In the course of a hypothetical meal, the stomach expands from 0.25 liters to 1.25 liters. If we assume that no buffering occurs and no acid is produced from the stomach contents, how much acid must be secreted to maintain pH = 1.0? How many grams of ATP would be consumed in the production of that acid?

In the course of a hypothetical meal, the stomach expands from 0.25 liters to 1.25 liters. If we assume that no buffering occurs and no acid is produced from the stomach contents, how much acid must be secreted to maintain pH = 1.0? How many grams of ATP would be consumed in the production of that acid?

Human Physiology: From Cells to Systems (MindTap Course List)

9th Edition

ISBN:9781285866932

Author:Lauralee Sherwood

Publisher:Lauralee Sherwood

Chapter1: Introduction To Physiology And Homeostasis

Section: Chapter Questions

Problem 2TAHL

See similar textbooks

Similar questions

If the cells of your body oxidize 1 mole of glucose, by how much would the temperature of your body (assume that your body consists of 75 kg of water) increase if the heat were not dissipated into the environment?
if pH level of solution changes from pH 5 to pH 2, how much acidity increased in that solution and why?
The greatest buffering capacity at physiological pH would be provided by a protein rich in which of the following amino acids? Choose one from among the possible answers and explain. Serine Cysteine Alanine Histidine
Indicate whether each of the following is due to an increase in pH, a decrease in pH or neither and explain why: __Makes carrots soften more when cooked __Color shifts due to adding chlorine to cake flour __Lowers the amount of iron sulfide formed in hard cooked eggs __Makes anthocyanins more red __Makes an egg white foam more stable __Makes starch dextrinize when heated in boiling water __Raises osmotic pressure
In a 0.1000 M acetic acid solution at 25 degrees celsius , the acid ionizes to the extent of about 1.34 %. Since each molecule of acetic acid which ionizes produces 1 H+ ion and 1 C2H3O2- ion, the concentration in the solution are: HC2H3O2 < -----------> H+ + C2H3O2-
Could the amino acid glycine serve as the basis of a buffer system? If so, in what pH range would it be useful?
Bicarbonate/carbonic acid buffer in blood is an example of an equilibrium reaction that is meant to be very insensitive to change. How does the bicarbonate/carbonic acid buffer re-establish equilibrium if acidity increases? How does the bicarbonate/carbonic acid buffer re-establish equilibrium if alkalinity increases?
Based on the Henderson-Hasselbalch equation (shown below), calculate the pH when half of a solution of acetic acid is dissociated to acetate (the pKa of acetic acid is 4.76). A. 1.00 B. 3.76 C. 4.76 D. 5.76
Biological fluids typically contain compounds known as buffers that function to minimize the effects of changes in H+ and OH- concentrations and the resulting pH changes in a cell. What does a buffer have to do with respect to each of these ions in order to control the pH within the cell? Why are buffers important for living organisms?
Using the data in the table below, calculate the average molar mass of an amino acid residue in each of the proteins in the table (excluding cytochrome c, myoglobin, and hemoglobin). Next, calculate the mean of the mean molar mass considering all proteins (excluding cytochrome c, myoglobin and hemoglobin)
Indicate the ionic species of phosphoric acid that predominates at pH 4, 8, and 11.
Based on the Henderson-Hasselbalch equation (shown below), calculate the pH when the ratio of acetic acid to acetate is 10 to 1 (the pKa of acetic acid is 4.76). A. 1.00 B. 3.76 C. 4.76 D. 5.76