The following statement has to be proved. Beginning with the equilibrium equation for the dissociation of a weak acid HA, show that “ the percent dissociation varies directly as the square root of K a and inversely as the square root of the initial concentration of HA when the concentration of HA that dissociates is negligible compared with its initial concentration” Concept Introduction: Consider a weak-acid equilibrium reaction, HA ⇌ K a H + +A - The acid dissociation constant K a can be given as, K a = [ H + ] [ A - ] [ HA ] p K a : pK a = -logK a Where, pK a decreases as K a increases. Percent dissociation: It is defined as concentration of dissociated acid divided by the concentration of the acid times 100 % . Percent dissociation = [ HF ] dissociated [ HA ] initial × 100 %
The following statement has to be proved. Beginning with the equilibrium equation for the dissociation of a weak acid HA, show that “ the percent dissociation varies directly as the square root of K a and inversely as the square root of the initial concentration of HA when the concentration of HA that dissociates is negligible compared with its initial concentration” Concept Introduction: Consider a weak-acid equilibrium reaction, HA ⇌ K a H + +A - The acid dissociation constant K a can be given as, K a = [ H + ] [ A - ] [ HA ] p K a : pK a = -logK a Where, pK a decreases as K a increases. Percent dissociation: It is defined as concentration of dissociated acid divided by the concentration of the acid times 100 % . Percent dissociation = [ HF ] dissociated [ HA ] initial × 100 %
Solution Summary: The author explains that the percent dissociation of a weak acid HA varies directly as the square root of
Beginning with the equilibrium equation for the dissociation of a weak acid HA, show that “the percent dissociation varies directly as the square root ofKaand inversely as the square root of the initial concentration of HA when the concentration of HA that dissociates is negligible compared with its initial concentration”
Concept Introduction:
Consider a weak-acid equilibrium reaction,
HA⇌KaH++A-
The acid dissociation constant Ka can be given as,
Ka=[H+][A-][HA]
pKa:
pKa = -logKa
Where, pKa decreases as Ka increases.
Percent dissociation:
It is defined as concentration of dissociated acid divided by the concentration of the acid times 100%.
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