1. Calculate the pH of the following solutions:A. [H+] = 1.36 x 10-9 MВ. [ОН] —D 3.86 x 10-8 М2. Calculate the pOH of the following solutions:A. [OH-] = 8.6 x 10-8 MВ. рH %3D 3.23. What is the pH of a buffer prepared by mixing 100 ml 0.050 mM NAH2PO4 and 25 ml0.075 mM Na2HPO4?(рКa1%32.2; рКо23 7.21; pКаз312.7)

1A- ph= -logH+ = -log 1.36 × 10^-9 = 9- log 1.36 pH=9-0.133 = 8.867 1B- pOH = -logOH- = -log…

Answered: 1. Calculate the pH of the following…

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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Consider a pH titration curve at 298 K for 50 mL of 0.10 M hypobromous acid, HBrO (Ka = 2.8 x 10−9), titrated with 0.10 M KOH solution. a. What volume of KOH is needed to reach the half-equivalence point? b. Calculate the pH of the HBrO sample at the half-equivalence point. c. Calculate the equivalence point pH. d. Identify a satisfactory pH indicator for the equivalence point. The pH range of colour change is indicated in parentheses. A) Methyl orange (3.0 - 4.3) B) Bromocresol purple (5.0 - 6.5) C) Alizarin yellow R (10.0 - 12.0) D) Methyl red (4.2 - 6.2)
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Work out the following problems:a. Will an H bond form between H3C—CH=O and H2O? Draw asimple figure to support your answer.b. Draw the following molecules and determine which are polar:Cl2, NH3, CH4.c. What is the pH of a solution with a concentration of0.00001 moles/ml (M) of H+?
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Example The reference range for blood pH is 7.35 – 7.42. What is this range expressed as [H+] in nmol l-1? Calculation: pH = - log [H+] 7.35 = - log [H+] [H+] = antilog -7.35 = 4.47 x 10-8 mol.l-1 = 44.7nmol.l-1 similarly: pH 7.42 = 38.0 nmol.l-1 Range [H+] = 38 – 44.7 nmol.l-1 If the blood pH decreases in an acidosis from 7.42 to 7.15, what is the change in [H+] in nmol.l-1? so this is example on the worksheet, but i still understand how to answer the question.
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1. Calculate the pH of the following solutions: A. [H+] = 1.36 x 10-9 M B. [OH] = 3.86 x 10-8 M 2. Calculate the pOH of the following solutions: A. [OH] = 8.6 x 10-8 M B. pH = 3.2 %3D