Question

Fluoroacetic acid is a poison that has been used by ranchers in the western United States. The ranchers place the poison in the carcasses of dead animals to kill coyotes that feed in them; unfortunately, however, eagles and hawks are also killed in the process. How many mL of 0.01500 M Ca(OH)₂ are needed to completely neutralize 125.0 mL of 0.3659 M fluoroacetic acid (pK_a = 2.59)? What is the initial pH of the acid solution? What is the pH at the equivalence point?

Answer 1

-log [st] = + 1 / 2 (-log ka-log () F CH₂ coon & Calon), (FCH₂ 200), Ca +H2O It is acidic buffer Initial ph ph= pka + log [(FCH₂ coo), Ca] [ast] = 5 kac [Fch coon 7= 2.59+ log [(FCH220o), a ph i [pka-log (0.36551] [F CH₂ coon (F CH₂600), ca ph= √ (2.59+0.44] 4.41 0.3659X 125 [(FCH₂600), Ca] =201.702 *ph at equivalence point 7 NXV =201702 (0.015X2) V-201702 IN=6723.4 me] Volume of Calon), required 10 ph=1.52 Initial pn