Question

Calculate [H ], [ClO4–], and [OH–] in an aqueous solution that is 0.135 M in HClO4(aq) at 25 °C.

H^+ =

ClO-4 =

OH- =

Is the solution acidic basic or neutral?

Answer 1

Since, in 0.135 M solution, water is also present at a concentration of 10^-7 mol/L

Hence [H⁺] = 0.135 + 10^-7 ~/== 0.135 M

Since HClO₄ being a strong acid, is a strong electrolyte, hence considering full dissociation:

[ClO₄^-] = 0.135 M

Solution will be acidic due to presence of H⁺ ions in high concentration.

Furhter, concentraion of OH^- will be only because of water, which is:

[OH^-] = 10^-7.

Note that water has 10^-7 H⁺ and 10^-7 OH^- ions in it (based on ionic product of water).

Thanks