What is the ph of a 0.286 m solution of hypochlorous acid (ka 2.9 x 10-8)?

4.0406

Explanation:

Given that:

Concentration = 0.286 M

Consider the ICE take for the dissociation of acetic acid as:

                                      HClO    ⇄     H⁺ +        ClO⁻

At t=0                            0.286                 -              -

At t =equilibrium        (0.286-x)                x           x            

The expression for dissociation constant of acetic acid is:

x is very small, so (0.286 - x) ≅ 0.286

Solving for x, we get:

x = 9.1071×10⁻⁵  M

pH = -log[H⁺] = -log(9.1071×10⁻⁵) = 4.0406

the correct answer is answer a. a mixture

no other options make sense

hope this

have a great day : )

  - sprinkles

samuel de champlain. in 1608, king henry iv sponsored pierre dugua, sieur de mons and samuel de champlain as founders of the city of quebec with 28 men. this was the second permanent french settlement in the colony of canada.