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
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.
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