Not sure about my answers. So I would like to see Half
equivilance point, pKa, Ka and molarity of acid values worked out
from these graphs. Impotant data: titration of 25.00 +/- 0.01 mL of
unknown acid by 0.1069 M NaOh. Two runs were done, but data
calculations for ony one is needed now (they sets are nearly
identical).
.
Homework Answers
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Not sure about my answers. So I would like to see Half
equivilance point, pKa, Ka...
calculations for: concentration of the unknown acid and values for pKa and Ka. Part E: pH...
calculations for:
concentration of the unknown acid and values for pKa and
Ka.
Part E: pH pH pH pH Average Volume Trial 1 Trial 2 Trial 3 5.0 0 5 5.0। 5.1 .0 । 5.1 5.1 5.2 5.3 [5.0। 5.1 5.1 5.1 5.2 5.3 [5.2 5.3 5.3 5.4 5.5 16. 16.5 17.0 | 17.5। 18.0 18.5 19.0 19.5 | 20.0 20.5 21.0 | 21.5 | 22.0 22.5 23.0 23.5 24.0 24.5 | 5.6 5.7 [5.3 [5.4 | 5.5 | 5.6...
I am looking for help with just trial one. I am not sure what equations to use or how to go about even answering these questions. I figure if I can get help with trial 1 I should be able to do trial 2...
I am looking for help with just trial one. I am not sure what
equations to use or how to go about even answering these questions.
I figure if I can get help with trial 1 I should be able to do
trial 2 on my own.
( This week has been really bad, I lost my grandfather, so if you
could "dumb" down the steps as much as possible I would appreciate
it, my brain is just not working...
Not sure if I did number 4 correct. The half way point was 7.89mL with a...
Not sure if I did number 4 correct.
The
half way point was 7.89mL with a pH of 3.42
4) Determine the pK, and calculate the K, of the unknown acid. Mass of Unknown 2.40 g Sample Value Unit Initial burette volume of NaOH 2.00 ml Final burette volume of NaOH 18.00ml Fast Titration #2: I Sample Value Unit Initial burette volume of NaOH 18.00 mL Final burette volume of NaOH 33.8 ml Slow Titration: Volume of NaOH/mL pH volume...
I need help with part c and d please. I would like to see steps to...
I need help with part c and d please. I would like to see
steps to understand.
Equal volumes of two acids are titrated with 0.10M NaOH resulting in the two titration curves shown in the following figure(Figure 1) Figure < 1 of 1 > PH 0 10 20 30 ml NaOH 40 50 Part C To the nearest integer, estimate the pka of the acid that produced the blue curve IV ALQ RO ? Submit Previous Answers Request Answer...
In the second image it states that after I pass the equivalence point, I should add...
In the second image it states that after I
pass the equivalence point, I should add 2ml of aliquots of NaOH
until there's no PH change. How do I identify when the equivalence
point is?
Preparation of the unknown weak acid Select the NaOH and fill the buret with the now standardized NaOH solution. [NaOH]=0.097M Record the initial buret volume in your Notebook. 3 Using the volumetric pipet, transfer 25.00 mL of the unknown weak acid to the Erlenmeyer flask....
I'm doing a titration lab tomorrow and I am not sure what the formulas are to...
I'm doing a titration lab tomorrow and I am not sure what the
formulas are to calculate the moles of NaOH, the moles of
HCl, and the molarity of HCl.
The objective of this laboratory is to determine the molarity of
a hydrochloric acid solution using a known concentration of sodium
hydroxide as the titrant.
volume of HCl in flask: 25.00 mL
the net ionic equation for the reaction is:
H+(aq) + OH-(aq) --> H2O(l)
I don't have the data...
A thorough explanation would sure be appreciated!!!! Thank you!! Acid-Base Chemistry: Unknown Acid Analysis (in two...
A thorough explanation would sure be appreciated!!!!
Thank you!!
Acid-Base Chemistry: Unknown Acid Analysis (in two experiments) Introduction In this experiment you will titrate a monoprotic weak acid with a strong ak acid with a strong base in the nd using a pH meter (Exp 2). An analysis of concentration and molar mass of the the titration data will allow you to determine the concentration and more unknown acid (Exp 1) and the ionization constant Ka (Exp 2). At the...
I dont know how to do this exercise please ignore my answers ME General Chemistry I...
I dont know how to do this exercise please ignore my
answers
ME General Chemistry I Molarity of Acetic Acid in Vinegar: A Titration Experiment NaOH = 40.019/mols NaOH DATA AND CALCULATIONS STANDARDIZATION OF NaOH lesina Check the 2 (at least) trials O O O Check the 2 (at least) trials used to calculate the average molarity. Trial 1 Trial 2 Trial 3 Mass of KHP Moles of KHP 1991/ 37.50 m2 read - 1-0.72893 0 7599 0.75792- 16,59 Initial...
If you could help answer the blanks and check what I have using the graph and info sheet that would be great...
If you could help answer the blanks and check what I have using the
graph and info sheet that would be great.
Questions: 1. Write the chemical reaction that occurs during the titration. NaOH + HCL NaCl + H₂O 2. Locate in the experiment the definition of equivalence point. Write it here. 3. Read the Plotting the Results section in the experiment and locate the equivalence point on the curve you've drawn using the method described. Mark it on your...
DATA AND CALCULATIONS Time at equivalence point (s) Time of color Trial *Equation for acid-base reaction...
DATA AND CALCULATIONS Time at equivalence point (s) Time of color Trial *Equation for acid-base reaction change (s) NaOH+HCI - 21 0s 1 250.5 NaOH+ HC2H3O2- 2 8l.55 99s 3 NH3+ HCl- 930s 4 NH3 + HC2H3O2- 90.55 81.Os Complete the reactions above. Attach copies of all four graphs to this report. 1. 2. Examine the time data for each of the Trials 1- -4. In which trial(s) did the indicator change color at about the same time as the...
calculations for:
concentration of the unknown acid and values for pKa and
Ka.
Part E: pH pH pH pH Average Volume Trial 1 Trial 2 Trial 3 5.0 0 5 5.0। 5.1 .0 । 5.1 5.1 5.2 5.3 [5.0। 5.1 5.1 5.1 5.2 5.3 [5.2 5.3 5.3 5.4 5.5 16. 16.5 17.0 | 17.5। 18.0 18.5 19.0 19.5 | 20.0 20.5 21.0 | 21.5 | 22.0 22.5 23.0 23.5 24.0 24.5 | 5.6 5.7 [5.3 [5.4 | 5.5 | 5.6...
I am looking for help with just trial one. I am not sure what
equations to use or how to go about even answering these questions.
I figure if I can get help with trial 1 I should be able to do
trial 2 on my own.
( This week has been really bad, I lost my grandfather, so if you
could "dumb" down the steps as much as possible I would appreciate
it, my brain is just not working...
Not sure if I did number 4 correct.
The
half way point was 7.89mL with a pH of 3.42
4) Determine the pK, and calculate the K, of the unknown acid. Mass of Unknown 2.40 g Sample Value Unit Initial burette volume of NaOH 2.00 ml Final burette volume of NaOH 18.00ml Fast Titration #2: I Sample Value Unit Initial burette volume of NaOH 18.00 mL Final burette volume of NaOH 33.8 ml Slow Titration: Volume of NaOH/mL pH volume...
I need help with part c and d please. I would like to see
steps to understand.
Equal volumes of two acids are titrated with 0.10M NaOH resulting in the two titration curves shown in the following figure(Figure 1) Figure < 1 of 1 > PH 0 10 20 30 ml NaOH 40 50 Part C To the nearest integer, estimate the pka of the acid that produced the blue curve IV ALQ RO ? Submit Previous Answers Request Answer...
In the second image it states that after I
pass the equivalence point, I should add 2ml of aliquots of NaOH
until there's no PH change. How do I identify when the equivalence
point is?
Preparation of the unknown weak acid Select the NaOH and fill the buret with the now standardized NaOH solution. [NaOH]=0.097M Record the initial buret volume in your Notebook. 3 Using the volumetric pipet, transfer 25.00 mL of the unknown weak acid to the Erlenmeyer flask....
I'm doing a titration lab tomorrow and I am not sure what the
formulas are to calculate the moles of NaOH, the moles of
HCl, and the molarity of HCl.
The objective of this laboratory is to determine the molarity of
a hydrochloric acid solution using a known concentration of sodium
hydroxide as the titrant.
volume of HCl in flask: 25.00 mL
the net ionic equation for the reaction is:
H+(aq) + OH-(aq) --> H2O(l)
I don't have the data...
A thorough explanation would sure be appreciated!!!!
Thank you!!
Acid-Base Chemistry: Unknown Acid Analysis (in two experiments) Introduction In this experiment you will titrate a monoprotic weak acid with a strong ak acid with a strong base in the nd using a pH meter (Exp 2). An analysis of concentration and molar mass of the the titration data will allow you to determine the concentration and more unknown acid (Exp 1) and the ionization constant Ka (Exp 2). At the...
I dont know how to do this exercise please ignore my
answers
ME General Chemistry I Molarity of Acetic Acid in Vinegar: A Titration Experiment NaOH = 40.019/mols NaOH DATA AND CALCULATIONS STANDARDIZATION OF NaOH lesina Check the 2 (at least) trials O O O Check the 2 (at least) trials used to calculate the average molarity. Trial 1 Trial 2 Trial 3 Mass of KHP Moles of KHP 1991/ 37.50 m2 read - 1-0.72893 0 7599 0.75792- 16,59 Initial...
If you could help answer the blanks and check what I have using the
graph and info sheet that would be great.
Questions: 1. Write the chemical reaction that occurs during the titration. NaOH + HCL NaCl + H₂O 2. Locate in the experiment the definition of equivalence point. Write it here. 3. Read the Plotting the Results section in the experiment and locate the equivalence point on the curve you've drawn using the method described. Mark it on your...
DATA AND CALCULATIONS Time at equivalence point (s) Time of color Trial *Equation for acid-base reaction change (s) NaOH+HCI - 21 0s 1 250.5 NaOH+ HC2H3O2- 2 8l.55 99s 3 NH3+ HCl- 930s 4 NH3 + HC2H3O2- 90.55 81.Os Complete the reactions above. Attach copies of all four graphs to this report. 1. 2. Examine the time data for each of the Trials 1- -4. In which trial(s) did the indicator change color at about the same time as the...
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