🤓 Based on our data, we think this question is relevant for Professor Walsby's class at SFU.
We’re being asked to calculate the pH of a 0.135 M aqueous solution of HClO2.
Since HClO2 has a low Ka value, it’s a weak acid. Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). The dissociation of HClO2 is as follows:
HClO2(aq) + H2O(l) ⇌ H3O+(aq) + ClO2–(aq); Ka = 1.1 × 10–2
From this, we can construct an ICE table. Remember that liquids are ignored in the ICE table.
The Ka expression for HClO2 is:
Note that each concentration is raised by the stoichiometric coefficient: [HClO2], [H3O+] and [ClO2–] are raised to 1.
Find the pH of a 0.135 M aqueous solution of HCIO 2 , for which Ka = 1.1 x 10–2 .