🤓 Based on our data, we think this question is relevant for Professor Zhai's class at UCF.
We are being asked to calculate the pH of 0.21 M KCHO2.
KCHO2 is an ionic compound and will break up into its ions in the solution:
KCHO2(aq) → K+(aq) + CHO2-
• main group metals should have a +3 charge or higher to be considered acidic. K+ has only a +1 charge and is a neutral ion so it will not contribute to the pH of the solution
• CHO2- is the conjugate base of the weak acid CHO2H
CHO2H(aq) + H2O(l) ⇌ CHO2-(aq) + H3O+(aq) Ka = 1.8x10-4
(weak acid) (conjugate base)
**Ka value can be found in books or online sources
CHO2- also acts as weak base and can ionize in the solution to form the weak acid
Determine the pH of each of the following solutions.
0.21 M KCHO2