Question

PH. OF of pH 5.00. Acetic decrease in pH? What Example 6. (a) It is desired to prepare 100 ml of a buffer of pH 5.00 benzoic,

5.10 = 4.74 - log 18x + 1 x - 1 Solving gives x = 6.6 mmol, and 1.8x = 11.9 mmol. The molar concentrations are then [HOAc] =

how it is solved that problem, there it is the answer, but I tried many steps and I cant get that results. please provide step by step. thank you

0 0
Add a comment Improve this question Transcribed image text
Answer #1

AcOH + ou - AO + H₂O on addition of base, ph would x 1 1.82 increases, pr-5.00 +0.10 = 5.10 t- newequili. x.) - 1.8x+1 5.10=4

Add a comment
Know the answer?
Add Answer to:
how it is solved that problem, there it is the answer, but I tried many steps...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

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
  • 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...

  • With this how I calculate the Ammonia solutions pH and Ammonia Buffer solutions ph B. Preparation...

    With this how I calculate the Ammonia solutions pH and Ammonia Buffer solutions ph B. Preparation of Ammonia-Ammonium Buffer Solution Note that an ammonia buffer contains the conjugate base, ammonia, and its conjugate acid, the ammonium ion, NH typically added as NH,CI. Accordingly, the pk, value stated in Eq. (7) is that of the buffer's conjugate acid, NH.. For ammonia, pk, -log (1.8 x 107 4.74. (Note that the fact that the pk for NH, is the same value as...

  • With this information what is the PH of the .1 M acetic acid sol and .1...

    With this information what is the PH of the .1 M acetic acid sol and .1 M acetic acid buffer sol? Please help solutions to observe that buffers resist pH changes. Burette readings should be made to the nearest 0.1 mL (or 0.05 mL if possible), A. Preparation of Acetic Acid-Acetate Buffer Solution An acetate buffer contains the acid-base pair, acetic acid and the acetate ion (typically added as sodium acetate). For acetic acid, pK, = -log (1.8 x 10-)...

  • dont know how to calculate moles of HoAc and the ratio and the bottom table. please...

    dont know how to calculate moles of HoAc and the ratio and the bottom table. please help. 50 Postlaboratory Exercise ratory Exercise Used Mtor poldle on graph Have this page available for your class session after completing your report. (Do not attach it to your report.) the pH, ml, and moles NaOH columns only, before class (moles - M Calculate the equivalence point values first. note about significant figures: When a decimal number is converted to a log, the number...

  • I added everything thing. this is the lab question you need to solve. First assigned buffer...

    I added everything thing. this is the lab question you need to solve. First assigned buffer pH: 2.031 Second assigned buffer pH: 9.171 Available Buffer Systems (acid/ base) pka of Conjugate Acid 2.847 4.757 malonic acid/ monosodium malonate acetic acid/ sodium acetate ammonium chloride/ ammonia triethylammonium chloride/ triethylamine 9.244 10.715 1) Buffer system details: Given pH Name and volume conjugate acid Name and volume conjugate base 2) Calculations for preparation of high capacity buffer system. Introduction In this experiment, you...

  • 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...

  • Part A You need to produce a buffer solution that has a pH of 5.14. You...

    Part A You need to produce a buffer solution that has a pH of 5.14. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pk of acetic acid is 4.74 Express your answer numerically in millimoles. View Available Hint(s) V AED ROO? mmol acetate Pall A beaker with 1 90x102 mL of an acetic acid buffer...

  • Question two A buffer solution is able to maintain a constant pH when small amounts of...

    Question two A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 ml solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O2. The initial concentration of both the acid and the base are 0.0100 mol/0.1000...

  • Please answer all parts. 4. Buffer capacity refers to the amount of acid or base a...

    Please answer all parts. 4. Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can "absorb five times as much acid or base as a 0.1 M buffer for a iven p calculate the new pH after a particular quantity of acid or base is ad You are given 60...

  • the answer is not "not change" and "of the salt" i tried that answer an it...

    the answer is not "not change" and "of the salt" i tried that answer an it was incorrect. A buffer solution that is 0.301 M in CH, COOH and 0.301 M in CH3COONa has a pH of 4.74. The addition of 0.01 mol of H, 0 to 1.0 L of this buffer would cause the pH to not change The capacity of this buffer for added H30+ could be increased by the addition of 0.112 mol of the salt A...

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