Problem: Find the pH of a 0.135 M aqueous solution of HCIO 2 , for which Ka = 1.1 x 10–2 .A) 1.25B) 3.28C) 1.17D) 1.34E) 1.48

🤓 Based on our data, we think this question is relevant for Professor Walsby's class at SFU.

FREE Expert Solution
FREE Expert Solution

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.


View Complete Written Solution
Problem Details

Find the pH of a 0.135 M aqueous solution of HCIO 2 , for which Ka = 1.1 x 10–2 .

A) 1.25

B) 3.28

C) 1.17

D) 1.34

E) 1.48