Problem: 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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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 baseproton acceptor
H2O → will act as the weak acidproton donor


Equilibrium reaction:        ClO-(aq)  + H2O(l)  HClO(aq) + OH-(aq)


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Problem Details

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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Our tutors have indicated that to solve this problem you will need to apply the Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.