The Buffer-pair equation allows us to O Calculate the pka of an acid from the pH of a solution of an acid O Calculate the pH of the solution of an acid from the pKa of the acid Calculate the molar ratio of an acid from the pka of its conjugate base O Calculate the molar ratio of an acid and its conjugate base from the pka of the acid and the pH of the solution of the acid O Calculate the pH of the solution of a base from the pka of its conjugate acid

The Buffer-pair equation allows us to O Calculate the pka of an acid from the pH of a solution of an acid O Calculate the pH of the solution of an acid from the pKa of the acid Calculate the molar ratio of an acid from the pka of its conjugate base O Calculate the molar ratio of an acid and its conjugate base from the pka of the acid and the pH of the solution of the acid O Calculate the pH of the solution of a base from the pka of its conjugate acid

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 97QRT

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Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base? The pH will always be greater than 7, regardless of the acid and conjugate base. The pH of the solution will be equal to the pKa of the acid. The pH of the solution will be equal to Kw. The pH will be equal to the concentration of the conjugate base. The pH will be equal to the concentration of the acid.
One of the factors that can affect the pH of a buffered solution is the molar ratio of the conjugate base and weak acid. Which of the following statement is correct? "If the concentration of the conjugate base is higher than the weak acid, the pH will be less than the pKa." "If the concentration of the conjugate base is less than the weak acid, the pH will be less than the pKa." "If the concentration of the conjugate base is higher than the weak acid, the net change of the pH is going to the acidic side (lower pH)" "If the concentration of the conjugate base is less than the weak acid, the net change of the pH is going to the basic side (higher pH)"
Consider a buffer solution containing HCN and NaCN where the concentration of HCN is double the concentration of NaCN. Which statement about the buffer solution is true? (A) The pH of this solution is equal to the pK, value of HCN. (B) The pKa value of HCN will decrease if a strong acid is added. (C) The cyanide ion concentration will increase if a strong base is added. (D) The buffer capacity of this solution will improve if a strong acid is added.
A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is the pKa of the solution would it be considered a buffer
Acetic acid (pK, = 4.76) was dissolved in an aqueous solution buffered to a pH of 5.76. Determine the ratio of the concentrations of acetate ion and acetic acid in this solution. Which species predominates under these conditions? O The acid predominates, because the ratio of [acetate ion]/[acetic acid] = 0.01. O Neither species predominates, because the ratio of [acetate ion]/[acetic acid] = 1. O The conjugate base predominates, because the ratio of [acetate ion]/[acetic acid] = 10. The conjugate base predominates, because the ratio of [acetate ion]/[acetic acid] = 100. %3D O The acid predominates, because the ratio of [acetate ion]/[acetic acid] = 0.1.
An analytical chemist Is titrating 150.5 mL of a 0.1400M solution of aniline (CH,NH,) with a 0.4000M solution of HNO,. The p K, of aniline is 9.37. Calculate the pH of the base solutlon after the chemist has added 17.1 mL of the HNO, solution to It. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. 3. Round your answer to 2 decimal places. pH = || Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibilit hp -> Ce esc & @ #3 $4 8. 1 3 4 t y W tab
Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base? O The pH of the solution will be equal to Kw. The pH will be equal to the concentration of the conjugate base. O The pH of the solution will be equal to the pka of the acid. O The pH will always be greater than 7, regardless of the acid and conjugate base. The pH will be equal to the concentration of the acid.
What will be the pH of a solution when 200ml of 0.1M HEPES in the basic form and 100mL of 0.1 M HEPES in the acid form are mixed together? The pKa of HEPES is 7.55
The pH of a solution that is 0.5 in MA and 0.3 in HA is 5.40; determine the pKa of the acid.
Calculate the pH of a blood plasma sample with a total CO, concentration of 25.7 mM and bicarbonate concentration of 24.4 mM. The relevant pKa of carbonic acid is 6.1 Enter the answer with three significant figures pH 6.077 Hyperventilating can result in a decrease in CO, (g) concentration in the blood. How would this affect the pH of the extracellular fluid? The pH increases The pH does not change appreciably The pH decreases