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where the brackets denote the concentration of the species at equilibrium. The value of K c can provide insights about the extent of a reaction. A large K c means the reaction largely produces products, while a small Kc means mostly reactants are present at equilibrium.
The concentrations are usually given in molarity (M). The letters a, b, c, and d represent the stoichiometric coefficients in the balanced chemical equation. [A], [B], [C], and [D] indicate the equilibrium concentrations of the species.
The relation between K p and K c is:
If you're working with gaseous reactions and using partial pressures, you'd denote the reaction quotient as Q
p
. The formula is analogous, but with partial pressures instead of concentrations:
Where: [A], [B], [C], and [D] are the concentrations (or partial pressures for Q
p
) of the reactants and products at a specific time. a, b, c, and d are the stoichiometric coefficients.
A larger K a value indicates a stronger weak acid.
A larger K
b
value indicates a stronger weak base.
Similarly, if you know K
b
for a weak base, you can determine K
a
for its conjugate acid.
Integrated Form (over a temperature range):
K
1
and K
2
indicate equilibrium constants at temperatures T
1
and T
2
, respectively.
Where K
w
is the ionic product of water, and K
a
is the ionization constant of the weak acid (in this case, CH
3
COOH).
Degree of hydrolysis,
C is the concentration of the salt.
