[Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution is 0.337 M in H₂S and 0.280 M in NaHS. If Kal for H₂S is 1.0 x 10-7, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group No more group attempts remain

[Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution is 0.337 M in H₂S and 0.280 M in NaHS. If Kal for H₂S is 1.0 x 10-7, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group No more group attempts remain

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 2ALQ: A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt...

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Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is -320.1 kJ/mol. (a) What is the pH of a 0.100 M solution of HF at 100C? (b) Compare with the pH of a 0.100 M solution of HF at 25C.
The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.
You add 0.979 g of Pb(OH)2 to 1.00 L of pure water at 25 C. The pH is 9.15. Estimate the value of Ksp for Pb(OH)2.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
Which base in Table 14.3 is must appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or base? Explain.