Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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4. Human blood is slightly basic in nature with a normal pH range of 7.35-7.45. The blood pH
is maintained by the carbonic acid-bicarbonate buffer system, shown by the following
equilibrium reaction.
H2CO3 + H2O
H,O* + HCO3
a) If you add a small amount of an acid to this buffer, then which component of the carbonic
acid-bicarbonate buffer will react with the added acid? Explain.
solution. Methylamine is a weak base with K = 4.4 x 104. What mass of
A chemistry graduate student is given 125. mL of a 1.80M methylamine (CH₂NH₂):
CH3NH₂Cl should the student dissolve in the CH₂NH₂ solution to turn it into a buffer with pH = 10.95?
You may assume that the volume of the solution doesn't change when the CH3NH₂Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to
2 significant digits.
M
buffer with pH=4.5? K,
5. a)
Calculate the pH of the buffer solution made by mixing 200.0 mL of 0.100 mol/L acetic acid,
CH₂COOH, and 400.0 mL of 0.100 mol/L sodium acetate, CH,COONa. K₁=1.8 x 10.
What will the pH change to if 1.00 mL of 12.0 M HCl is added?
b)
B
1.
8.83
D. 2. a) 4.12
b) none
Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- A buffer solution is prepared by dissolving 1.50 g each of benzoic acid, C6H5CO2H, and sodium benzoate, NaC6H5CO2, in 150.0 mL of solution. (a) What is the pH of this buffer solution? (b) Which buffer component must be added, and in what quantity, to change the pH to 4.00? (c) What quantity of 2.0 M NaOH or 2.0 M HCl must be added to the buffer to change the pH to 4.00?arrow_forwardA good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetatearrow_forwardA 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.) (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of nitric acid is required to reach the equivalence point? (d) What is the pH of the solution before any HNO3 is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?arrow_forward
- A buffer solution is composed of 1.324 g of KH,PO4 and 4.362 g of Naz HPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass =arrow_forward3. What is the pH of a solution that contains 20 grams of sodium hydroxide (NaOH) dissolved in 5.5 liters of solution? 4. What is the pH of a buffer solution that is 0.25 M in HF and 0.10 M in NaF? (Ka for HF is 6.8 x 10-4)arrow_forward4. Formic acid, HFor, has a K value of 1.8 x 104. You need to prepare 125 mL of a buffer hav- ing a pH of 3.25 from 0.10 M HFO solution and a 0.10 M NaFor solution. How many mL of NaFor and HFO should be mixed to make the desired buffer? mL NaFor mL HFOarrow_forward
- bha A buffer prepared by dissolving oxalic acid dihydrate (H2C2O4·2H2O) and disodium oxalate (Na2C2O4) in 1.00 L of water has a pH of 5.333. How many grams of oxalic acid dihydrate (MW = 126.07 g/mol) and disodium oxalate (MW = 133.99 g/mol) were required to prepare this buffer if the total oxalate concentration is 0.241 M? Oxalic acid has pKa values of 1.250 (pKa1) and 4.266 (pKa2).arrow_forwardWhat is the pH of the buffer solution that contains 2.0 g of NH4Cl in 250 mL of 0.050 M NH3? Is the final pH lower or higher than the pH of the 0.050 M ammonia solution? ( K for ammonia is 1.8 x 10-5.) pH of the buffer= The final pH is than the pH of the 0.050 M ammonia solution.arrow_forward4 b A chemistry graduate student is given 450. mL of a 0.70M methylamine (CH3NH₂) solution. Methylamine is a weak base with K = 4.4 × 10 What mass of CH3NH₂Cl should the student dissolve in the CH3NH₂ solution to turn it into a buffer with pH = 10.16? You may assume that the volume of the solution doesn't change when the CH3NH₂Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. □ x10 X Sarrow_forward
- A buffer solution contains 1.250 mol of phenol, C6H5OH, and 0.950 mol of sodium phenoxide, C6H5ONa, in 1.00 L of solution. Ka = 1.30 x 10-10. a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.525 mol of NaOH? (assume no volume change upon the addition of the NaOH) c. To the buffer produced in part a, what is the pH of the buffer after the addition of 0.225 mol of HCl? (assume no volume change up the addition of the HCl)arrow_forwardA buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium formate, HCOONa in enough water for a total volume of 1.00L. The Ka of formic acid is 1.87 x 10-4 a. What is the pH of this buffer? b. If 0.075 mol HCI is added to this buffer, what is the pH of the resulting buffer? (assume no volume changes) c. If 0.055 mol NaOH is added to this buffer, what is the pH of the resulting buffer? (Assume no volume changes)arrow_forwardA butanoic acid/potassium butanoate (C,H,COOH/KOOCC,H,) buffer is prepared to 1.12x10-2 mol L1CH,COOH and 8.38x10-3 mol L1 KOocC;H. The K, for butanoic acid is 1.5x10-5. What is the pH of the buffer solution? Part A O 4.82 O 4.70 O 5.25 O 4.65 O 4.95 o o o o oarrow_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY