Study Set Content:
pKa is related to
Ka
Remember that the stronger the acid
the smaller the pKa
Two important characteristics of a buffer are its
pH and its buffer capacity
The solution has the ability to resist changes in pH upon the addition of
small amounts of either acid or base
principal ingredient in vinegar; that's why it tastes sour.
Acetic Acid
the presence of suppresses the ionization of a weak acid or a weak base.
common ion
Blood contains
H2CO3 and HCO3 -
Equilibria involving weak bases are to those for weak acids
treated similarly
A stronger acid has a larger than does a weaker acid.
ionization constant
For any conjugate acid-base pair, the product of the aciddissociation constant for the acid and the base-dissociation constant for the base is always equal to the
ion-product constant of water
change upon addition of a strong acid or a strong base.
pH of a buffer
This relationship holds for all the conjugate acid-base pairs. As the strength of an acid increases (larger Ka), the strength of its conjugate base decreases (smaller Kb) because the product Ka x Kb remains constant at 1.0 x 10-14 .
yes
is the equilibrium constant for the solubility equilibrium of a slightly soluble (or nearly insoluble) ionic compound.
solubility product constant (Ksp)
The value of Ksp indicates the solubility of an ionic compound— the smaller the value, the (blank) the compound in water.
less soluble
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tooth decay (occurs when the calcium hydroxylapatite ,Ca5(PO4)3(OH), in our teeth dissolves
Dissolution
Controlling the equilibrium between a slightly soluble ionic solid and an aqueous solution of its ions
PRECIPITATION AND DISSOLUTION
formulation of antacids (aluminum hydroxide); stalactites and stalagmites (CaCO3 ), barium sulfate (BaSO4 ), an insoluble white precipitate is used as a diagnostic aid
Precipitation
Lewis Concept of Acids and Bases
Gilbert Newton Lewis
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