Problem: Determine the pH of each of the following solutions.0.21 M KCHO2

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FREE Expert Solution

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

88% (401 ratings)
Problem Details

Determine the pH of each of the following solutions.

0.21 M KCHO2

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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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Based on our data, we think this problem is relevant for Professor Zhai's class at UCF.