +I HClo2l H20 I c1o2
`I
`. jHclo ........ !
`!H2o
`jCio-
`loH-
`ICio- +H2o -+HCIO+OH-
`r~:~~;~~-~?~9~=-~~~~~::~~~~~]~-~.~~~I~;~~~J~~~~~~~~~-,-~_~:~~~·-·_I~:;~~; __ .:~~~~~~~~-~~~
`
`Applications
`
`One use of conjugate acids and bases lies in buffering systems, which include a buffer solution. In a
`buffer, a weak acid and its conjugate base (in the form of a salt), or a weak base and its conjugate acid
`are used in order to limit the pH change during a titration process. Buffers have both organic and non(cid:173)
`organic chemical applications; for instance, besides buffers being used in lab processes, our blood acts
`as a buffer to maintain pH. The most important buffer in our bloodstream is the carbonic acid-
`bicarbonate buffer, which prevents drastic pH changes when C02 is introduced. This functions as such:
`
`Furthermore, here is a table of common buffers.
`
`https:/ I en.wikipedia.org/wiki/Conjugate _acid
`
`7/8/2016
`
`Petitioner - Catalanet Pharma Solutions
`Ex. 1017, Pg. 3 of 6
`
`

`

`Conjugate acid - Wikipedia, the free encyclopedia
`
`Page 4 of6
`
`A second common application with an organic compound would be the production of a buffer with
`acetic acid. If acetic acid, a weak acid with the formula CH3COOH, was made into a buffer solution, it
`would need to be combined with its conjugate base CH3 COO- in the form of a salt. The resulting
`mixture is called an acetate buffer, consisting of aqueous CH3COOH and aqueous CH3COONa. Acetic
`acid, along with many other weak acids, serve as useful components of buffers in different lab settings,
`each useful within their own pH range.
`
`An example with an inorganic compound would be the medicinal use of lactic acid's conjugate base
`known as lactate in Lactated Ringer's solution and Hartmann's solution. Lactic acid has the formula
`C3H60 6 and its conjugate base is used in intravenous fluids that consist of sodium and potassium cations
`along with lactate and chloride anions in solution with distilled water. These fluids are commonly
`isotonic in relation to human blood and are commonly used for spiking up the fluid level in a system
`after severe blood loss due to trauma, surgery, or burn injury.
`
`Table of acids and their conjugate bases
`
`Tabulated below are several examples of acids and their conjugate bases; notice how they differ by just
`one proton (H+ ion). Acid strength decreases and conjugate base strength increases down the table.
`
`https :1/en.wikipedia.org/wiki/Conjugate _acid
`
`7/8/2016
`
`Petitioner - Catalanet Pharma Solutions
`Ex. 1017, Pg. 4 of 6
`
`

`

`Conjugate acid- Wikipcdia, the free encyclopedia
`
`Page 5 of6
`
`......... { ........................................... ''"''"'"''''''"'''
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`.~ ....... ~ .... ,..~._...._,.,...,..,,~,"'""'~'•.,_,..,,., .. ,:
`
`j H3P04 Phosphoric acid
`
`·lNc;:· .. Ni~~~i~~--m
`.................... !
`.
`~~ J
`. ~~;~;~:~;~;~ io~
`i H2P04- Dihydrogen phosphate ion j
`~~~i~~~f;1f:0.: . --=-==·:=l~~~~~ffii~~~f~~;;~:.1
`lir~s·fi;ct;~~~i.furi·~ .. ~~·ict ......................................................... l.ils·~ .. 8;d~~~·~~·~·~ifid~ .. i·~~ ...................... !
`:·il~P·c;~~·~·ih;ci;;~~~ .. ~h;~~·h~·~~ .. i~~· ............................ l.iiP.oi~·fl;ci;~~~~··;h~~;·h~~~··i~~· .... I
`:··· ••W•• ,..,.~ .... " """'"'·""'" ooW•": "'"'' ,•,, •:••o•,,·,.,•,•,, •'•"••"•W•'o'o'oW'o o"o>-0 .. ""'"""~"""• .. "'"' · - ' " '•'-r•• ••" """ '• •·' ••W "''•""•'•"":"""'""~•Y"""-·"-•••"" .. '"""-"''" ~"!
`:NH4 Ammoruum wn
`·
`!NHJ Ammoma
`i
`! ....... ' ........ '' ........... ., ' ..... ' '" ...... ' ......... ·····' .................. ,. .............................. " .. ~ ................................................................................ ' ......... ?
`! HC03- Hydrogencarbonate (bicarbonate) ion! C03
`2
`- Carbonate ion
`;
`jPOl- Phosphate ion
`! HP042
`- Hydrogen phosphate ion
`
`i······"'""'''············"''''''"""'''"''"''"''"'''"''''''""'''•·• .. ··""'"""'"""""""""'"i· .................................................................................... ..
`
`:~~~-~-~~~i~~~i.~~:~~:."~~.:?x:::::_:·~~::·:::~·:::~~~=.~~~~ .. ~J~~~~f~~;~~~i:~?.;·_·:: .. :~.-~:::::::·::~~-~~~J
`
`.
`
`Table of bases and their conjugate acids
`
`B~~·~.................. .. . .. .
`
`} ' '<' >
`
`0' < 0 0. OJ.~'·~---· 0 -~<>.< 0 ' " ' - - ~~-~-·- • , . - . . , • ...,., ... ~, ... _ _.,...,.,......,.>'< .... < ... <.., ........ :
`' " " ' ... ' ' " " ' ' " ' " ' .... ~ ...... ~ .......... ~.~~-~·- 0 OA~ ... AO~ ·~ , , ~-~:v.~ .. <'
`1 NH; Ammonium ion
`
`In contrast, here is a table ofbases and their conjugate acids. Similarly, base strength decreases and
`conjugate acid strength increases down the table.
`Conjugat~.A~·id ................ ~
`! C2~~NH~.i~h~~~~i~~ .... ·:·~·ii~~HfE~h;l~~~~ium io~ -~
`I C·H~~~··~·~~h~~~~i~~ .... CH~NH; ·~~~h;l~~~~~·;~~··i·~·~· .. ,
`!
`r~~·~~~ .. ~;~~~~ .................. r~~~~~+·~·d~~~~~ ................................ !
`! NH3 Ammonia
`rc~i~~N~;·~~iii~~ ............... rc~·~~~~f;h~·~;i·~~~~i~ .. i~~·l
`r.~.;~;~~~::~i;~;!·~.:i?~:r:~~~~~~~~~;? .. ~~:-~~:i·~::::.::::·: .... :":"')
`i
`
`j F- Fluoride ion
`
`j HF Hydrogen fluoride
`
`!.oo.~ '-"'~' -...~,.....,..,.....,.,,... ~-'-" ~ ~ . ._.,..,"'"~""•'-'•~··· ·•·~·~•"''•'_..'~.~·'• N"'-'' ~r" '•' ~· "·''-'•~-·.o.•• ..,..,.,....,_.......,.~,....., .... ~,..,~~"'''"'......_ ... .._.,.,..,..,~•A.,.,v,'-'........,...._V,.,..,• ... ~·?•'l
`
`See also
`
`https :/I en. wikipedia.orglwiki/Conj ugate _acid
`
`7/8/2016
`
`Petitioner - Catalanet Pharma Solutions
`Ex. 1017, Pg. 5 of 6
`
`

`

`Conjugate acid- Wikipedia, the free encyclopedia
`
`Page 6 of6
`
`• Buffer solution
`• Deprotonation
`• Protonation
`• Salt (chemistry)
`
`References
`
`1. Zumdahl, StephenS., & Zumdahl, Susan A Chemistry. Houghton Mifflin, 2007, ISBN 0618713700
`2. "Brons ted-Lowry theory". Encyclopredia Britannica. Encyclopredia Britannica Online. Encyclopredia
`Britannica Inc., 2015. Web. 21 Apr. 2015 <http://www.britaunicu.com/EBchecked/topic/80953/Bronsted(cid:173)
`Lowry-theory>.
`
`Retrieved from "https://en.wikipedia.org/w/index.php?title=Conjugate_acid&oldid=720365841"
`
`Categories: Acid-base chemistry
`
`• This page was last modified on 15 May 2016, at 12:06.
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`
`https :/ /en.wikipcdia.org/wiki!Conjugate _acid
`
`7/8/2016
`
`Petitioner - Catalanet Pharma Solutions
`Ex. 1017, Pg. 6 of 6
`
`