23. Which of the following combinations would be best to buffer an aqueous solution at a pH of 7.42?a) H3PO4 and H2PO4¯, Ka1 = 7.5 × 10-3b) HNO2 and NO2", Ka = 4.5 x 10c) CH3CO2H and CH3COO", Ka = 1.8 x 10-sd) H2PO4¯ and HPO4²¯, Ka2 = 6.2 × 108e) NH4* and NH3, K, = 5.7 × 10¬10f) none of the above%3D%3D%3D%3D

The buffer is the combination of weak acid/ weak base with its salt from a strong base / strong…

23. Which of the following combinations would be best to buffer an aqueous solution at a pH of 7.42? a) H3PO4 and H,PO, Ka1 = 7.5 x 103 b) HNO2 and NO2", K, = 4.5 x 10 c) CH3CO2H and CH3COO", K, = 1.8 x 10-5 d) H2PO4 and HPO,, Ka2 = 6.2 x 10 e) NHa and NH3, K, 5.7 x 10-10 f) none of the above %3D

23. Which of the following combinations would be best to buffer an aqueous solution at a pH of 7.42? a) H3PO4 and H,PO, Ka1 = 7.5 x 103 b) HNO2 and NO2", K, = 4.5 x 10 c) CH3CO2H and CH3COO", K, = 1.8 x 10-5 d) H2PO4 and HPO,, Ka2 = 6.2 x 10 e) NHa and NH3, K, 5.7 x 10-10 f) none of the above %3D

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.18QAP

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

23. Which of the following combinations would be best to buffer an aqueous solution at a pH of 7.42?
a) H3PO4 and H2PO4¯, Ka1 = 7.5 × 10-3
b) HNO2 and NO2", Ka = 4.5 x 10
c) CH3CO2H and CH3COO", Ka = 1.8 x 10-s
d) H2PO4¯ and HPO4²¯, Ka2 = 6.2 × 108
e) NH4* and NH3, K, = 5.7 × 10¬10
f) none of the above
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Suppose you have an alkaline buffer consisting of 0.20 M aqueous ammonia (NHs) and 0.10 M ammonium chloride (NH4CI). What is the pH of the solution? 5 Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0 x 10-10. How do the concentration/volumes of the buffer affect the buffer capacity? E.g., 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid solution with 25.0 mL of 0.10 M sodium acetate solution).
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