We are being asked to calculate the pH of a 0.10-M solution of monochloroacetic acid (HC2H2ClO2).
Since we’re dealing with a weak acid, we will have to create an ICE chart to determine the equilibrium concentration of each species:
• HC2H2ClO2 → weak acid → proton donor
• H2O → will act as the weak base → proton acceptor
Equilibrium reaction: HC2H2ClO2(aq) + H2O(l) ⇌ C2H2ClO2–(aq) + H3O+(aq)
Monochloroacetic acid, HC2H2ClO2, is a skin irritant that is used in “chemical peels” intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of Ka for monochloroacetic acid is 1.35 X 10 -3. Calculate the pH of a 0.10-M solution of monochloroacetic acid.
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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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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.