Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 17.5, Problem 17.11WE
(a)
Interpretation Introduction
Interpretation:
From the given compounds, the compounds that are more soluble in acidic solution compared to water has to be identified.
Concept introduction:
- Dissociation of salt forms strong conjugate base is more soluble in acidic compared to water.
- An anion reacts with acid only if it is conjugate base of a weak acid.
To identify: The
(b)
Interpretation Introduction
Interpretation:
From the given compounds, the compounds that are more soluble in acidic solution compared to water has to be identified.
Concept introduction:
- Dissociation of salt forms strong conjugate base is more soluble in acidic compared to water.
- An anion reacts with acid only if it is conjugate base of a weak acid.
To identify: The solubility of
(c)
Interpretation Introduction
Interpretation:
From the given compounds, the compounds that are more soluble in acidic solution compared to water has to be identified.
Concept introduction:
- Dissociation of salt forms strong conjugate base is more soluble in acidic compared to water.
- An anion reacts with acid only if it is conjugate base of a weak acid.
To identify: The
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
A buffer solution was prepared that contained 0.60 M hydrogen fluoride, HF (Ka = 7.2 x
104) and 1.00M potassium fluoride, KF. The total volume was 250 mL.
(a) What ions and molecules are present in the solution? List them in order of decreasing
concentration:
Decreasing order of Concentration
(b) What is the pH of the buffer solution described above?
(c) What is the pH of 100. mL of the buffer solution if you add 100. x 10-3 g of NaOH? Assume
negligible change in volume. (USEFUL INFORMATION: MM NaOH = 39.997 g mol-1)
4. A solution prepared to be initially 1 M in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5):
(A) a solution with a pH less than 7 that is not a buffer solution
(B) a buffer solution with a pH between 4 and 7
(C) a buffer solution with a pH between 7 and 10
(D) a solution with a pH greater than 7 that is not a buffer solution
(E) a solution with a pH of 7
(4) A solution is made of a mixture of 0.500 M Calcium chloride and 0.0100 M iron (II) nitrate.
The two metals are to be separated by precipitation by increasing the pH.
(a) At what pH will the first metal begin to precipitate?
(b) At what pH will 99.9% of the first metal be precipitated?
(c) At what pH will the second metal begin to precipitate?
(d) Can the metals be separated successfully?
Chapter 17 Solutions
Chemistry: Atoms First
Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Determine the pH at 25C of a solution prepared by...Ch. 17.1 - Prob. 17.1.1SRCh. 17.1 - Prob. 17.1.2SRCh. 17.2 - Starting with 1.00 L of a buffer that is 1.00 M in...Ch. 17.2 - Prob. 2PPACh. 17.2 - Prob. 2PPBCh. 17.2 - Prob. 17.3WECh. 17.2 - Prob. 3PPA
Ch. 17.2 - Prob. 3PPBCh. 17.2 - Prob. 17.2.1SRCh. 17.2 - Consider 1 L of a buffer that is 0.85 M in formic...Ch. 17.2 - Prob. 17.2.3SRCh. 17.2 - Prob. 17.2.4SRCh. 17.3 - Calculate the pH in the titration of 50.0 mL of...Ch. 17.3 - For the titration of 10.0 mL of 0.15 M acetic acid...Ch. 17.3 - Prob. 4PPBCh. 17.3 - Prob. 4PPCCh. 17.3 - Prob. 17.5WECh. 17.3 - Prob. 5PPACh. 17.3 - Prob. 5PPBCh. 17.3 - Which of the graphs [(i)(iv)] best represents the...Ch. 17.3 - Prob. 17.6WECh. 17.3 - Prob. 6PPACh. 17.3 - Prob. 6PPBCh. 17.3 - Calculate the pH at the equivalence point in the...Ch. 17.3 - Prob. 17.3.2SRCh. 17.3 - Prob. 17.3.3SRCh. 17.4 - Calculate the solubility of copper(II) hydroxide...Ch. 17.4 - Calculate the molar solubility and the solubility...Ch. 17.4 - Calculate the molar solubility and the solubility...Ch. 17.4 - Prob. 17.8WECh. 17.4 - Prob. 8PPACh. 17.4 - Prob. 8PPBCh. 17.4 - Prob. 8PPCCh. 17.4 - Prob. 17.9WECh. 17.4 - Predict whether a precipitate will form from each...Ch. 17.4 - Prob. 9PPBCh. 17.4 - Prob. 17.4.1SRCh. 17.4 - Prob. 17.4.2SRCh. 17.4 - Prob. 17.4.3SRCh. 17.5 - Prob. 17.10WECh. 17.5 - Calculate the molar solubility of AgI in (a) pure...Ch. 17.5 - Arrange the following salts in order of increasing...Ch. 17.5 - Prob. 17.11WECh. 17.5 - Determine if the following compounds are more...Ch. 17.5 - Prob. 11PPBCh. 17.5 - Prob. 11PPCCh. 17.5 - Prob. 17.12WECh. 17.5 - Prob. 12PPACh. 17.5 - Prob. 12PPBCh. 17.5 - Beginning with a saturated solution of AgCl, which...Ch. 17.5 - Prob. 17.5.1SRCh. 17.6 - Prob. 17.13WECh. 17.6 - Prob. 13PPACh. 17.6 - Prob. 13PPBCh. 17.6 - Prob. 17.6.1SRCh. 17.6 - Prob. 17.6.2SRCh. 17 - Which of the acids in Table 16.5 (page 732) can be...Ch. 17 - Prob. 17.3KSPCh. 17 - How much sodium fluoride must be dissolved in 250...Ch. 17 - Use Le Chteliers principle to explain how the...Ch. 17 - Describe the effect on pH (increase, decrease, or...Ch. 17 - Prob. 17.3QPCh. 17 - Prob. 17.4QPCh. 17 - Determine the pH of (a) a 0.40 M CH3COOH solution,...Ch. 17 - Determine the pH of (a) a 0.20 M NH3 solution, and...Ch. 17 - Which pair of substances can be dissolved together...Ch. 17 - Prob. 17.2VCCh. 17 - Prob. 17.3VCCh. 17 - Prob. 17.4VCCh. 17 - Prob. 17.7QPCh. 17 - Prob. 17.8QPCh. 17 - Calculate the pH of the buffer system made up of...Ch. 17 - Calculate the pH of the following two buffer...Ch. 17 - Prob. 17.11QPCh. 17 - Prob. 17.12QPCh. 17 - Prob. 17.13QPCh. 17 - The pH of blood plasma is 7.40. Assuming the...Ch. 17 - Calculate the pH of the 0.20 M NH3/0.20 M NH4Cl...Ch. 17 - Calculate the pH of 1.00 L of the buffer 1.00 M...Ch. 17 - Prob. 17.17QPCh. 17 - Prob. 17.18QPCh. 17 - Prob. 17.19QPCh. 17 - Prob. 17.20QPCh. 17 - The diagrams [(a)(d)] contain one or more of the...Ch. 17 - Prob. 17.22QPCh. 17 - Prob. 17.23QPCh. 17 - Prob. 17.24QPCh. 17 - Prob. 17.25QPCh. 17 - The amount of indicator used in an acid-base...Ch. 17 - Prob. 17.27QPCh. 17 - Prob. 17.28QPCh. 17 - Prob. 17.29QPCh. 17 - Prob. 17.30QPCh. 17 - Prob. 17.31QPCh. 17 - Prob. 17.32QPCh. 17 - Prob. 17.33QPCh. 17 - Prob. 17.34QPCh. 17 - A 25.0-,L solution of 0n100 M CH3COOH is titrated...Ch. 17 - A 10.0-mL solution of 0.300 M NH3 is titratee with...Ch. 17 - Prob. 17.37QPCh. 17 - Prob. 17.38QPCh. 17 - Prob. 17.39QPCh. 17 - Prob. 17.40QPCh. 17 - Diagrams (a) through (d) represent solutions at...Ch. 17 - Prob. 17.42QPCh. 17 - Prob. 17.43QPCh. 17 - Prob. 17.44QPCh. 17 - Write balanced equations and solubility product...Ch. 17 - Prob. 17.46QPCh. 17 - Prob. 17.47QPCh. 17 - Prob. 17.48QPCh. 17 - Prob. 17.49QPCh. 17 - Prob. 17.50QPCh. 17 - Prob. 17.51QPCh. 17 - The solubility of an ionic compound MX (molar mass...Ch. 17 - Prob. 17.53QPCh. 17 - Prob. 17.54QPCh. 17 - Prob. 17.55QPCh. 17 - Prob. 17.56QPCh. 17 - Prob. 17.57QPCh. 17 - A volume of 75 mL of 0.060 M NaF is mixed with 25...Ch. 17 - Prob. 17.59QPCh. 17 - Prob. 17.60QPCh. 17 - Prob. 17.5VCCh. 17 - Prob. 17.6VCCh. 17 - Prob. 17.7VCCh. 17 - How would the concentration of silver ion in the...Ch. 17 - Prob. 17.61QPCh. 17 - Prob. 17.62QPCh. 17 - Prob. 17.63QPCh. 17 - Prob. 17.64QPCh. 17 - The solubility product of PbBr2 is 8.9 106....Ch. 17 - Prob. 17.66QPCh. 17 - Calculate the molar solubility of BaSO4 in (a)...Ch. 17 - Prob. 17.68QPCh. 17 - Prob. 17.69QPCh. 17 - Prob. 17.70QPCh. 17 - Prob. 17.71QPCh. 17 - Prob. 17.72QPCh. 17 - Calculate the concentrations of Cd2+, Cd(CN)42 ,...Ch. 17 - Prob. 17.74QPCh. 17 - Prob. 17.75QPCh. 17 - (a) Calculate the molar solubility of...Ch. 17 - Prob. 17.77QPCh. 17 - Prob. 17.78QPCh. 17 - Prob. 17.79QPCh. 17 - Prob. 17.80QPCh. 17 - Prob. 17.81QPCh. 17 - Prob. 17.82QPCh. 17 - Prob. 17.83QPCh. 17 - Prob. 17.84QPCh. 17 - In a group 1 analysis, a student adds HCl acid to...Ch. 17 - Prob. 17.86QPCh. 17 - Prob. 17.87QPCh. 17 - Sketch the titration curve of a weak acid with a...Ch. 17 - Prob. 17.89QPCh. 17 - Prob. 17.90QPCh. 17 - Prob. 17.91QPCh. 17 - Tris [tris(hydroxymethyl)aminomethane] is a common...Ch. 17 - Prob. 17.93QPCh. 17 - Prob. 17.94QPCh. 17 - Prob. 17.95QPCh. 17 - Prob. 17.96QPCh. 17 - Prob. 17.97QPCh. 17 - Find the approximate pH range suitable for...Ch. 17 - Prob. 17.99QPCh. 17 - Prob. 17.100QPCh. 17 - Prob. 17.101QPCh. 17 - Prob. 17.102QPCh. 17 - Barium is a toxic substance that can seriously...Ch. 17 - The pKa of phenolphthalein is 9.10. Over what pH...Ch. 17 - Prob. 17.105QPCh. 17 - Prob. 17.106QPCh. 17 - Prob. 17.107QPCh. 17 - The molar mass of a certain metal carbonate, MCO3,...Ch. 17 - Prob. 17.109QPCh. 17 - Prob. 17.110QPCh. 17 - Describe how you would prepare a 1 -L 0.20 M...Ch. 17 - Phenolphthalein is the common indicator for the...Ch. 17 - Prob. 17.113QPCh. 17 - Prob. 17.114QPCh. 17 - Prob. 17.115QPCh. 17 - Prob. 17.116QPCh. 17 - Prob. 17.117QPCh. 17 - Prob. 17.118QPCh. 17 - When lemon juice is added to tea, the color...Ch. 17 - How many milliliters of 1.0 M NaOH must be added...Ch. 17 - Prob. 17.121QPCh. 17 - Prob. 17.122QPCh. 17 - Prob. 17.123QPCh. 17 - Prob. 17.124QPCh. 17 - Calcium oxalate is a major component of kidney...Ch. 17 - Water containing Ca2+ and Mg2+ ions is called hard...Ch. 17 - Prob. 17.127QPCh. 17 - Prob. 17.128QPCh. 17 - Prob. 17.129QPCh. 17 - (a) Referring to Figure 17.4, describe how you...Ch. 17 - Prob. 17.131QPCh. 17 - Prob. 17.132QPCh. 17 - Prob. 17.133QPCh. 17 - Prob. 17.134QPCh. 17 - Prob. 17.135QPCh. 17 - Prob. 17.136QPCh. 17 - A sample of 0.96 L of HCl gas at 372 mmHg and 22C...Ch. 17 - Prob. 17.138QPCh. 17 - The solutions (a) through (f) represent various...Ch. 17 - Prob. 17.140QPCh. 17 - Prob. 17.141QP
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 solution is 1.5 104 M Zn2 and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of zinc sulfide when the solution is saturated with hydrogen sulfide (0.10 M H2S)?arrow_forwardWhat must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO4, from a solution that is 0.0034 M Sr2+?arrow_forwardA chemistry graduate student is given 125. mL of a 1.60 M dimethylamine ((CH,) NH) solution. Dimethylamine is a weak base with K; = 5.4 × 10¯*. What mass of (CH,) NH,Cl should the student dissolve in the (CH, NH solution to turn it into a buffer with pH = 10.46? You may assume that the volume of the solution doesn't change when the (CH, NH,Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.arrow_forward
- 7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)Truearrow_forwardA buffer solution contains 0.50 M acetic acid (CH3COOH; Ka = 1.8 x 10–5) and 0.35 M sodium acetate, NaCH3CO2. What is the pH of the solution? (A) 4.59 (B) 4.90 (C) 2.29 (D) 2.52arrow_forwardpH and Solubility Is the solubility of the following compounds increased in an acidic solution? (a) Ca(OH)2 (b) Mg3(PO4)2 (c) PbBr2arrow_forward
- 6. (a) Consider the pH of a solution containing a weak acid, HA , and a soluble salt of the weak acid, such as NaAarrow_forward2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCl; (ii) 5.0 mmol of NAOH . Ka = 4.5 x 10*arrow_forward11 (a) Define a buffer solution (b) What are the components of (i) an acidic buffer ? (ii) a basic buffer ?arrow_forward
- 31. (a) Calculate the pH of a mixture containing 0.1 M propanoic acid (CH3CH₂COOH) and 0.050 M sodium propanoate (CH3CH₂COONa) (b) Determine the change in pH that occurs when 0.15 mol solid NaOH is added to 1.00 litre of the buffered solution. 32. (a) Calculate the pH of a buffer solution produced by adding 3.28 g of sodium ethanoate to 1 dm3 of 0.01 M of ethanoic acid (Ka = 1.84x 10-5 at 300K) (b) calculate the pH of this buffer if 10 cm3 of 0.1 M HCl are now addedarrow_forwardPredict the solubility change (increase, decrease, or no change) of the following compounds. Explain your choice in details. (a) Cu(OH)2 when adding HCl solution (b) AgI when adding HCl solution (c) PbCl2 when adding KCl solutionarrow_forward(a) True or false: “solubility” and “solubility-product constant”are the same number for a given compound. (b) Writethe expression for the solubility-product constant for eachof the following ionic compounds: MnCO3, Hg(OH)2, andCu3(PO4)2.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY