For my previous question you answered "So, the molar ratio of the ionic form to the neutral form in the stomach (pH 1) is approximately 1.58\times 10-4, and in the bloodstream (pH 7.40), it is approximately 398.107. This indicates that the ionic form predominates in the bloodstream due to its higher pH compared to the stomach.". Put the values in terms of percentage

For my previous question you answered "So, the molar ratio of the ionic form to the neutral form in the stomach (pH 1) is approximately 1.58\times 10-4, and in the bloodstream (pH 7.40), it is approximately 398.107. This indicates that the ionic form predominates in the bloodstream due to its higher pH compared to the stomach.". Put the values in terms of percentage

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 78AP

See similar textbooks

Similar questions

For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
Consider a weak organic base (nonelectrolyte) with molar mass 281 g/mol. An aqueous solution of the base has a pH of 8.73 and an osmotic pressure of SS mm Hg at 25C. What is Kb for the weak base?
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
A chilled carbonated beverage is opened and warmed to room temperature. Does the pH change and, if so, how does it change?
. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?
Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?
State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species. (a) NH3. (b) HPO4-. (c) Br-. (d) NH4+. (e) ASO43-
The following four diagrams represent aqueous solutions of four different acids with the general formula HA. Which of the four acids is the strongest acid?
Indicate whether each of the solutions in Problem 10-65 is acidic, basic, or neutral. a. 3.5 103 M b. 4.7 106 M c. 1.1 108 M d. 8.7 1010 M
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
Which of the following beakers best represents a container of a weak acid, HA, in water? (Water molecules have been omitted for clarity.)