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A chemist titrates 142. mL of a 0.2400 M of HCNO with 0.2300 M solution of NaOh. The pKa of cyanic acid is 3.46.

Calculate pH after:

1. Initial pH

2. After 125.25 mL is added

3. After 148.17 mL is added

4. After 176.0 mL is added

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Determining the volume of NaOH is one of the most important parts as it is required to reach equivalence provided insight on where you are in the problem.

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We must set up an ICE Table to find the initial pH

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We must set up an ICE Table to find the initial pH

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The initial pH= 2.04

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Since 125.25 mL NaOH is before equivalence, this means we are given a buffer problem. Now the moles must be calculated, use the BCA Table and the Henderson-Hasselbalch equation with the pKa given.

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Now, because we are at equivalence , we are dealing with a SALT PROBLEM! We must set an ICE table to find the pH. To find pKb, subtract pKa from 14. Then, take 10^-10.54 and that will be your Kb.

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We're at the end!

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