Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 17, Problem 84GQ
A sample of hard water contains about 2.0 × 10−3 M Ca2+. A soluble fluoride-containing salt such as NaF is added to “fluoridate” the water (to aid in the prevention of dental cavities). What is the maximum concentration of F− that can be present without precipitating CaF2?
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
A pink solid has the formula CoCl3·5NH3·H2O. A solution of this solid is also pink in color and when titrated with silver nitrate quickly forms 3 mol of AgCl. Upon heating the pink solid, it loses 1 mole of water and forms a purple solid with the same NH3:Cl:Co ratio. Dissolving and titrating with AgNO3, the purple solid slowly releases one of its chlorides.
a) Derive the formulas of the two octahedral complexes.b) draw and name them.c) write the chemical equations of all described reactions.
What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?
A 50.0 mL solution of Ca(OH) 2
with an unknown concentration
was titrated with 0.340 M HNO3.
To reach the endpoint, a total of
26.2 mL of HNO3 was required.
Given that 0.00891 mol of HNO3
are used in the titration, What
quantity in moles of Ca(OH)2 had
to be present in the initial
reaction?
Chapter 17 Solutions
Chemistry & Chemical Reactivity
Ch. 17.1 - You have a 0.30 M solution of formic acid (HCO2H)...Ch. 17.1 - 1. What is the pH of the solution that results...Ch. 17.2 - What is the pH of a buffer solution composed of...Ch. 17.2 - Use the Henderson-Hasselbalch equation to...Ch. 17.2 - Using an acetic acid/sodium acetate buffer...Ch. 17.2 - Calculate the pH of 0.500 L of a buffer solution...Ch. 17.2 - 1. Which choice would be a good buffer...Ch. 17.2 - 2. If an acetic acid/sodium acetate buffer...Ch. 17.2 - Prob. 3RCCh. 17.2 - 4. To prepare a buffer containing CH3CO2H and...
Ch. 17.3 - The titration of 0.100 M acetic acid with 0.100 M...Ch. 17.3 - Calculate the pH after 75.0 mL of 0.100 M HO has...Ch. 17.3 - 1. What is the pH after 25.0 ml of 0.100 M NaOH...Ch. 17.3 - 2. What is the pH at the equivalence point in the...Ch. 17.3 - Prob. 3RCCh. 17.3 - Phosphate ions are abundant in cells, both as the...Ch. 17.3 - A typical total phosphate concentration in a cell,...Ch. 17.4 - The barium ion concentration, [Ba2+], in a...Ch. 17.4 - Calculate the solubility of AgCN in moles per...Ch. 17.4 - Calculate the solubility of Ca(OH)2 in moles per...Ch. 17.4 - Calculate the solubility of BaSO4 (a) in pure...Ch. 17.4 - 12. Calculate the solubility of Zn(CN)2 at 25°C...Ch. 17.4 - What is the Ksp expression for silver carbonate?...Ch. 17.4 - 2. Using Ksp values, predict which salt in each...Ch. 17.4 - What is the solubility of PbSO4 in water at 25C?...Ch. 17.4 - 4. What is the solubility of PbSO4 in water at...Ch. 17.4 - Prob. 5RCCh. 17.5 - Solid Pbl2 (Ksp = 9.8 109) is placed in a beaker...Ch. 17.5 - Prob. 2CYUCh. 17.5 - Prob. 3CYUCh. 17.5 - 1. Will SrSO4 precipitate from a solution...Ch. 17.6 - Silver nitrate (0.0050 mol) is added to 1.00 L of...Ch. 17.6 - 1. Iron(II) chloride (0.025 mol) is added to 1.00...Ch. 17.7 - Calculate the value of the equilibrium constant,...Ch. 17.7 - 1. What is the equilibrium constant for the...Ch. 17.7 - Prob. 1QCh. 17.7 - What is the minimum volume of 0.0071 M NaCN(aq)...Ch. 17.7 - Use the formation constant of [Au(CN)2] in...Ch. 17.7 - Silver undergoes similar reactions as those shown...Ch. 17.7 - Write a balanced chemical equation for the...Ch. 17 - Does the pH of the solution increase, decrease or...Ch. 17 - Does the pH of the solution increase, decrease, or...Ch. 17 - What is the pH of a solution that consists of 0.20...Ch. 17 - What is the pH of 0.15 M acetic acid to which 1.56...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the buffer solution that...Ch. 17 - Lactic acid (CH3CHOHCO2H) is found in sour milk,...Ch. 17 - What mass of sodium acetate, NaCH3CO2, must he...Ch. 17 - What mass of ammonium chloride, NH4Cl, must be...Ch. 17 - Calculate the pH of a solution that has an acetic...Ch. 17 - Calculate the pH of a solution that has an...Ch. 17 - What must the ratio of acetic acid to acetate ion...Ch. 17 - What must the ratio of H2PO4 to HPO42 be to have a...Ch. 17 - A buffer is composed of formic acid and its...Ch. 17 - A buffer solution is composed of 1.360 g of KH2PO4...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Describe how to prepare a buffer solution from...Ch. 17 - Describe how to prepare a buffer solution from NH3...Ch. 17 - Determine the volume (in mL) of 1.00 M NaOH that...Ch. 17 - Determine the volume (in mL) of 1.00 M HC1 that...Ch. 17 - A buffer solution was prepared by adding 4.95 g of...Ch. 17 - You dissolve 0.425 g of NaOH in 2.00 L of a buffer...Ch. 17 - A buffer solution is prepared by adding 0.125 mol...Ch. 17 - What is the pH change when 20.0 mL of 0.100 M NaOH...Ch. 17 - Phenol, C6H5OH, is a weak organic acid. Suppose...Ch. 17 - Assume you dissolve 0.235 g of the weak acid...Ch. 17 - You require 36.78 mL of 0.0105 M HCl to reach the...Ch. 17 - A titration of 25.0 mL of a solution of the weak...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - You titrate 25.0 mL of 0.10 M NH3 with 0.10 M HCl....Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Name two insoluble salts of each of the following...Ch. 17 - Prob. 38PSCh. 17 - Using the solubility guidelines (Figure 3.10),...Ch. 17 - Predict whether each of the fallowing is insoluble...Ch. 17 - For each of the following insoluble salts, (1)...Ch. 17 - Prob. 42PSCh. 17 - When 1.55 g of solid thallium(I) bromide is added...Ch. 17 - At 20 C, a saturated aqueous solution of silver...Ch. 17 - When 250 mg of SrF2, strontium fluoride, is added...Ch. 17 - Calcium hydroxide, Ca(OH)2, dissolves in water to...Ch. 17 - You add 0.979 g of Pb(OH)2 to 1.00 L of pure water...Ch. 17 - You place 1.234 g of solid Ca(OH)2 in 1.00 L of...Ch. 17 - Estimate the solubility of silver iodide in pure...Ch. 17 - What is the molar concentration of Au+(aq) in a...Ch. 17 - Prob. 51PSCh. 17 - Estimate the solubility of lead(II) bromide (a) in...Ch. 17 - The Ksp value for radium sulfate, RaSO4, is 4.2 ...Ch. 17 - If 55 mg of lead(II) sulfate is placed in 250 mL...Ch. 17 - Prob. 55PSCh. 17 - Prob. 56PSCh. 17 - Calculate the molar solubility of silver...Ch. 17 - Calculate the solubility of silver bromide, AgBr,...Ch. 17 - Compare the solubility, in milligrams per...Ch. 17 - What is the solubility, in milligrams per...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Which insoluble compound in each pair should be...Ch. 17 - Which compound in each pair is more soluble in...Ch. 17 - You have a solution that has a lead(II) ion...Ch. 17 - Sodium carbonate is added to a solution in which...Ch. 17 - If the concentration of Zn2+ in 10.0 mL of water...Ch. 17 - You have 95 mL of a solution that has a lead(II)...Ch. 17 - Prob. 69PSCh. 17 - Will a precipitate of Mg(OH)2 form when 25.0 mL of...Ch. 17 - Zinc hydroxide is amphoteric (Section 16.10). Use...Ch. 17 - Solid silver iodide, AgI, can be dissolved by...Ch. 17 - What amount of ammonia (moles) must be added to...Ch. 17 - Can you dissolve 15.0 mg of AuCl in 100.0 mL of...Ch. 17 - What is the solubility of AgCl (a) in pure water...Ch. 17 - Prob. 76PSCh. 17 - Prob. 77GQCh. 17 - Prob. 78GQCh. 17 - Prob. 79GQCh. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - For each of the following cases, decide whether...Ch. 17 - Prob. 83GQCh. 17 - A sample of hard water contains about 2.0 103 M...Ch. 17 - What is the pH of a buffer solution prepared from...Ch. 17 - Prob. 86GQCh. 17 - Describe the effect on the pH of the following...Ch. 17 - What volume of 0.120 M NaOH must be added to 100....Ch. 17 - A buffer solution is prepared by dissolving 1.50 g...Ch. 17 - What volume of 0.200 M HCl must be added to 500.0...Ch. 17 - What is the equilibrium constant for the following...Ch. 17 - Calculate the equilibrium constant for the...Ch. 17 - Prob. 93GQCh. 17 - The solubility product constant for calcium...Ch. 17 - In principle, the ions Ba2+ and Ca2+ can be...Ch. 17 - A solution contains 0.10 M iodide ion, I, and 0.10...Ch. 17 - A solution contains Ca2+ and Pb2+ ions, both at a...Ch. 17 - Prob. 98GQCh. 17 - Prob. 99GQCh. 17 - Prob. 100GQCh. 17 - Each pair of ions below is found together in...Ch. 17 - Each pair of ions below is found together in...Ch. 17 - The cations Ba2+ and Sr2+ can be precipitated as...Ch. 17 - You will often work with salts of Fe3+, Pb2+, and...Ch. 17 - Aniline hydrochloride, (C6H5NH3)Cl, is a weak...Ch. 17 - The weak base ethanolamine. HOCH2CH2NH2, can be...Ch. 17 - For the titration of 50.0 mL of 0.150 M...Ch. 17 - A buffer solution with it pH of 12.00 consists of...Ch. 17 - To have a buffer with a pH of 2.50, what volume of...Ch. 17 - What mass of Na3PO4 must be added to 80.0 mL of...Ch. 17 - You have a solution that contains AgNO3, Pb(NO3)2,...Ch. 17 - Prob. 112ILCh. 17 - Suggest a method for separating a precipitate...Ch. 17 - Prob. 114SCQCh. 17 - Prob. 115SCQCh. 17 - Two acids, each approximately 0.01 M in...Ch. 17 - Composition diagrams, commonly known as alpha...Ch. 17 - The composition diagram, or alpha plot, for the...Ch. 17 - The chemical name for aspirin is acetylsalicylic...Ch. 17 - Prob. 120SCQ
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
- Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.arrow_forwardThe solubility rules outlined in Chapter 4 say that Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble hydroxides. Calculate the pH of a saturated solution of each of these marginally soluble hydroxides.arrow_forwardPhosphate buffers are important in regulating the pH of intracellular fluids. If the concentration ratio of H2PO4/HPO42 in a sample of intracellular fluid is 1.1: 1, what is the pH of this sample of intracellular fluid? H2PO4(aq)HPO42(aq)+H+(aq)Ka=6.2108arrow_forward
- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forwardThe text describes zinc hydroxide as an amphoteric hydroxide, so Zn(OH)2 is soluble in basic solution. What is the molar solubility of Zn(OH)2 in 1.00 M NaOH? What is the pH of the equilibrium solution?arrow_forwardYou will often work with salts of Fe3+, Pb2+, and Al3+ in the laboratory. (All are found in nature, and all are important economically.) If you have a solution containing these three ions, each at a concentration of 0.10 M, what is the order in which their hydroxides precipitate as aqueous NaOH is slowly added to the solution?arrow_forward
- Calculate the mass of manganese hydroxide present in 1300 mL of a saturated manganese hydroxide solution. For Mn(OH)2, Ksp = 2.0 1013.arrow_forwardThe hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.arrow_forwardThe solubility rules outlined in Chapter 4 say that BaCOH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble hydroxides. Calculate the pH of a saturated solution of each of these marginally soluble hydroxides.arrow_forward
- Each pair of ions below is found together in aqueous solution. Using the table of solubility product constants in Appendix J, devise a way to separate these ions by adding a reagent to precipitate one of the ions as an insoluble salt and leave the other in solution. (a) Cu2+ and Ag+ (b) A13+ and Fe3+arrow_forwardA 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. Given that 0.00966 mol of HNO₃ are used in the titration, how many moles of Ca(OH)₂ had to be present in the initial reaction?arrow_forwardA 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. to reach the endpoint, a total of 17.8 mL of HNO3 was required. write the balanced chemical equation for the reaction how many moles of HNO3 is used in the titration how many moles of Ca(HO)2 had to be present in the initial reaction what was the concentration of the initial Ca(OH)2 solutionarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
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: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher: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: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY