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1. Given a solution of 0.13 M formic acid (HCOOH) with a pH of 2.40, calculate the acid's ka.

2. One tablet of aspirin typically holds 324 mg of the chemical compound. Aspirin, C9O4H8, functions as a monoprotic acid with a Ka of 2.8 x 10-4. If two tablets are dissolved in 300 mL of water, what would the pH of the solution be?

3. Explain what a high Ka value of an acid represents and what a low Ka value represents

4. State and explain the difference between the endpoint and the equivalence point in a titration

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