How would you solve c? 33. Formic acid, HCOOH (K₂ = 1.77 x 104) is naturally found in the venom of bee stings, and is usedsynthetically as a preservative in livestock feed.a. Write the K, expression for formic acid.Kax K₁=1.0 x· 10-14077x10-4 x K₁=1.0×10-14 [CO] [OH-]Kb = 5.6×10-11ко[HCOOHIL[0.00660][0.00665][0.243] 1.82x10²4-1.78×10-41682x10-4-97.25100-9720-2.75%"X100 -(0) HC (69)b. Calculate the pH of a 0.25 M solution of formic acid.1.77x10-4 = (0,25M) [H[H+]=7.08×10-4PH=-10g (7.08x10-41) |PH=3.15c. What is the % dissociation of the formic acid?HCOOH0.25M-X0.25-xHCO + + OHXXka=tazDOLLS.250(aq) 0.25025-1-77x10-4x²=4.425x10-5x=0.00665 [H-0005X [HCCOHT=0.243 LHCO1=0.00665px xX₁²

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Answered: PH=3.15 c. What is the % dissociation…

PH=3.15 c. What is the % dissociation of the formic acid? COOH DOLLS 25 = 1.77x10 3.25M (ac HCO + + OH(aq) 025- (aq) ▸ -X100

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.65PAE

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Question

How would you solve c?

3
3. Formic acid, HCOOH (K₂ = 1.77 x 104) is naturally found in the venom of bee stings, and is used
synthetically as a preservative in livestock feed.
a. Write the K, expression for formic acid.
Kax K₁=1.0 x· 10-14
077x10-4 x K₁=1.0×10-14 [CO] [OH-]
Kb = 5.6×10-11
ко
[HCOOHIL
[0.00660][0.00665]
[0.243] 1.82x10²4
-1.78×10-4
1682x10-4-97.25
100-9720-2.75%
"X100 -
(0) HC (69)
b. Calculate the pH of a 0.25 M solution of formic acid.
1.77x10-4 = (0,25M) [H
[H+]=7.08×10-4
PH=-10g (7.08x10-41) |
PH=3.15
c. What is the % dissociation of the formic acid?
HCOOH
0.25M
-X
0.25-x
HCO + + OH
XX
ka=
ta
z
DOLLS
.25
0
(aq) 0.25
025-1-77x10-4
x²=4.425x10-5
x=0.00665 [H-0005
X [HCCOHT=0.243 LHCO1=0.00665
px x
X₁²

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