What is the ph of a 2.1 m solution of hclo4?

3.61

Explanation:

Concentration = 2.1 M

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

                                      HClO    ⇄     H⁺ +        ClO⁻

At t=0                            2.1                 -              -

At t =equilibrium        (2.1-x)                x           x            

The expression for dissociation constant of acetic acid is:

x is very small, so (2.1 - x) ≅ 2.1

Solving for x, we get:

x = 2.47×10⁻⁴  M

pH = -log[H⁺] = -log(2.47×10⁻⁴) = 3.61

a electronegativity decreases beacuse the size of nucleus is bigger.