3. Normally the pH of the human body is fixed in a very narrow rangebetween 7.35 and 7.45. A patient with an acidotic blood pH of 7.3 maybe treated with an alkali such as sodium hydrogen carbonate. Whywould this treatment raise the pH of the blood?

pH stands for potential of hydrogen. It measures the concentration of hydrogen ions present in the…

Answered: 3. Normally the pH of the human body is…

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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2. Which of the following is a buffer? Why or why not? Can you give the components responsible for its buffering action? a. Stomach acid b. Blood c. Egg White d. Sea Water e. Bleaching Solution
Ions will flow _________ a concentration gradient. Around Up Down Parallel to
19. Blood pH varies between 7.35 and 7.45, with a targeted value of 7.4. If someone's blood pH begins to decrease, chemoreceptors detect this change and send the information to the brain. The brain analyzes the input and sends out a command to the respiratory muscles, causing breathing rate to increase, which reduces carbon dioxide levels, and thereby increases the pH of her blood. Name the body part, value(s), or actions in this specific scenario involving pH. Normal range: Set point: Stimulus: Receptor: Integrating center: Effector: Response:
9. What is the pH of a neutral solution? 10. Describe an example of an acid or a base that is involved in human digestion.
I am unsure how to answer question number 2: What volume of 0.100 M HCl would have to be added to this buffering system, to reduce the pH to 7.1?
4. In a solution, the medium in which atoms/ions/molecules are dispersed is the and the dispersed substances are called the pH Scale
8. At 100 °C, 1.00 gram of liquid water has a volume of 1.043 mL. What volume will 1.00 gram of water vapor occupy at 100 °C at a pressure of 1.00 bar? What is the percent volume change in the the sample?
6. From the titration curve at the right, determine a. If the acids/bases are strong or weak b. Whether the acid or base was added from the buret c. The volume required to reach the equivalence 13 11 9 pH 7 5 3 1 5 10 15 20 d. The pH of the equivalence point e. The region where buffering occurs f. The volume and pH at the half equivalence point g. The K of the base used Volume added (mL) 25 25 h. The region where the [B]: [BH+] ratio is greater than 1 i. The region where the [B]: [BH+] ratio is less than 1 j. The concentration of acid if the titration started with 50.0 mL of 0.050 M base. k. Suggest a good indicator to use for this titration and explain why.
18.Which of the following is true? A. When acid is added to pure water, kw, the ion-product constant of water, changes. B. The equilibrium constant of water (keq) is the rate that dissociation of the molecule occurs at room temperature C. The H* (or H³O*) in cells is the same concentration as that of undissociated water D. None of the above E. All of the above
In the human body,the -log of the hydrogen ion concentration ([H+]) is regulated by a. pH b. Acidity c.Alkalinity d.Bicarbonate ion e. Buffer system
I need to calculate the total change in pH
2. Calculate the pH of a buffer containing 0.1 M sodium acetate and 0.2 M acetic acid (pKa = 4.76).

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3. Normally the pH of the human body is fixed in a very narrow range between 7.35 and 7.45. A patient with an acidotic blood pH of 7.3 may be treated with an alkali such as sodium hydrogen carbonate. Why would this treatment raise the pH of the blood?