7. Rinse the burette and pipette with water and put the burette upside down with the tap open. Data Table Exp Rough titration Vi(mL) Vf(mL) Volume of NaOH used (mL) 1 2 3 0 29.8 29.8 0 30.0 30.0 30.2 30.2 Average volume of NaOH used = pH of vinegar (ethanoic acid solution) = 2.8 [NaOH)= 0.40 mol/L Volume of ethanoic acid used in the titration 10.00 mL 29.8+30.0+30.2 = 30.0 (mL) 3 1. Write the balanced equation for the neutralization reaction between ethanoic acid and sodium hydroxide solutions. Include states. CH3COOH(aq) + NaOH(aq) CHǝ CooNa (aq) + H2O (e) 2. Calculate the concentration of the ethanoic acid. Use the ratio in which the acid and base react according to the balanced equation. 30mL = 0.03L 144 C₁ V₁ = C2 V₂ = CH3COOH NaoH (0.4 mol/L) (0.03L)= C (0.01L) C = 1.2 mol/L 100mL=0.01 L molar ratio: 二十 CIVI C2V2 = + => CIV₁ = C₂ V2 3. Calculate the [H+] (or [H3O+]) from the pH measurement. PH = -log [H+] 2.8 = -109, CH+] 1028 = [H+] CH+] 1.58x10 mol/L 4. Write the Ka expression for ethanoic acid in water.[K/U 1 mark] CH3COOH (99) + H2O (l) → CH3 C00¯ +H30+ H2O(CH3 [CH3 C00][H3O+] ka: = [CH3COOH] 5. Set up into ep Keep out of ch Do not get in o leugh c of adım so 5. Set up an ICE table for the ionization of acetic acid in water. Then substitute the equilibrium concentrations into the Ka expression and calculate the value of Ka. CH3COOH caq) + H2O (e) CH 3 COO (aq) + H30+ (ag). I 1.2 -x ICE 1.2-X 0 X 0 X X X 6. Calculate the % ionization of the ethanoic acid in the vinegar. Write the equation and show the substitution.
7. Rinse the burette and pipette with water and put the burette upside down with the tap open. Data Table Exp Rough titration Vi(mL) Vf(mL) Volume of NaOH used (mL) 1 2 3 0 29.8 29.8 0 30.0 30.0 30.2 30.2 Average volume of NaOH used = pH of vinegar (ethanoic acid solution) = 2.8 [NaOH)= 0.40 mol/L Volume of ethanoic acid used in the titration 10.00 mL 29.8+30.0+30.2 = 30.0 (mL) 3 1. Write the balanced equation for the neutralization reaction between ethanoic acid and sodium hydroxide solutions. Include states. CH3COOH(aq) + NaOH(aq) CHǝ CooNa (aq) + H2O (e) 2. Calculate the concentration of the ethanoic acid. Use the ratio in which the acid and base react according to the balanced equation. 30mL = 0.03L 144 C₁ V₁ = C2 V₂ = CH3COOH NaoH (0.4 mol/L) (0.03L)= C (0.01L) C = 1.2 mol/L 100mL=0.01 L molar ratio: 二十 CIVI C2V2 = + => CIV₁ = C₂ V2 3. Calculate the [H+] (or [H3O+]) from the pH measurement. PH = -log [H+] 2.8 = -109, CH+] 1028 = [H+] CH+] 1.58x10 mol/L 4. Write the Ka expression for ethanoic acid in water.[K/U 1 mark] CH3COOH (99) + H2O (l) → CH3 C00¯ +H30+ H2O(CH3 [CH3 C00][H3O+] ka: = [CH3COOH] 5. Set up into ep Keep out of ch Do not get in o leugh c of adım so 5. Set up an ICE table for the ionization of acetic acid in water. Then substitute the equilibrium concentrations into the Ka expression and calculate the value of Ka. CH3COOH caq) + H2O (e) CH 3 COO (aq) + H30+ (ag). I 1.2 -x ICE 1.2-X 0 X 0 X X X 6. Calculate the % ionization of the ethanoic acid in the vinegar. Write the equation and show the substitution.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases
Section: Chapter Questions
Problem 118IL: Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H)...
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![7. Rinse the burette and pipette with water and put the burette upside down with the tap
open.
Data Table
Exp
Rough titration Vi(mL)
Vf(mL)
Volume of NaOH
used (mL)
1
2
3
0
29.8
29.8
0
30.0
30.0
30.2
30.2
Average volume of NaOH used
=
pH of vinegar (ethanoic acid solution) = 2.8
[NaOH)= 0.40 mol/L
Volume of ethanoic acid used in the titration
10.00 mL
29.8+30.0+30.2
= 30.0 (mL)
3
1. Write the balanced equation for the neutralization reaction between ethanoic acid and sodium hydroxide
solutions. Include states.
CH3COOH(aq) + NaOH(aq) CHǝ CooNa (aq) + H2O (e)
2. Calculate the concentration of the ethanoic acid. Use the ratio in which the acid and base react according to
the balanced equation.
30mL = 0.03L
144 C₁ V₁ = C2 V₂ = CH3COOH
NaoH
(0.4 mol/L) (0.03L)= C (0.01L)
C = 1.2 mol/L
100mL=0.01 L
molar ratio:
二十
CIVI
C2V2
= + => CIV₁ = C₂ V2
3. Calculate the [H+] (or [H3O+]) from the pH measurement.
PH = -log [H+] 2.8 = -109, CH+] 1028 = [H+]
CH+] 1.58x10 mol/L
4. Write the Ka expression for ethanoic acid in water.[K/U 1 mark]
CH3COOH (99) + H2O (l) → CH3 C00¯ +H30+
H2O(CH3
[CH3 C00][H3O+]
ka:
=
[CH3COOH]
5. Set up
into](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ad229d2-94c2-4360-b0ca-273c76ee826c%2F6fe7323c-cb35-42fe-b123-5e4b34267ad5%2F7x65ix_processed.jpeg&w=3840&q=75)
Transcribed Image Text:7. Rinse the burette and pipette with water and put the burette upside down with the tap
open.
Data Table
Exp
Rough titration Vi(mL)
Vf(mL)
Volume of NaOH
used (mL)
1
2
3
0
29.8
29.8
0
30.0
30.0
30.2
30.2
Average volume of NaOH used
=
pH of vinegar (ethanoic acid solution) = 2.8
[NaOH)= 0.40 mol/L
Volume of ethanoic acid used in the titration
10.00 mL
29.8+30.0+30.2
= 30.0 (mL)
3
1. Write the balanced equation for the neutralization reaction between ethanoic acid and sodium hydroxide
solutions. Include states.
CH3COOH(aq) + NaOH(aq) CHǝ CooNa (aq) + H2O (e)
2. Calculate the concentration of the ethanoic acid. Use the ratio in which the acid and base react according to
the balanced equation.
30mL = 0.03L
144 C₁ V₁ = C2 V₂ = CH3COOH
NaoH
(0.4 mol/L) (0.03L)= C (0.01L)
C = 1.2 mol/L
100mL=0.01 L
molar ratio:
二十
CIVI
C2V2
= + => CIV₁ = C₂ V2
3. Calculate the [H+] (or [H3O+]) from the pH measurement.
PH = -log [H+] 2.8 = -109, CH+] 1028 = [H+]
CH+] 1.58x10 mol/L
4. Write the Ka expression for ethanoic acid in water.[K/U 1 mark]
CH3COOH (99) + H2O (l) → CH3 C00¯ +H30+
H2O(CH3
[CH3 C00][H3O+]
ka:
=
[CH3COOH]
5. Set up
into
Transcribed Image Text:ep
Keep out of ch
Do not get in o
leugh c
of
adım so
5. Set up an ICE table for the ionization of acetic acid in water. Then substitute the equilibrium concentrations
into the Ka expression and calculate the value of Ka.
CH3COOH caq) + H2O (e) CH 3 COO (aq) + H30+ (ag).
I
1.2
-x
ICE
1.2-X
0
X
0
X
X
X
6. Calculate the % ionization of the ethanoic acid in the vinegar. Write the equation and show the substitution.
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