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We are being asked to determine the pH and concentration of CO32- in a solution of 0.10 M H2CO3
We will need the equilibrium constant for oxalic acid and construct an ICE chart to determine the equilibrium concentrations of the CO32-.
Carbonic acid → H2CO3
• can donate two protons (H+) → diprotic acid
• two equilibrium equations → two equilibrium constants
• Equilibrium constants (Ka) can be found in books or on the internet
Consider an aqueous solution of H2CO3. What is the pH and [CO32–] in a 0.10 M H2CO3 solution? [Ka1 = 4.3 × 10–7 ; Ka2 = 4.7 × 10–11]
A. 3.7 and 4.7 × 10–11 M
B. 6.4 and 2.1 × 10–4 M
C. 10.3 and 6.8 × 10–4 M
D. 3.8 and 4.3 × 10–7 M
E. 6.4 and 4.7 × 10–11 M
Frequently Asked Questions
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Our tutors have indicated that to solve this problem you will need to apply the Diprotic Acid concept. You can view video lessons to learn Diprotic Acid. Or if you need more Diprotic Acid practice, you can also practice Diprotic Acid practice problems.
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Based on our data, we think this problem is relevant for Professor Gavva's class at UTD.