QUESTION 16 Ką of hypobromous acid (HBrO) is 2.2*10-9 (2.2e-9). What is the pH of a buffer that is 0.161 in HBRO and 0.155 in NaBro? Submit your answer in standard notation. You may submit shown work to blackboard. Click Save and Submit to save and submit. Click Save All Answers to save all answers.

QUESTION 16 Ką of hypobromous acid (HBrO) is 2.2*10-9 (2.2e-9). What is the pH of a buffer that is 0.161 in HBRO and 0.155 in NaBro? Submit your answer in standard notation. You may submit shown work to blackboard. Click Save and Submit to save and submit. Click Save All Answers to save all answers.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.7QE

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Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?
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I am extremely confused as to the logic behind these conceptual/theory problems can you please add a lot of detail: Consider a buffer solution where [weak acid] > [conjugate base]. How is the pH of the solution related to the pka value of the weak acid? If [conjugate base] > [weak acid], how is pH related to pka?
I need help calculating the concentration of acid in each buffer solution show in the second picture!!!! ALSO - make sure for the unrounded values there is 6 sig figs!! EXPERIMENTAL DATA Sample HIn (mL) 1.10 M Acetic Acid (mL) 0.90 M Sodium Acetate (mL) 1 10.00 8.00 2.00 2 10.00 7.00 3.00 3 10.00 6.00 4.00 4 10.00 5.00 5.00 5 10.00 4.00 6.00 6 10.00 3.00 7.00 7 10.00 2.00 8.00 8 10.00 1.00 9.00 9 10.00 10.00 mL NaOH (0.10 M) 10 10.00 10.00 mL HCl (0.10 M)
Hello, I have a problem regarding buffer question. Mainly question c, I got 4.83 but I was told that I was wrong? (it's either my answer is wrong or the system is wrong, I doubt that(?)) I just want to know how do I do this question :( For a, I got 4.74 and for b I got 4.65
How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.396 M hypobromous acid, HBrO, to form a buffer solution of pH 8.95? The Ka of HOBr is 2.0 × 10–9. Express your answer in moles using at least three significant figures. Do not use scientific notation.
lets do Calculations System I * 0.010 M HCl * 0.0010 NaOH System II * 0.010 M ( HA ) * 0.0010 M ( B ) System IV * Buffer
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QUESTION 4. A biochemist wants to use X-ray diffraction to determine the structure of a protein. The biochemist must isolate crystals of the protein from solutions buffered to pH 5.20. Acetic acid/acetate ion would be a good choice for the buffer. What would the ratio of [acid]/[conjugate base] need to be in this buffer?