Question

For the dissociation reaction of a weak acid in water, HA(aq) + H?O(l) ? H?O?(aq) + A?(aq) the equilibrium constant is the acid-dissociation constant, Ka, and takes the form Ka = [H?O?][A?] / [HA] Weak bases accept a proton from water to give the conjugate acid and OH? ions: B(aq) + H?O(l) ? BH?(aq) + OH?(aq) The equilibrium constant Kb is called the base-dissociation constant and can be found by the formula Kb = [BH?][OH?] / [B] When solving equilibrium-based expression, it is often helpful to keep track of changing concentrations is through what is often called an I.C.E table, where I. stands for Initial Concentration, C. stands for Change, and E. stands for Equilibrium Concentration. To create such a table, write the reaction across the top creating the columns, and the rows I.C.E on the left-hand side. A + B ? AB Initial (M) Change (M) Equilibrium (M)

          For the dissociation reaction of a weak acid in water,
HA(aq) + H?O(l) ? H?O?(aq) + A?(aq)
the equilibrium constant is the acid-dissociation constant, Ka,
and takes the form
Ka = [H?O?][A?] / [HA]
Weak bases accept a proton from water to give the conjugate
acid and OH? ions:
B(aq) + H?O(l) ? BH?(aq) + OH?(aq)
The equilibrium constant Kb is called the base-dissociation
constant and can be found by the formula
Kb = [BH?][OH?] / [B]
When solving equilibrium-based expression, it is often helpful to
keep track of changing concentrations is through what is often
called an I.C.E table, where I. stands for Initial Concentration, C.
stands for Change, and E. stands for Equilibrium Concentration.
To create such a table, write the reaction across the top creating
the columns, and the rows I.C.E on the left-hand side.
A + B ? AB
Initial (M)
Change (M)
Equilibrium (M)

For the dissociation reaction of a weak acid in water,
HA(aq) + H?O(l) ? H?O?(aq) + A?(aq)
the equilibrium constant is the acid-dissociation constant, Ka,
and takes the form
Ka = [H?O?][A?] / [HA]
Weak bases accept a proton from water to give the conjugate
acid and OH? ions:
B(aq) + H?O(l) ? BH?(aq) + OH?(aq)
The equilibrium constant Kb is called the base-dissociation
constant and can be found by the formula
Kb = [BH?][OH?] / [B]
When solving equilibrium-based expression, it is often helpful to
keep track of changing concentrations is through what is often
called an I.C.E table, where I. stands for Initial Concentration, C.
stands for Change, and E. stands for Equilibrium Concentration.
To create such a table, write the reaction across the top creating
the columns, and the rows I.C.E on the left-hand side.
A + B ? AB
Initial (M)
Change (M)
Equilibrium (M)

Added by Colleen H.

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