Conjugate Acid & Base Pairs Chapter 16 John D. Bookstaver St. Charles Community College St. Peters,...
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Transcript of Conjugate Acid & Base Pairs Chapter 16 John D. Bookstaver St. Charles Community College St. Peters,...
![Page 1: Conjugate Acid & Base Pairs Chapter 16 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall, Inc. Chemistry, The Central.](https://reader035.fdocuments.in/reader035/viewer/2022062516/56649dc65503460f94abb200/html5/thumbnails/1.jpg)
Conjugate Acid & Base PairsChapter 16
John D. Bookstaver
St. Charles Community College
St. Peters, MO
2006, Prentice Hall, Inc.
Chemistry, The Central Science, 10th editionTheodore L. Brown; H. Eugene LeMay, Jr.;
and Bruce E. Bursten
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Some Definitions
• Arrhenius– Acid: Substance that, when dissolved in
water, increases the concentration of hydrogen ions.
– Base: Substance that, when dissolved in water, increases the concentration of hydroxide ions.
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Some Definitions
• Brønsted–Lowry– Acid: Proton donor– Base: Proton acceptor
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A Brønsted–Lowry acid…
…must have a removable (acidic) proton.
A Brønsted–Lowry base…
…must have a pair of nonbonding electrons.
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If it can be either…
...it is amphiprotic/amphoteric
.
HCO3−
HSO4−
H2O
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What Happens When an Acid Dissolves in Water?
• Water acts as a Brønsted–Lowry base and abstracts a proton (H+) from the acid.
• As a result, the conjugate base of the acid and a hydronium ion are formed.
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Conjugate Acids and Bases:
• From the Latin word conjugare, meaning “to join together.”
• Reactions between acids and bases always yield their conjugate bases and acids because a proton (H+) is transferred
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Practice Problem:
• Label the acids and bases and their conjugates for the following:
HCN + H2O ↔ CN- + H3O+
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Acid and Base Strength
• Strong acids are completely dissociated in water.– Their conjugate bases are
quite weak.
• Weak acids only dissociate partially in water.– Their conjugate bases are
weak bases.
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Strong Acids Review
• You will recall that the seven strong acids are HCl, HBr, HI, HNO3, H2SO4, HClO3, and HClO4.
• These are, by definition, strong electrolytes and exist totally as ions in aqueous solution.
• For the monoprotic strong acids,
[H3O+] = [strong acid].
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Acid and Base Strength
• Substances with negligible acidity do not dissociate in water.– Their conjugate bases are
exceedingly strong.
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Strong Bases
• Strong bases are the soluble hydroxides, which are the alkali metal and heavier alkaline earth metal hydroxides (Ca2+, Sr2+, and Ba2+).– Example: NaOH
• Again, these substances dissociate completely in aqueous solution.– [OH-] = [strong base]
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Acid and Base Strength
In any acid-base reaction, the equilibrium will favor the reaction that moves the proton to the stronger base.
HCl(aq) + H2O(l) H3O+(aq) + Cl−(aq)
H2O is a much stronger base than Cl−, so the equilibrium lies so far to the right K is not measured (K>>1).
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Acid and Base Strength
Acetate is a stronger base than H2O, so the equilibrium favors the left side (K<1).
C2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2−(aq)
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Strong or Weak, Acid or Base?
• NaOH• HI• HF
• Mg(OH)2
• CH3COOH
• NH3
• H2SO4
• HCN
• Ca(OH)2
• HClO4
• CN-
• HCl
• C2H2O2-
• LiOH
• HPO42-
• HNO3