We are being asked to calculate the pH for a .019 M solution of NaClO .
NaClO is the salt form of the conjugate base of HClO.
NaClO disociates as:
NaClO(aq) → Na+(aq) + ClO-(aq)
The acid dissociation goes as:
HClO(aq) + H2O(l) → ClO-(aq) + H3O+(aq)
Since we’re dealing with a weak base and Kb is an equilibrium expression we will have to create an ICE chart to determine the equilibrium concentration of each species:
• ClO-(aq) → weak base → proton acceptor
• H2O → will act as the weak acid → proton donor
Equilibrium reaction: ClO-(aq) + H2O(l) ⇌ HClO(aq) + OH-(aq)
HClO is a weak acid (Ka=4.0x10-8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is .019 M in NaClO?
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