I am extremely confused as to the logic behind these conceptual/theory problems can you please add a lot of detail: Consider a buffer solution where [weak acid] > [conjugate base]. How is the pH of the solution related to the pka value of the weak acid? If [conjugate base] > [weak acid], how is pH related to pka?

I am extremely confused as to the logic behind these conceptual/theory problems can you please add a lot of detail: Consider a buffer solution where [weak acid] > [conjugate base]. How is the pH of the solution related to the pka value of the weak acid? If [conjugate base] > [weak acid], how is pH related to pka?

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 55P

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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.
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)"
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.
If a buffer solution contains 2.1 M acetic acid and 2.7 M sodium acetate, what is the pH of the buffer if the K, of the acetic acid is 1.8 x 10-5. Round to 2 decimal places. Your Answer: Answer
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.
The ability of a solution to resist changes to the pH from added acid or base depends upon the amount of weak acid and weak base. The buffering capacity is the ratio of weak acid to weak base and the best buffering occurs when these are equal, making the buffering capacity equal to 1. In the above buffer the buffering capacity is the ratio of [H2PO4-1] to [HPO4-2], or Ka [H2PO4-1] Ka (4.44 x 10-5) Ka (8) [H3O+1] = ––––––––––––– = –––––––––––––––– = ––––––––– [HPO4-2] (5.55 x 10-5) (10) Here the buffering capacity is close to 1 (0.8) and so the buffering capacity is Blank 1. Fill in the blank, read surrounding text. When the buffering capacity is 1, the [H3O+1] = Ka and the pH = pKa This helps chemists choose the right buffer for the needed pH. To buffer at pH = 7, the weak acid should a pKa of close to 7, True or False ? Blank 2. Fill in the blank, read surrounding text. the weak…
The potentiometric titration of a weak base against a stong acid is shown below. In the following problems, calculate the pH at different stages of the titration using the appropriate chemical equation & formula and then select the appropriate answer. Example of answer: Between pH 8 and 9. (no decimals) - Between what is the pH of the solution after 40.00 mL strong acid has been added? - Between what is the pH of the solution after 50.00 mL strong acid has been added? - Between what is the pH of the solution after 60.00 mL strong acid has been added?
The fumarate ion is a dibasic base with pKb values of 9.52 and 10.98. What is the concentration of the fumarate ion (B) in a 0.100 M solution of disodium fumarate that is buffered at pH 5.21? SOLVE FOR CONCENTRATION NOT PH
a) Calculate the pH of a solution 0.145M with respect to CH3CH2COOH and 0.115M with respect to K+CH3CH2COO-. Ka=1.3*10-5; pKa=4.89 b) Calculate the pH of the same solution after adding 0.015M KOH c) Calculate the pH of the same solutions as in part (a) but after addition of 0.015M HBr
7 of 21 I Review | Constants | Periodic Table Part A You need to produce a buffer solution that has a pH of 5.21. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer numerically in millimoles. • View Available Hint(s) ΑΣφ mmol acetate
An analytical chemist is titrating 170.2 mL of a 0.7700M solution of aniline (C H,NH,) with a 0.3200M solution of HIO3. The p K, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 214.4 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. pH = |
Directions: Read and analyze the following questions and compute for is unknown in the given problem. 1. Calculate the pH of a buffer made up of 0.544M CH3NH2 and 0.678M CH:NH3°CI- Ka of CH:NH2 is 1.8 x 105. The buffer is made up of CH3NH2 (weak base) and CH3NH3 CI (salt or conjugate acid) 2. Calculate the pH of buffer made of 0.500M NH3 and 0.456M NH.CI, pKo NH3 = 4.74. 3. Calculate the pH of a buffer solution consisting of 0.96OM NH3 and 0.608M NH4". The Ko for NH3 = 1.8 x 105. The reaction is: NH3 + H2O = NH + OH" item 2 and 3