ZuoTi.Pro
Question

I've been having some trouble with answering this portion of an Ionization of Acids lab that...

I've been having some trouble with answering this portion of an Ionization of Acids lab that I finished up last week and would REALLY appreciate some guidance/help:

In this section of the experiment we were told to weigh out approximately ~0.5g and ~1.5g samples of anhydrous sodium acetate, then measure 50.0mL of 0.100M acetic acid into a 100mL beaker. From here we measured the pH of the solution, then dissolved the ~0.5g and measured the pH again, and finally one more pH measurement with the ~1.5g added to the same solution.

The question is related to this table below:

1. Calculate the total concentrations of added sodium acetate and record these in a table like the following when finished. (Consider the measured pH values and the fact that sodium acetate completely dissolves in water to give Na+ and C2H3O2-, calculate the actual concentrations of these two ions and acetic acid in the solution.

The amount of grams I added for the ~0.5 was 0.59g, and the amount that I added for the ~1.5 was 1.47g

Total Concentration of Acid

Total Concentration NaC2H3O2

pH

[H3O+]

[C2H3O2-]

[HC2H3O2]

0.100 M

0

2.88

0.100 M

4.75

0.100 M

5.33

Thanks a lot for the help ahead of time. If I'm missing any information please let me know!

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

I hope it helps. For further information please ask in comments.

0 0
Add a comment
Know the answer?
Add Answer to:
I've been having some trouble with answering this portion of an Ionization of Acids lab that...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • During this part #3 of the lab, you will make 2 acetic acid buffer solutions (HC2H3O2/NaC2H3O2)...

    During this part #3 of the lab, you will make 2 acetic acid buffer solutions (HC2H3O2/NaC2H3O2) of the same pH (pH = 4.0), but with different concentration of the components. Use the Henderson -Hasselbalch equation to perform the following calculations. The Ka of acetic acid is 1.8 x 10-5 M. a. Buffer A: Calculate the mass of the solid sodium acetate (NaC2H3O2) required to mix with 100 ml of 0.1 M acetic acid (HC2H3O2), to prepare a pH 4 buffer....

  • How many milliliters of 10.0 M HNO3 solution must be added to a 1.0 L buffer...

    How many milliliters of 10.0 M HNO3 solution must be added to a 1.0 L buffer that is .01 M acetic acid ( HC2H3O2) and .2M sodium acetate (NaC2H3O2) to bring the pH to 5.6? the pKa of acetic acid is 4.75

  • The following information and reaction equation will be used for the folliowing problems. A 120 mL...

    The following information and reaction equation will be used for the folliowing problems. A 120 mL solution of 0.110M acetic acid is going to be titrated with a series of additions of 0.100 M NaOH. (Acetic actic has a Ka= 1.8x10-5) HC2H3O2 (aq) + H2O (aq) <-----> H3O+ (aq) + C2H3O2- (aq) HC2H3O2 (aq) + NaOH (aq) <-----> H2O (aq) + NaC2H3O2 (aq) a) What is the pH of the above system after 66 mL of the 0.100 M NaOH...

  • An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...

    An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab was prepared using the following components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M HC2H3O2 55.0 mL of water If you take half of this solution and add 2 mL of 1.00 M HCl to it, then what is the pH of this new solution?

  • 1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic...

    1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...

  • With this information how would I calculate the pH of .01 M Ammonia solution and the...

    With this information how would I calculate the pH of .01 M Ammonia solution and the pH of .01 M Ammonia buffer solution I need Ph of acetic acid! sorry for the wrong wording! A. Preparation of Acetic Acid-Acetate Buffer Solution An acetate buffer contains the acid-base pair, acetic acid and the acetate fon (typically added as sodium acetate). For acetic acid, pk, = -log (1.8 10 = 4.74. Consider the con ditions that will yield 100 ml of an...

  • Normal blood glucose concentrations are between 70-100 mg% (mg per 100 ml of blood) a. Express...

    Normal blood glucose concentrations are between 70-100 mg% (mg per 100 ml of blood) a. Express this concertation range of blood glucose in mM? b. Convert the concentration obtained in question 3 as mg% How many mL of 0.5 M sodium acetate should be added to 100 mL of 0.1M acetic acid to make a buffer of pH 5.1? Acetic acid pKa 4.76 How many mL of 0.1 M HCl should be added to 100mL of 0.1 M tris base...

  • PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all...

    PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. Write out the chemical equation and equilibrium constant expression (Law of Mass Action) for the acetic acid / acetate ion buffer system. Derive the Henderson-Hasselbach equation for this system. 2. Calculate the pH of a buffer solution made by adding 1.3230 g of sodium acetate trihydrate (NaC,H,O, 3H,O) to 50.00 mL of 0.1652 M acetic acid. Assume there is...

  • 1. Phosphoric acid, H3PO4 is a triprotic acid with pKsı = 2.14 and pKa = 7.20 and pkas 12.38. Dra...

    1. Phosphoric acid, H3PO4 is a triprotic acid with pKsı = 2.14 and pKa = 7.20 and pkas 12.38. Draw the titration curve predicted for 0.1 M phosphoric acid titrated by 0.1 M NaOH. (Assume the volume of acid is 20. mL) 2. The pKb of the acetate ion is 9.25. a. Using this information, calculate the pKa of acetic acid. b. Using the Henderson-Hasselbalch equation, calculate the ratio of the concentration of acetate to acetic acid required to produce...

  • Each beaker in a series contains an identical sample of an acetic acid/sodium acetate buffer. The...

    Each beaker in a series contains an identical sample of an acetic acid/sodium acetate buffer. The pH meter registers a value of 3.55. To each beaker the substance listed is added, and the pH again is measured. Assume this is done such that the total volume of the buffer does not change. In which beaker(s) will the pH remain at 3.55? a. Beaker 1: 0.5 g NaCl is added b. Beaker 2: 0.5 g KOH is added c. Beaker 3:...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT