![L. Determination of K, of acetic aci A. Measure out 10.0 mL of 1.0 M acetic acid (CH,COOH) into a beaker B. Rinse the pH probe with DI H,O and place it into the solution in the beaker eneurine thst the vin Experiment VIl: Buffers Lab Report Il. Determination of the K, of acetic acid 1. Measured pH of the solution pH 2. Calculate the [H,0] at equilibrium for this solution. (include units) 3. Calculate the (CH,COO] at equilibrium for this solution. (include units) [CH.???), 4. What is the [CH,COOH] at equilibrium for this solution? (include units) CH COOH)q 5. Based on these values, what the acid dissociation constant (K,) of acetic acid? (include units)](http://img.homeworklib.com/questions/6cb55200-470e-11ec-a7fd-7ddc95f43d13.png?x-oss-process=image/resize,w_560)
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L. Determination of K, of acetic aci A. Measure out 10.0 mL of...
Experiment VII: Buffers Lab Report ( 49 pts) I. Determination of the K, of acetic acid...
Experiment VII: Buffers Lab Report ( 49 pts) I. Determination of the K, of acetic acid 1. Measured pH of the solution PH 2.40 < Calculate the [H3O*) at equilibrium for this solution. (include units) Tog [HT] = 10-2.40 H 0% 0.004 m. 3. Calculate the [CH,C00] at equilibrium for this solution. (include units) [CH.CO01 0.004 m 4. What is the [CH3COOH) at equilibrium for this solution? (include units) 700. [CH.COOH): 0.00lem 5. Based on these values, what the acid...
d (HCH3 CO2) is 1.8 × 10- e acid dissociation K of acetic aci Th Calculate...
d (HCH3 CO2) is 1.8 × 10- e acid dissociation K of acetic aci Th Calculate the pH of a 2.6 × 10-4M aqueous solution of acetic acid. Round your answer to 2 decimal places.
LUULISI Part B: Determination of K. of Acetic Acid 3. Record the measured pH of vinegar...
LUULISI Part B: Determination of K. of Acetic Acid 3. Record the measured pH of vinegar (acetic acid). Measured pH (2pts) 2.5 a. Calculate the concentration of hydronium ions [H:0") of vinegar from the measured pH values. Express your answer in two significant figures for this question (although it is not correct to do so. Show your work. (10 pts) 4. The concentration of distilled white vinegar is written as 5% (w/v) of acetic acid (CH,COOH), Convert the concentration units...
I need help with the problem in the last photo.. I thought I’d post my lab...
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH...
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH of this solution. 50.0 mL buffer + 2.0mLION NAOH pH 2. Measured pH of this solution. pH 4.59 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 ml the buffer in part D and 2.0...
You are given 75 mL of 0.70 M acetic acid/acetate buffer to test. The starting composition...
You are given 75 mL of 0.70 M acetic acid/acetate buffer to test. The starting composition of the two major species are: Concentration of CH,COOH: 0.250 M Concentration of CH,COO: 0.450 M a. Calculate the initial pH of the buffer. Clearly show all work required to arrive at your answer. b. You add 1.0 mL of 2.00 M HCl to the buffer. Calculate the molarity of H, O' added as HCl, and the final molarities of acetic acid and acetate...
4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO;H and 10.0 mL of a 0.50 M CHC...
4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO;H and 10.0 mL of a 0.50 M CHCO Na. Record this pH in Part II data sheet, Beaker #1 & N2 for Theoretical Initial pH. K for CHCOH = 1.8 x 10 at 25°C. a. Calculate the pH of the buffer solution upon addition of 0.25 mL of a 6.0 M HCL Record in Part Il data sheet, for Theoretical Final pH...
please answer the questions thank you Name: Lab Section: Date: Experiment VII: Buffers Review Questions (23...
please answer the questions thank you
Name: Lab Section: Date: Experiment VII: Buffers Review Questions (23 pts) 1. (3 pts). A solution is prepared by mixing 25.0 mL 0.45 M NaCH,coo and 30.0 mL 0.38 M CH,COOH is prepared. Calculate the pH of this solution if the K, 1.76 x 10 for acetic acid. 2. (3 pts)How many grams of sodium lactate, NaCsHsOs, should be added to 1.00 L of 0.150 M lactic acid, HCsHsOs, to form a buffer solution...
a. Using the initial concentration of CH,COOH (from Problem 3) and the equilibrium concentration of H,0...
a. Using the initial concentration of CH,COOH (from Problem 3) and the equilibrium concentration of H,0 calculated (from Problem 4), complete the reaction table for vinegar. Ignore the column under H:O() (shaded in gray). Don't forget to write a sign (+ or -) for the "Change” row entry. (9 pts: each entry is 1 pt.) Reaction Table CH.COOH (aq) + H20(0) CH,COO (aq) + H2O (ag) Initial Change Equilibrium b. By using the concentration values at equilibrium in the reaction...
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O...
IV. Comparing Buffering Capacity A. pH of Pure Water i. Measure out 30.0 mL DI H2O into a beaker. 1. Calculate the expected pH of pure water. pH ________ 2. Measured pH of pure water. pH ___3.88______ 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error __________ B. pH of Water and Strong Acid i. Measure out 30.0 mL DI H2O and 2.0...
Experiment VII: Buffers Lab Report ( 49 pts) I. Determination of the K, of acetic acid 1. Measured pH of the solution PH 2.40 < Calculate the [H3O*) at equilibrium for this solution. (include units) Tog [HT] = 10-2.40 H 0% 0.004 m. 3. Calculate the [CH,C00] at equilibrium for this solution. (include units) [CH.CO01 0.004 m 4. What is the [CH3COOH) at equilibrium for this solution? (include units) 700. [CH.COOH): 0.00lem 5. Based on these values, what the acid...
d (HCH3 CO2) is 1.8 × 10- e acid dissociation K of acetic aci Th Calculate the pH of a 2.6 × 10-4M aqueous solution of acetic acid. Round your answer to 2 decimal places.
LUULISI Part B: Determination of K. of Acetic Acid 3. Record the measured pH of vinegar (acetic acid). Measured pH (2pts) 2.5 a. Calculate the concentration of hydronium ions [H:0") of vinegar from the measured pH values. Express your answer in two significant figures for this question (although it is not correct to do so. Show your work. (10 pts) 4. The concentration of distilled white vinegar is written as 5% (w/v) of acetic acid (CH,COOH), Convert the concentration units...
I need help with the problem in the last photo.. I thought I’d
post my lab explanation and data if that helps you get a better
understanding, but it’s just the question at the end. I know I need
to use the Henderson Hasselbach equation.. so... 4.70 = pKa + log(
[acetate-ion] / [acetic-ion] ) and solve for pKa, then Ka.. but how
do I find the concentrations to put in the log fraction?
Thanks, in advance!
Learning Objectives: 1....
F. pH of Buffer after the addition of the Strong Base 1. Calculate the expected pH of this solution. 50.0 mL buffer + 2.0mLION NAOH pH 2. Measured pH of this solution. pH 4.59 3. What is the percent error between the calculated and measured value? What are some of the possible sources of this error? % error pH of Buffer after the addition of the Strong Base: ix. Measure out 50.0 ml the buffer in part D and 2.0...
You are given 75 mL of 0.70 M acetic acid/acetate buffer to test. The starting composition of the two major species are: Concentration of CH,COOH: 0.250 M Concentration of CH,COO: 0.450 M a. Calculate the initial pH of the buffer. Clearly show all work required to arrive at your answer. b. You add 1.0 mL of 2.00 M HCl to the buffer. Calculate the molarity of H, O' added as HCl, and the final molarities of acetic acid and acetate...
4. Calculate the pH of a buffer solution prepared by mixing 10.0 mL of a 0.50 M CH,CO;H and 10.0 mL of a 0.50 M CHCO Na. Record this pH in Part II data sheet, Beaker #1 & N2 for Theoretical Initial pH. K for CHCOH = 1.8 x 10 at 25°C. a. Calculate the pH of the buffer solution upon addition of 0.25 mL of a 6.0 M HCL Record in Part Il data sheet, for Theoretical Final pH...
please answer the questions thank you
Name: Lab Section: Date: Experiment VII: Buffers Review Questions (23 pts) 1. (3 pts). A solution is prepared by mixing 25.0 mL 0.45 M NaCH,coo and 30.0 mL 0.38 M CH,COOH is prepared. Calculate the pH of this solution if the K, 1.76 x 10 for acetic acid. 2. (3 pts)How many grams of sodium lactate, NaCsHsOs, should be added to 1.00 L of 0.150 M lactic acid, HCsHsOs, to form a buffer solution...
a. Using the initial concentration of CH,COOH (from Problem 3) and the equilibrium concentration of H,0 calculated (from Problem 4), complete the reaction table for vinegar. Ignore the column under H:O() (shaded in gray). Don't forget to write a sign (+ or -) for the "Change” row entry. (9 pts: each entry is 1 pt.) Reaction Table CH.COOH (aq) + H20(0) CH,COO (aq) + H2O (ag) Initial Change Equilibrium b. By using the concentration values at equilibrium in the reaction...
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