Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in some ants. If the formate (HCOO–) concentration is 0.100 M, determine the formic acid (HCOOH) concentration required to buffer a solution at pH = 3.35 HCOOH(aq) ↔ HCOO–(aq) + H+(aq) Ka = 1.80 × 10-4 i) Calculate the pKa of the acid and provide your final answer with 3 decimal places ii) Write the main equation that you will use to help you calculate the formic acid concentration iii) Calculate the formic acid concentration required to buffer the solution at pH = 3.35 and provide your final answer with 3 decimal places
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Formic acid, HCOOH, is the simplest of the
HCOOH(aq) ↔ HCOO–(aq) + H+(aq)
Ka = 1.80 × 10-4
i) Calculate the pKa of the acid and provide your final answer with 3 decimal places
ii) Write the main equation that you will use to help you calculate the formic acid concentration
iii) Calculate the formic acid concentration required to buffer the solution at pH = 3.35 and provide your final answer with 3 decimal places
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