Chemistry Practice Problems Diprotic Acid Practice Problems Solution: Consider an aqueous solution of H2CO3. What is the...

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Solution: 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 MC. 10.3 and 6.8 × 10–4 M D. 3.8 and 4.3 × 10–7 ME. 6.4 and 4.7 × 10–11 M

Problem

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

B. 6.4 and 2.1 × 10–4 M

C. 10.3 and 6.8 × 10–4

D. 3.8 and 4.3 × 10–7 M

E. 6.4 and 4.7 × 10–11 M

Solution

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

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