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 (pKa = 2.59)? What is the initial pH of the acid solution? What is the pH at the equivalence point?

Answer 1

(a) volume required to neutralise floacetic acid as follows: Giren M, = 0.015OOM of Ca6142 VE? My = 0.3569 n of fleuroacetic acid V = lar.omL M, V = V2 V2 M2 V2 0.3569 x 125.0mL My O-OISOOML ve 3049 mL $ 6016)

Ca@W) - FC14-00014 (F-cy cou), Cu + 10 the total wlume of aci acid & base is 6049 + 1250 mL => 31 74mL → Corconfuhim of Felycooh is 304 125ml x 0.3569 M > 44. Gimmol Concentration of Ca6H), =) 30 49 mL x 0.015 -) 45.73 mmol mmol of cality left after complete yol-neutralisatm. is (45.73 - 44.6 mmol 110 mmol [oH] in Molarity 1.12 mmol 31 7 4 mL (OH) = 3.53x154M pOH = -log CoH]

pOH = -log[3.83 x 104 H) POH= 3.45 But paten 4 pH a poh= 14 PH₂ 14-pot - 14-3.45 PH=10.15