Formic acid is a weak acid. It has a pKa of 3.75. Now a mixture of formic acid with its corresponding salt will give a buffer mixture.
Thus here the formic acid and sodium formate mixture is a type of acidic buffer solution.
To find out the pH of this solution we have to apply the Henderson equation, which looks like:
Where the terms in the parentheses denote the concentrations of the salt and acid.
Now given terms are, pKa = 3.75; [formic acid] = 0.020 M; [sodium formate] = 0.060 M
Thus,
The pH of the solution is = 4.22
a What is the pH of a solution that has a formic acid concentration of 0.020...
A buffer is composed of formic acid and its conjugate base, the formate ion. K for formic acid is 1.8 x 10. a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH
For the solution of 0.020 moles of formic acid (HCOOH) and 0.010 moles of sodium formate (pka = 3.7545 at 25 C) obtain: a) the reactions involved in the process b) the derivation of the Henderson-Hasselbalch expression from equilibrium for the dissolution of the formic acid. c) the pH of the system and the pOH d) the concentration of H3O+ e) the concentration of OH- of the system
A solution of 0.073 M in formic acid, HCOOH, and has a pH of 4.59. What is the concentration of formate ion?
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
a. Find the pH of a solution that is 0.500 M in formic acid and 0.250 M in sodium formate. K. (formic acid) = 1.8 x 10-4 pH- b. Find the pH after 0.100 mol HCl has been added to 1.00 liter of the solution. pH =
What is the change in pH from a solution containing 0.523 M of formic acid (Ka = 1.77 x 10-4) vs a solution containing 0.523 M formic acid and 0.496 M Sodium formate? Report your answer to 2 decimal places.
24. (25 points) A buffer solution was prepared by dissolving 0.500 mol formic acid and 0.060 mol sodium formate in enough water to make 1 L of solution, K, for formic acid is 1.80 x 104 a) Calculate the pH of the solution. b) If this solution was diluted to 10 times its volume, what would be the pH.
Using Henderson-Hasselbalch equation, Calculate the pH of a buffer solution that is 0.060 M formic acid (HCHO) and 0.150 M potassium formate (KCHO2). Remember that Kg = 1.8 X 10-4 for formic acid. O 1.45 O 2.36 09.12 4.13 O 0.0125 7.00
Calculate the pH of a solution that is made up of 2.39 M formic acid (HCOOH) and 0.77 M sodium formate (NaOOCH)
Using Henderson-Hasselbalch equation, Calculate the pH of a buffer solution that is 0.060 M formic acid (HCHO2) and 0.150 M potassium formate (KCHO2). Remember that Ka = 1.8 X 10-4 for formic acid. Group of answer choices A 1.45 B 2.36 C.9.12 D.4.13 E. 0.0125 F. 7.00