QUESTION 9 Consider a buffer NH3/NH4. Fill in the blank using the numbers corresponding to each species. NH3 NH4 Na H20 OH 1 2 3 4 Please note that choices can be used more than once. The basic component of the buffer is The acidic component of the buffer is The reactants of the reaction that occurS when a small amount of sodium hydroxide (NaOH) is added to the buffer solution are and The products of the reaction that occurs when a small amount of NaOH is added to the buffer solution are and

QUESTION 9 Consider a buffer NH3/NH4. Fill in the blank using the numbers corresponding to each species. NH3 NH4 Na H20 OH 1 2 3 4 Please note that choices can be used more than once. The basic component of the buffer is The acidic component of the buffer is The reactants of the reaction that occurS when a small amount of sodium hydroxide (NaOH) is added to the buffer solution are and The products of the reaction that occurs when a small amount of NaOH is added to the buffer solution are and

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 17ALQ

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Blood is buffered mainly by the HCO3 H2CO3 buffer system. The normal pH of blood is 7.40. (a) Calculate the [ H2CO3 ]/[ HCO3 ] ratio. (b) What does the pH become if 15% of the HCO3 ions are converted toH2CO3? (c) What does the pH become if 15% of the H2CO3 molecules converted to HCO3 ions?
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
A certain acetic acid solution has pH = 2.68. Calculate the volume of 0.0975 M KOH required to reach the equivalence point in the titration of 25.0 mL of the acetic acid solution.
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?
A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049 g/mL) must be added to 465 mL of 0.0941 M NaOH solution to obtain such a buffer?
A solution of KOH has a pH of 13.29. It requires 27.66 mL of 0.2500 M HCI to reach the equivalence point. (a) What is the volume of the KOH solution? (b) What is the pH at the equivalence point? (c) What is [K+] and [Cl-] at the equivalence point? Assume volumes are additive.