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

the only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation:

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)