Calculate the ph at of a solution of sodium hypochlorite . note that hypochlorous acid is a weak acid with a of . round your answer to decimal place.

The question is incomplete, here is the complete question:

Calculate the pH at 25°C of a 0.39 M solution of sodium hypochlorite NaClO. Note that hypochlorous acid HClO is a weak acid with a pKa of 7.50. Round your answer to 1 decimal place.

The pH of the solution is 10.4

Explanation:

We are given:

Molarity of sodium hypochlorite = 0.39 M

of HClO = 7.50

We know that:

 of HClO =

To calculate the base dissociation constant for the given acid dissociation constant, we use the equation:

where,

= Ionic product of water =

= Acid dissociation constant  =

= Base dissociation constant

Putting values in above equation, we get:

The chemical equation for the reaction of hypochlorite ion with water follows:

Initial:           0.39

At eqllm:      0.39-x                   x           x

The expression of for above equation follows:

Putting values in above equation, we get:

Neglecting the negative value of 'x' because concentration cannot be negative

To calculate the pOH of the solution, we use the equation:

We are given:

Putting values in above equation, we get:

To calculate pH of the solution, we use the equation:

Hence, the pH of the solution is 10.4

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