14. Each of the following mixtures can produce an effective buffer solution EXCEPT:(Explain your answer!)a. NaF and KF.b. NaH2PO4 and NazHPO4.c. NaHCO3 and Na2CO3.d. Na3PO4 and Na2HPO4.e. HNO2 and NANO2.

Buffer solutions are formed when weak acids or weak bases combine with their conjugate base or…

Answered: 14. Each of the following mixtures can…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section18.4: Neutralization

Problem 53SSC

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Similar questions

A best buffer has about equal quantities of weak acid and conjugate base present as well as having a large concentration of each species present. Explain.
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
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?
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.
Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
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?
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
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?
How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00? (Him: Assume a negligible change in volume as the solid is added.)
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?
You dissolve 0.425 g NaOH in 2.00 L of a solution that originally had [H2PO4]=[HPO42] = 0.132 M. Calculate the resulting pH.

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14. Each of the following mixtures can produce an effective buffer solution EXCEPT: (Explain your answer!) a. NaF and KF. b. NaH2PO4 and NazHPO4. c. NaHCO3 and Na2CO3. d. Na3PO4 and Na2HPO4. e. HNO2 and NANO2.