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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Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution.
What happens to the buffer system if some hydrochloric acid is added to the solution?
The hydrochloric acid reacts with the fluoride ions so the pH decreases only slightly.
The hydrochloric acid reacts with the fluoride ions so the pH decreases significantly.
) The hydrochloric acid reacts with the hydrofluoric acid so the pH increases only slightly.
The hydrochloric acid reacts with the hydrofluoric acid so the pH increases significantly.
What is the number of moles of 10.0 g NH₄Cl?
What is the molar concentration of NH₄Cl?
What is the pH of the buffer solution?
An aqueous solution contains 0.18 M ammonium nitrate.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) more than one can be selected.
0.08 mol HBr
0.18 mol HBr
0.17 mol NH3
0.17 mol Ba(NO3)2
0.04 mol Ba(OH)2
Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- Calculate the pH of these buffers.arrow_forward7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?arrow_forwardExplain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.arrow_forward
- Suppose that an aqueous solution is in equilibrium with solid calcium sulfate and solid barium sulfate. What are the concentrations of calcium ion and barium ion in the solution?arrow_forwardThe solubility product constant for calcium oxalate is estimated to be 4 109. What is its solubility in grams per liter?arrow_forwardWhich of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.arrow_forward
- a.Calculate the pH of a buffer that is 0.1M in lactic acid, C2H4(OH)COOH, and 0.1M in sodium lactate, C2H4(OH)COONa. b.What is the pH of a buffer that is 1M in lactic acid and 1M in sodium lactate? c.What is the difference between the buffers described in parts a and b?arrow_forwardUse the References to acces Which of the following aqueous solutions are good buffer systems? 0.27 M ammonium bromide + 0.37 M ammonia O 0.12 M acetic acid + 0.20 M sodium acetate 0.25 M hydrochloric acid + 0.24 M sodium chloride O 0.15 M sodium fluoride + 0.21 M hydrofluoric acid O 0.39 M hydrocyanic acid + 0.29 M sodium cyanidearrow_forwardAn aqueous solution contains 0.34 M potassium hypochlorite.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) More than one can be selected. 0.34 mol HNO3 0.33 mol KCl 0.17 mol NaOH 0.33 mol HClO 0.17 mol HNO3arrow_forward
- A buffer solution was prepared by adding acetic acid and sodium acetate to prepare half a liter of the solution. If the concentration of the acid is equal to the salt concentration, what is the value of the acid function after adding 0.1 normal, and the volume of 10 ml of sodium hydroxide, and if you know that the acid ionization constant is 1.85 x 10-6 * O 3.54 O 5.68 O 4.87arrow_forwardA buffer solution contains 0.371 Mhydrocyanic acid and 0.449 M potassium cyanide. If 0.0218 moles of hydrobromic acid are added to 150. mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydrobromic acid) pH=arrow_forward6.) A 25.00 mL sample of HCL is titrated with 0.1001 M NaOH. 49.90 mL of base is required to reach equivalence and completely neutralize the sample of acid. a. What is the initial concentration of the acid sample? What is the initial pH? b. What is the pH of the solution at equivalence? What indicator should be used? c. What is the pH of the solution after the addition of 25.00 mL of NaOH?arrow_forward
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