Question

In a titration experiment, 38.3 mL of 0.763 M HCOOH neutralizes 39.3 mL of Ba(OH)2. What is the concentration of the Ba(OH)2 solution?

Answer 1

first write the balanced equation

2HCOOH + Ba(OH)2 ---> Ba(HCOO)2 + 2H2O

from this balanced equation it is clear that one mole of barium hydroxide required 2 moles of fomic acid

now calulate the no of moles of fromic acid

no of moles of HCOOH = molarity of HCOOH x volume of HCOOH in liters

= 0.763 x 0.0383 L

= 0.0292 moles

from the balanced equation

one mole of formic acid required half mole of barium hydroxide

so no of moles of Ba(OH)2 = 0.0292/2 = 0.0146 moles

molarity of Ba(OH)2 = moles of Ba(OH)2 / volume of Ba(OH)2

= 0.0146 / 0.0393

= 0.372M