Calculate the ph of a solution formed by mixing 300.0 ml of 0.30 mhclo with 150.0 ml of 0.20 mliclo. the ka for hclo is 2.9×10−8.

pH = 7.06

Explanation:

The solution formed will be a buffer solution, which is a solution that contains a weak acid-base conjugate pair. The Henderson-Hasselbalch equation may be used to calculate the pH of a buffer solution, where A⁻ is the conjugate base (in this case, ClO⁻) and HA is the conjugate acid (in this case, HClO):

pH = pKa + log([A⁻]/[HA]) = -log(Ka) + log([A⁻]/[HA])

The concentration of the ClO⁻ in the final solution can be calculated using the dilution equation. The volume of the final solution is 450.0 mL.

C₂ = (C₁V₁)/V₂ = (0.20M)(150.0mL)/450.0mL = 0.066...M

Similarly, the concentration of HClO in the final solution is:

C₂ = (C₁V₁)/V₂ = (0.30M)(300.0mL)/450.0mL = 0.20 M

Substituting these values into the Henderson-Hasselbalch equation gives:

pH = -log(Ka) + log([A⁻]/[HA]) = -log(2.9 x 10⁻⁸) + log(0.066.../0.2) = 7.06

it would be d. henry moseley

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