Concept explainers
You are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and any amount you need of sodium fluoride (NaF).
a. What is the pH of the hydrofluoric acid solution prior to adding sodium fluoride?
b. How many grams of sodium fluoride should be added to prepare the buffer solution? Neglect the small volume change that occurs when the sodium fluoride is added.
Learn your wayIncludes step-by-step video
Chapter 3 Solutions
Chemistry: The Central Science (13th Edition)
Additional Science Textbook Solutions
Chemistry: Structure and Properties (2nd Edition)
Essential Organic Chemistry (3rd Edition)
General, Organic, and Biological Chemistry (3rd Edition)
Living by Chemistry
Principles of Chemistry: A Molecular Approach (3rd Edition)
Introductory Chemistry (5th Edition) (Standalone Book)
- 7. 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_forwardA 5.36-g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L.. (a) What is the pH of this buffer solution?. (b) Is the solution acidic or basic?. (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?arrow_forwardUse Le Chátelier's principle to explain what happens to the equilibrium H2O(l)H+(aq)+OH(aq) when a few drops of HCl are added to pure water.arrow_forward
- Which of the following additions will result in a decrease in the pH of the solution? Adding ammonium nitrate to an ammonia solution. Adding potassium chloride to a hydrochloric acid solution. Adding sodium formate to a formic acid solution.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_forwardLactic acid is a monoprotic acid with the formula C3O3H6. You have a 25.00 mL sample of lactic acid with a concentration between 1.00 M and 3.00 M.To determine the exact concentration of this sample of lactic acid, you decide to perform a titration. What titrant should you use? a. 2.50 M Lactic Acid b. 10.5 M NaOH c. 1.75 M Ethanol d. 1.25 M KOH e. 2.00 M HClarrow_forward
- Which of the following aqueous solutions are good buffer systems? A. 0.22 M nitric acid + 0.24 M sodium nitrate B. 0.14 M hydrofluoric acid + 0.19 M potassium fluoride C. 0.36 M sodium nitrate + 0.21 M calcium nitrate D. 0.32 M ammonia + 0.40 M barium hydroxide E. 0.19 M potassium hydroxide + 0.26 M potassium bromidearrow_forward3. a. You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO, and an 0.68 M solution of NAOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. b. If the acid used in a. was nitric acid, HNO, could the same buffer solution be made? Briefly explain. If the buffer solution prepared in a. also contained ~10°M Ni²* and ~10-6 M Pb²* , could those metal ions be separated from each other by saturating the solution with H,S? Explain your answer by showing the necessary calculations. C.arrow_forwardA 1 liter solution contains 0.514 M hydrocyanic acid and 0.386 M potassium cyanide. What will the addition of 0.193 moles of hydrobromic acid do? (Assume that the volume does not change upon the addition of hydrobromic acid.) *More than one answer is accepted. A. Raise the pH slightly B. Lower the pH slightly C. Raise the pH by several units D. Lower the pH by several units E. Not change the pH F. Exceed the buffer capacityarrow_forward
- A 1.00 liter solution contains 0.59 M ammonia and 0.45 M ammonium bromide.If 0.23 moles of perchloric acid are added to this system,indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of NH3 will increase. B. The number of moles of NH4+ will remain the same. C. The equilibrium concentration of H3O+ will decrease. D. The pH will remain the same. E. The ratio of [NH3] / [NH4+] will remain the same.arrow_forwardConsider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO₂, which provides the conjugate base, HCO,. H_COjlog) + HJO W 7 HyO" loạ) + HCOy loa) How does the buffer react when some base is added? The bicarbonate ion (HCO) of the buffer reacts with the base. OHCO and H₂CO, both react with the base. O The buffer does not react. O The carbonic acid (H₂CO₂) of the buffer reacts with the base Question 15 Indicate whether each of the following reactions is an example of reaction of an acid with a metal, reaction of an acid with a carbonate, or acid-base neutralization reaction using the dropdown on the right. Reaction A: ZnCO3(s) + 2HBr(aq) → ZnBr₂(aq) + CO₂(g) + H₂O(l) Reaction B: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) HCI(g) + NaHCO3(s)→ NaCl(aq) + CO₂(g) + H₂O(0) H₂SO4(aq) + Mg(OH)2(s)→ MgSO4(aq) + 2H₂O(1) 3LIOH(aq) + H₂PO₂(aq) → Li₂PO₂(aq) + 3H₂O(0) Cal(s) + H₂SO4(aq) → H₂(g) + CaSO₂(aq) Reaction C: Reaction D: Reaction E: Reaction Earrow_forwardA 1.00 liter solution contains 0.36 moles hydrofluoric acid and 0.28 moles sodium fluoride .If 0.14 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HF will remain the same. B. The number of moles of F- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will remain the same. E. The ratio of [HF] / [F-] will remain the same.arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning