The pka of hypochlorous acid is 7.530. a 52.0 ml solution of 0.149 m sodium hypochlorite (naocl) is titrated with 0.293 m hcl. calculate the ph of the solution

The pH of the buffer solution is 7.236

Explanation:

Henderson - Hasselbalch equation of a buffer solution consisting of a weak acid and its conjugate base is given as:

The hypochlorous acid (HCIO),  is the weak acid  and the conjugate base the  hypochlorite anion (ClO⁻) is the conjugate base.

The dissociation of the salt is given by:

NaOCl(aq)  ⇒  Na⁺(aq) + ClO⁻(aq)

The salt dissociate at a ratio of 1:1

Substituting values to get:

The pH of the buffer solution is 7.236

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.