1) Consider a titration of 43.8 mL of 0.124M solution of formic acid [Ka(HCOOH)=

Question

1) Consider a titration of 43.8 mL of 0.124M solution of formic acid [Ka(HCOOH)=1.8x10^-4] with a 0.161 M solution of sodium hydroxide. Calculate (show all work for full marks):

a) the pH of the formic acid solution before the solution before the titration,

b) the pH of the solution at half-equivalence point,

c) the pH of the solution at the equivalence point,

d) the pH of the solution whe 1.00 mL of the NaOH have been added after the equivalence point was reached.

e) What would have been the volume (in mL) of 0.161M solution of barium hydroxide added to the equivalence point if it were used instead of the 0.161M NaOH solution?

Explanation / Answer

HCOOH + NaOH ? HCOO- + Na+ + H2O

From the equation we can see that the ratio between HCOOH and NaOH is 1:1

NOTE: we need to know how many moles of HCOOH is present to start with

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.