ACIDS nad BASES are compounds with three definitions based on how they react when placed in water, what they do with hydrogen ions or protons, and what they do with electron pairs. ELECTROLYTES are compunds that dissociate in water and conduct electricity. Acids, bases, and salts are electrolytes. SALTS are electrolytes fromed from the reaction of acids with bases. NEUTRALIZATION is the reaction of an acid and base carried out to the EQUIVALENCE POINT or END POINT. The EQUIVALENCE POINT occurs when there is an equivalent amount of moles of acid and base in the solution. The END POINT occurs when the the pH indicator changes color near the EQUIVALENCE POINT. BUFFERS are formed from the mixture of a weak acid and its conjugate base or a weak base and its conjugate acid. Buffers are used to keep the pH of a solution constant even when acids or bases are added to it.
DEFINITION OF ACIDS, BASES AND ELECTROLYTES
ACID BASE
Arrhenius add HON produses H3O+ add HON produses OH-
Bronsted-Lowry proton donor proton acceptor
Lewis electron pair acceptor electron pair donor
STRONG acids, bases, and electrolyts dissociate completely in water.
WEAK acids, bases, and electrolyts dissociate incompletely in water and the extent of dissociation is governed by Ka, Kb, or Ksp dissociation constants.
pVALUES are used in acid and base calculations to make it easier to handle the small numbers used.
pVALUE = -LOG10(VALUE)
All the pVALUES in acid base calculations add up to 14.
[H3O+][OH-] = 10^-14
pH + pOH = 14
[H3O+]= 10^-pH
[OH-] = 10^-pOH
Ka * Kb = 10^-14
pKa + pKb = 14
Ka = 10^-pKa
Kb = 10^-pKb
For Buffers use the Henderson Hasselbach Equation
For weak acid HA + HOH <==> A- + H3O+
pH = pKa + LOG10([A-]/[HA])
For weak base B= + HOH <==> HB + OH-
pOH = pKb + LOG10([HB]/[B=])
ICE TABLES are often used to aid in the calculations for acid, base, and electrolyte solutions.
ACIDS
BASES
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BUFFERS