EBK CHEMISTRY:CENTRAL SCIENCE
13th Edition
ISBN: 9780321924520
Author: Brown
Publisher: PEARSON CO
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 3, Problem 12E
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.
Expert Solution & Answer
Learn your wayIncludes step-by-step video
schedule05:20
Students have asked these similar questions
A buffer is prepared by adding 5.0 g of ammonia, NH3, and 20.0 g of ammonium chloride, NH4Cl, to enough water to form 2.50 L of solution. (a) What is the pH of the buffer? (b) Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. (c) Write the complete ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.
A 100.00 mL buffer is prepared by dissolving 1.22 grams benzoic acid (pKa = 4.20, Molar Mass, μ = 122 g/mol) and 2.88 grams sodium benzoate (Molar Mass, μ = 144 g/mol) in an appropriate amount of water.
What is the pH of the buffer solution?
What is the pH of the solution if 10.00 mL of 0.25 M HCl is added?
What is the pH of the solution if 5.00 mL of 0.25 M NaOH is added instead of HCl?
-How many grams of solid ammonium chloride should be added to 1.50 L of a 0.235 M ammonia solution to prepare a buffer with a pH of 9.770 ?grams ammonium chloride = g
-A buffer solution that is 0.473 M in HCN and 0.473 M in NaCN has a pH of 9.40.
The addition of 0.01 mol of OH^- to 1.0 L of this buffer would cause the pH to _________increase slightly,increase by 2 units,decrease slightly,decrease by 2 units or not change.
The capacity of this buffer for added H3O^+ could be increased by the addition of 0.175 mol _________of the weak acid or of the salt.
Please help, thank you.
Chapter 3 Solutions
EBK CHEMISTRY:CENTRAL SCIENCE
Ch. 3.1 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 3.1 - Prob. 3.1.2PECh. 3.1 - Consider a saturated solution of the salt MA3, in...Ch. 3.1 - Prob. 3.2.2PECh. 3.2 - Prob. 3.3.1PECh. 3.2 - Prob. 3.3.2PECh. 3.2 - Prob. 3.4.1PECh. 3.2 - Prob. 3.4.2PECh. 3.3 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 3.3 - Does a precipitate form when 0.050 L of 2.0 × 10-2...
Ch. 3.3 - Under what conditions does an ionic compound...Ch. 3.3 - Prob. 3.6.2PECh. 3.4 - Prob. 3.7.1PECh. 3.4 - The following boxes represent aqueos solutions...Ch. 3.4 - Prob. 3.8.1PECh. 3.4 - Prob. 3.8.2PECh. 3.4 - Prob. 3.9.1PECh. 3.4 - Prob. 3.9.2PECh. 3.4 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 3.4 - Practice Exercise 2 Calculate the pH of a solution...Ch. 3.4 - Calculate the concentration of the lactate ion in...Ch. 3.4 - Practice Exercise 2 Calculate the format ion...Ch. 3.4 - Practice Exercise 1 If the pH of a buffer solution...Ch. 3.4 - Prob. 3.12.2PECh. 3.5 - Prob. 3.13.1PECh. 3.5 - Prob. 3.13.2PECh. 3.5 - Calculate the number of grams of ammonium chloride...Ch. 3.5 - Prob. 3.14.2PECh. 3.5 - Prob. 3.15.1PECh. 3.5 - Determine The pH of the original buffer described...Ch. 3.6 - An acid-base titration is performed: 250.0 mL of...Ch. 3.6 - Prob. 3.16.2PECh. 3.6 - Prob. 3.17.1PECh. 3.6 - Calculate the pH in the solution formed by adding...Ch. 3.7 - Prob. 3.18.1PECh. 3.7 - Prob. 3.18.2PECh. 3.7 - Prob. 3.19.1PECh. 3.7 - Prob. 3.19.2PECh. 3.7 - Prob. 3.20.1PECh. 3.7 - Prob. 3.20.2PECh. 3 - The accompanying graph shows the titration curves...Ch. 3 - Prob. 2ECh. 3 - Prob. 3ECh. 3 - Prob. 4ECh. 3 - Prob. 5ECh. 3 - Prob. 6ECh. 3 - Prob. 7ECh. 3 - Prob. 8ECh. 3 - Prob. 9ECh. 3 - Use information from Appendix D to calculate the...Ch. 3 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 3 - You are asked to prepare a pH = 3.00 buffer...Ch. 3 - You are asked to prepare an pH = 4.00 buffer...Ch. 3 - Prob. 14ECh. 3 - Prob. 15ECh. 3 - Prob. 16ECh. 3 - Prob. 17ECh. 3 - Prob. 18ECh. 3 - Prob. 19ECh. 3 - Prob. 20ECh. 3 - 17.35 The samples of nitric and acetic acids shows...Ch. 3 - 17.36 Determine whether each of the following...Ch. 3 - Prob. 23ECh. 3 - Prob. 24ECh. 3 - Prob. 25ECh. 3 - Assume that 30.0 mL of a M solution of a week base...Ch. 3 - Prob. 27ECh. 3 - Prob. 28ECh. 3 - Prob. 29ECh. 3 - Prob. 30ECh. 3 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 3 - Prob. 32ECh. 3 - Prob. 33ECh. 3 - Prob. 34ECh. 3 - The solubility of two slighty soluble salts of...Ch. 3 - Prob. 36ECh. 3 - 17.52
a. true or false: solubility and...Ch. 3 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 3 - Prob. 39ECh. 3 - Prob. 40ECh. 3 - using calculate the molar solubility of AgBr in a....Ch. 3 - calculate the solubility of LaF3 in grams per...Ch. 3 - Prob. 43ECh. 3 - Consider a beaker containing a saturated solution...Ch. 3 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 3 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 3 - 17.63 Which of the following salts will be...Ch. 3 - For each of the following slightly soluble salts,...Ch. 3 - Prob. 49ECh. 3 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 3 - Prob. 51ECh. 3 - Prob. 52ECh. 3 - Prob. 53ECh. 3 - Calculate the minimum pH needed to precipitate Mn...Ch. 3 - Prob. 55ECh. 3 - Prob. 56ECh. 3 - Prob. 57ECh. 3 - Prob. 58ECh. 3 - Prob. 59ECh. 3 - An unknown solid is entirely soluble in water. On...Ch. 3 - Prob. 61ECh. 3 - Prob. 62ECh. 3 - 17.81
Precipitation of the group 4 cautions of...Ch. 3 - Prob. 64ECh. 3 - Prob. 65ECh. 3 - Prob. 66ECh. 3 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 3 - Prob. 68ECh. 3 - Equal quantities of 0.010 M solution of an acid HA...Ch. 3 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 3 - (a) Define the terms limiting reactant and excess...Ch. 3 - Prob. 72ECh. 3 - Prob. 73ECh. 3 - Prob. 74ECh. 3 - What is the pH of a solution made by mixing 0.30...Ch. 3 - Suppose you want to do a physiological experiment...Ch. 3 - Prob. 77ECh. 3 - Prob. 78ECh. 3 - For each pair of compounds, use Kap values to...Ch. 3 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 3 - Salts containing the phosphate ion are added to...Ch. 3 - Prob. 82ECh. 3 - 17.103 The solubility –product constant for barium...Ch. 3 - Prob. 84ECh. 3 - Prob. 85ECh. 3 - A buffer of what pH is needed to give a Mg2+...Ch. 3 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 3 - Prob. 88AECh. 3 - Prob. 89AECh. 3 - Prob. 90AECh. 3 - Prob. 91AECh. 3 - Prob. 92AECh. 3 - Prob. 93AECh. 3 - Prob. 94AECh. 3 - Prob. 95AECh. 3 - A concentration of 10-100 parts per billion (by...Ch. 3 - Prob. 97AECh. 3 - Prob. 98AECh. 3 - In nonaqueous solvents, it is possible to react HF...Ch. 3 - Prob. 100AECh. 3 - Prob. 101AECh. 3 - Prob. 102AECh. 3 - 17.9 The following graphs represent the behavior...Ch. 3 - Prob. 104AECh. 3 - 17.11 The graph below shows the solubility of a...Ch. 3 - Prob. 106IECh. 3 - Prob. 107IECh. 3 - (a) If an automobile travels 225 mi with a gas...Ch. 3 - Prob. 109IECh. 3 - Prob. 110IECh. 3 - Hydrogen cyanide, HCN, is a poisonous gas. The...Ch. 3 - Prob. 112IE
Additional Science Textbook Solutions
Find more solutions based on key concepts
110. Have each group member choose a set of quantum numbers for an electron in a hydrogen atom. Calculate the w...
Chemistry: Structure and Properties (2nd Edition)
Draw the structures of straight-chain alcohols that have from one to six carbons with an OH group at the end of...
Essential Organic Chemistry (3rd Edition)
A catalyst speeds up a chemical reaction by lowering the activation energy. Sketch Diagram A and draw a second ...
General, Organic, and Biological Chemistry (3rd Edition)
The correct option needs to be identified for molarity. Concept Introduction : Molarity of a solution is the nu...
Living by Chemistry
For Practice 1.1
Is each change physical or chemical? Which kind of property (chemical or physical) is demonst...
Principles of Chemistry: A Molecular Approach (3rd Edition)
In the explosion of a hydrogen-filled balloon, 0.50 g of hydrogen reacts with 4.0 g of oxygen. How many grams o...
Introductory Chemistry (5th Edition) (Standalone Book)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- A buffer solution was prepared by adding 4.95 g sodium acetate to 250. mL of 0.150-M acetic acid. What ions and molecules are present in the solution? List them in order of decreasing concentration. Calculate the pH of the buffer solution. Calculate the pH of 100. mL of the buffer solution if you add 80. mg NaOH. (Assume negligible change in volume.) Write a net ionic equation for the reaction that occurs to change the pH.arrow_forwardConsider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.) a. Calculate the pH of this solution. b. Calculate the pH after 0.10 mole of HCl has been added to the original solution. Assume no volume change on addition of HCl. c. Calculate the pH after 0.20 mole of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH.arrow_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 prepared by adding 0.125 mol ammonium chloride to 500. mL of 0.500-M aqueous ammonia. Calculate the pH of the buffer. If 0.0100 mol HCl gas is bubbled into 500. mL buffer and all of the gas dissolves, calculate the new pH of the solution.arrow_forwardYou want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?arrow_forwardConsider the titration of butyric acid (HBut) with sodium hydroxide. In an experiment, 50.00 mL of 0.350 M butyric acid is titrated with 0.225 M NaOH. Ka HBut=1.5105. (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 sodium hydroxide is required to reach the equivalence point? (d) What is the pH of the solution before any NaOH 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 formed by adding 0.150 moles of solid strontium acetate, Sr(C₂H₃O₂)₂, to 500.0 ml of 0.400 M acetic acid, HC₂H₃O₂ solution. You may assume that the change in volume is negligible upon addition of the solid.Calculate the pH of the buffer solution.Calculate the pH of the buffer solution after the addition of 7.50 ml of 2.00 M NaOH. Acetic Acid: pKa = 4.75 Ka=1.76E-5 M.w.=60.05 g/molarrow_forwardChemistry Buffer solutions can be produced by mixing a weak acid with its conjugate base or by mixing a weak base with its conjugate acid. The Henderson-Hasselbalch equation, pH=pKa+log[base][acid] allows you to calculate the pH of a buffer. Note that molarity, moles, and millimoles are all proportional, so you can substitute the number of moles, or millimoles, for the concentration terms in this formula. Part A You need to produce a buffer solution that has a pH of 5.09. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer numerically in millimoles.arrow_forwarda. A buffer solution contains 0.387 M hydrocyanic acid and 0.409 M potassium cyanide.If 0.0293 moles of perchloric acid are added to 250. mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume change does not change upon adding perchloric acid)pH = ? b. A buffer solution contains 0.329 M KHSO3 and 0.294 M K2SO3.If 0.0527 moles of sodium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume does not change upon adding sodium hydroxide)pH = ? c. A buffer solution contains 0.459 M ammonium chloride and 0.396 M ammonia.If 0.0191 moles of sodium hydroxide are added to 125 mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume change does not change upon adding sodium hydroxide)pH = ?arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
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