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HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts...

HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.026 M in NaClO at 25 °C?

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Expert Solution

Given Ka = 4.0x10-8

Kb of the base is = Kw / Ka

                         = (1.0x10-14) / (4.0x10-8)

                         = 2.5x10-7

OCl- + H2O HOCl + OH-

Kb = ([HOCl][OH- ]) / [OCl-]

2.5x10-7 = [OH- ]2 / [OCl-]                 Since [HOCl]=[OH- ]

[OH- ] = (2.5x10-7 x[OCl-])

         = (2.5x10-7 x0.026)

         = 8.06x10-5 M

pOH = - log[OH- ]

        = - log(8.06x10-5)

       = 4.1

We know that pH + pOH = 14

So pH = 14 - pOH

          = 14 - 4.1

          = 9.9

Therefore the pH of the solution is 9.9

queen_honey_blossom answered 2 years ago
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