**Buffer Solution Ratio Calculation****Problem Statement:**Calculate the ratio of pyridine (C₅H₅N) to its conjugate acid, the pyridinium ion (C₅H₅NH⁺), in a buffer made of pyridine and the pyridinium ion when the pH of that buffer solution is 4.94. The acid dissociation constant (Kₐ) for the pyridinium ion is 5.60 x 10⁻⁶.**Detailed Explanation:**To solve this problem, one needs to employ the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the pKₐ and the ratio of the concentrations of the conjugate base and the conjugate acid.The Henderson-Hasselbalch equation is given by:\[ \text{pH} = \text{p}K_a + \log \left( \frac{[\text{Conjugate Base}]}{[\text{Conjugate Acid}]} \right) \]Where:- $ \text{Conjugate Base} $ is pyridine (C₅H₅N),- $ \text{Conjugate Acid} $ is pyridinium ion (C₅H₅NH⁺).First, calculate the pKₐ from the Kₐ:\[ \text{p}K_a = -\log(K_a) \]\[ K_a = 5.60 \times 10^{-6} \]\[ \text{p}K_a = -\log(5.60 \times 10^{-6}) \]Then, use the Henderson-Hasselbalch equation to find the ratio of pyridine to the pyridinium ion. This will involve substituting the known values of pH and pKₐ into the equation.Lastly, solve for the ratio:\[ \frac{[\text{C₅H₅N}]}{[\text{C₅H₅NH⁺}]} = 10^{(\text{pH} - \text{p}K_a)} \]Thus, through substitution and calculation, the ratio can be determined.

Answered: Image /qna-images/answer/6efb8c3e-c1aa-4f82-beac-b805a9df6690.jpg

Calculate the ratio of pyridine (C3H,N) to it's conjugate acid, the Pyridinium ion (C3H,NH"), CHN in a buffer made of pyridine CH,NH and the pridinium ion when the pH of that buffer solution is 4.94. K for the pyridinium ion is 5.60 x 106

Calculate the ratio of pyridine (C3H,N) to it's conjugate acid, the Pyridinium ion (C3H,NH"), CHN in a buffer made of pyridine CH,NH and the pridinium ion when the pH of that buffer solution is 4.94. K for the pyridinium ion is 5.60 x 106

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A chemistry graduate student is given 450. mL of a 1.00M chlorous acid (HClO₂) solution. Chlorous acid is a weak acid -2 with K = 1.1 × 10 . What mass of NaClO₂ should the student dissolve in the HClO2 solution to turn it into a buffer with a pH = 1.52? You may assume that the volume of the solution doesn't change when the NaClO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. [] x10 X
An analytical chemist is titrating 152.0 mL of a 0.2100 M solution of benzoic acid (HCH,CO,) with a 0.6700 M solution of NaOH. The p K, of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 29.70 mL of the NaOH solution to it.
An analytical chemist is titrating 64.9 mL of a 0.5800M solution of isopropylamine ((CH3),CHNH2) with a 0.3400M solution of HNO3. The p K, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 69.8 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,3 solution added. Round your answer to 2 decimal places. pH =
In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 24.54 mL of 0.100M H2SO4(aq) is placed in a beaker. After 22.04 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution? Report your answer with 3 sig figs
At 25 °C, the molar solubility of Mg(OH)2 in pure water is 1.4x10-4 mol L-1. Calculate the molar solubility in a buffer medium whose pH is 12.00.
6
A chemistry graduate student is given 500. mL of a 0.70M propanoic acid (HC₂H,CO₂) solution. Propanoic acid is a weak acid with K=1.3 × 10. What mass of NaC₂H,CO₂ should the student dissolve in the HC₂H5CO₂ solution to turn it into a buffer with pH = 4.52? You may assume that the volume of the solution doesn't change when the NaC₂H,CO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 Explanation 83°F Mostly sunny A Check F4 $ X C % Ś F6 4 Q Search F7 & FB alc H F9 F10 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use F11 F12 PrtSc Insert Privacy Center | Accessi 4) Delete Backspace
What accounts for the discrepancy in pH? When you have already dissolved the computed masses of reagents for the buffer in an ample amount of distilled water, and upon checking the pH using the pH meter the pH is less than the target pH.
A chemistry graduate student is given 250. mL of a 0.30M chloroacetic acid (HCH,CICO,) solution. Chloroacetic acid is a weak acid with K= 1.3 × 10 °. What mass of KCH,CICO, should the student dissolve in the HCH,CICO, solution to turn it into a buffer with pH = 2.80? You may assume that the volume of the solution doesn't change when the KCH,CICO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A chemistry graduate student is given 125. mL of a 0.30 M benzoic acid (HC, H;CO,) solution. Benzoic acid is a weak 5 acid with K, = 6.3 × 10 °. What mass of KC,H,CO, should the student dissolve in the HCH,CO, solution to turn it 5. into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the KC,H,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5 1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?
Calculate the molar solubility of Ni(OH)2 when buffered at pH 14.0