What is the approximate ph at the equivalence point of a weak acid-strong base titration if 25 ml of aqueous formic acid requires 29.80 ml of 0.3567 m naoh? ka =1.8 × 10-4 for formic acid.

pH at equivalence point is 8.52

Explanation:

1 mol of HCOOH reacts with 1 mol of NaOH to produce 1 mol of

So, moles of NaOH used to reach equivalence point equal to number of moles produced at equivalence point.

As density of water is 1g/mL, therefore molarity is equal to molality of an aqueous solution.

So, moles of produced =

Total volume of solution at equivalence point = (25+29.80) mL = 54.80 mL

So, at equivalence point concentration of =

At equivalence point, pH depends upon hydrolysis of . So, we have to construct an ICE table.

I: 0.1940                                   0                 0

C: -x                                          +x               +x

E: 0.1940-x                                x                  x

So,

species inside third bracket represent equilibrium concentrations

So,

or,

So,

So,

So,

i believe it is 40–40–20%

explanation:

let that person have a turn to speak : )