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

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons