Question

Question 6 0.1 pts Consider a titration of formic acid (HCOOH, K2 = 1.8 x 10-4) with NaOH. The experiment is halted when half of the acid has been titrated. Which statement correctly describes the composition of the titration solution? Check all that apply. The concentrations of HCOOH and H+ are equal. The concentration of HCOOH is greater than the concentration of H+. The concentration of formate ions (HCOO-) is smaller than the concentration of H+. The concentration of HCOO-is approximately equal to the concentration of HCOOH.

Answer 1

First see balance reaction between formic acid and NaOH -

HCOOH + NaOH $\LARGE \rightarrow$ HCOONa + H₂O

From balance reaction it is clear that one mole of formic acid required one mole of sodium hydroxide.

So experiment is halted after exactly half of addition of formic acid. That's means half of formate ion(HCOO^-) gets formed and half of formic acid should be remain as it is (HCOOH). So option '4 ' is only correct .