We are being asked to calculate the Ka of a weak acid if 0.021 M solution of the weak acid has a pH of 3.95.
We're going to represent the weak acid as HA. Since we’re dealing with a weak acid and Ka is an equilibrium expression, we will have to create an ICE chart to determine the equilibrium concentration of each species:
• HA → weak acid → proton donor
• H2O → will act as the weak base → proton acceptor
Equilibrium reaction: HA(aq) + H2O(l) ⇌ A-(aq) + H3O+(aq)
The pH of a 0.021 M solution of a weak acid is 3.95. What is the value of Ka for this acid.
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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 Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.
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