Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 12, Problem 12.17PAE
12.17 Which of the following is more likely to precipitate sulfate ions?
PbSO4(s) Pb*+(aq) + SO42’(aq) K = 1.8 X IO"8 CaSO4(s) i=i Ca2+(aq) + SO42'(aq) K = 9.1 X 10-6
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The molar solubility of the
metal hydroxide (M(OH)2) in
water is:
M(OH)2
= M2+ +
2ОН
Ksp = 5.02 x
10-6
3.60 x 10-2 M
1.10 x 10-2 M
3.30 x 10-6 M
1.00x 10-5 м
4.31 x 10-6 M
At 500 K, the equilibrium constant for this reaction: X2(g) + 2Y2(g) ⇒ 3Z2(g) is Kc = 0.222. At
the same temperature, what would be the Kc for the following reaction: Z2(g) = 1/3X2(g) +
2/3Y2(g)?
1.65
91.4
1.50
4.50
Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1.
When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium:
Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq)
Use this information above to find the value of Ksp for Ca(OH)2 at 25°C.
What is the pH of this saturated Ca(OH)2 solution?
Chapter 12 Solutions
Chemistry for Engineering Students
Ch. 12 - list chemical reactions important in the...Ch. 12 - Explain that equilibrium is dynamic, and that at...Ch. 12 - Prob. 3COCh. 12 - calculate equilibrium constants from experimental...Ch. 12 - Prob. 5COCh. 12 - calculate molar solubility from Kspor vice versa.Ch. 12 - Prob. 7COCh. 12 - Prob. 8COCh. 12 - calculate the new equilibrium composition of a...Ch. 12 - Explain the importance of both kinetic and...
Ch. 12 - Identify the first chemical step in the production...Ch. 12 - Explain why the hydration process for concrete is...Ch. 12 - Prob. 12.3PAECh. 12 - 12.4 In what geographical region of the country...Ch. 12 - Prob. 12.5PAECh. 12 - Prob. 12.6PAECh. 12 - Prob. 12.7PAECh. 12 - On your desk is a glass half-filled with water and...Ch. 12 - An equilibrium involving the carbonate and...Ch. 12 - A small quantity of a soluble salt is placed in...Ch. 12 - Prob. 12.11PAECh. 12 - Prob. 12.12PAECh. 12 - Write equilibrium (mass action) expressions for...Ch. 12 - What is the difference between homogeneous...Ch. 12 - Write equilibrium expressions for each of the...Ch. 12 - Write equilibrium expressions for each of the...Ch. 12 - 12.17 Which of the following is more likely to...Ch. 12 - The reaction, 3 H2(g) + N2(g) (g), has the fol...Ch. 12 - 12.19 For each of the following equations, write...Ch. 12 - Consider the following equilibria involving SO2(g)...Ch. 12 - Prob. 12.21PAECh. 12 - Prob. 12.22PAECh. 12 - Prob. 12.23PAECh. 12 - Prob. 12.24PAECh. 12 - Prob. 12.25PAECh. 12 - The following data were collected for the...Ch. 12 - The following data were collected for a system at...Ch. 12 - Prob. 12.28PAECh. 12 - Nitrosyl chloride, NOCI, decomposes to NO and Cl,...Ch. 12 - Hydrogen gas and iodine gas react via the...Ch. 12 - 12.31 A system consisting of 0.100 mole of oxygen...Ch. 12 - Prob. 12.32PAECh. 12 - Prob. 12.33PAECh. 12 - 1’he reaction in Exercise 12.33 was repeated. This...Ch. 12 - In the reaction in Exercise 12.33, another trial...Ch. 12 - The experiment in Exercise 12.33 was redesigned so...Ch. 12 - Again the experiment in Exercise 12.33 was...Ch. 12 - At a particular temperature, the equilibrium...Ch. 12 - A student is simulating the carbonic acid—hydrogen...Ch. 12 - Because carbonic acid undergoes a second...Ch. 12 - Because calcium carbonate is a sink for CO32- in a...Ch. 12 - 12.42 The following reaction is in equilibrium in...Ch. 12 - Prob. 12.43PAECh. 12 - Prob. 12.44PAECh. 12 - The following equilibrium is established in a...Ch. 12 - Write the K_, expression for each of the following...Ch. 12 - Prob. 12.47PAECh. 12 - calculate the molar solubility of the following...Ch. 12 - 12.49 The Safe Drinking Water Act of 1974...Ch. 12 - In Exercise 12.49, what is the allowed...Ch. 12 - Prob. 12.51PAECh. 12 - Because barium sulfate is opaque to X-rays, it is...Ch. 12 - The ore cinnabar (HgS) is an important source of...Ch. 12 - Prob. 12.54PAECh. 12 - From the solubility data given for the following...Ch. 12 - The solubility of magnesium fluoride, MgF2, in...Ch. 12 - Solid Na2SO4 is added slowly to a solution that is...Ch. 12 - Will a precipitate of Mg(OH)2 form when 25.0 mL of...Ch. 12 - Use the web to look up boiler scale and explain...Ch. 12 - Prob. 12.60PAECh. 12 - Prob. 12.61PAECh. 12 - 12.62 Write the formula of the conjugate acid of...Ch. 12 - 12.63 For each of the following reactions,...Ch. 12 - What are the products of each of the following...Ch. 12 - Prob. 12.65PAECh. 12 - Prob. 12.66PAECh. 12 - 12.67 Hydrofluoric acid is a weak acid used in the...Ch. 12 - The pH of a 0.129 M solution of a weak acid, HB,...Ch. 12 - Calculate the pH of a 0.10 M solution of propanoic...Ch. 12 - Find the pH of a 0.115 M solution of NH3(aq).Ch. 12 - Acrylic acid is used in the polymer industry in...Ch. 12 - Prob. 12.72PAECh. 12 - Prob. 12.73PAECh. 12 - Prob. 12.74PAECh. 12 - Cyanic acid (HOCN) is a weak acid with AL, = 3.5 X...Ch. 12 - In a particular experiment, the equilibrium...Ch. 12 - Prob. 12.77PAECh. 12 - Prob. 12.78PAECh. 12 - Prob. 12.79PAECh. 12 - Prob. 12.80PAECh. 12 - Prob. 12.81PAECh. 12 - Prob. 12.82PAECh. 12 - Prob. 12.83PAECh. 12 - Prob. 12.84PAECh. 12 - 12.85 In the figure, orange fish are placed in one...Ch. 12 - For the system in the preceding problem, show the...Ch. 12 - Prob. 12.87PAECh. 12 - Which of the following is more likely to...Ch. 12 - Prob. 12.89PAECh. 12 - Prob. 12.90PAECh. 12 - In the following equilibrium in a closed system,...Ch. 12 - Consider the following system:...Ch. 12 - The decomposition of NH4HS , NH4HS(s)NH3(g)+H2S(g)...Ch. 12 - You are designing a process to remove carbonate...Ch. 12 - Equal amounts of two gases, A and B3, are placed...Ch. 12 - Prob. 12.96PAECh. 12 - Prob. 12.97PAECh. 12 - Prob. 12.98PAECh. 12 - Solid CaCO3 ; is placed in a closed container and...Ch. 12 - 12.100 A reaction important in smog formation is...Ch. 12 - 12.101 An engineer working on a design to extract...Ch. 12 - 12.102 A chemical engineer is working to optimize...Ch. 12 - 12.103 Methanol, CH3OH, can be produced by the...Ch. 12 - Prob. 12.104PAECh. 12 - 12.105 Using the kinetic-molecular theory, explain...Ch. 12 - 12.106 The solubility of KCl is 34.7 g per 100 g...Ch. 12 - Prob. 12.107PAECh. 12 - 12.108 A nuclear engineer is considering the...Ch. 12 - 12.109 Copper(II) iodate has a solubility of 0.136...Ch. 12 - 12.110 In Exercise 12.109, what do you predict...Ch. 12 - 12.111 You have three white solids. What...Ch. 12 - Prob. 12.112PAECh. 12 - Prob. 12.113PAECh. 12 - Prob. 12.114PAECh. 12 - Prob. 12.115PAECh. 12 - Prob. 12.116PAECh. 12 - 12.117 The vapor pressure of water at 80.0 °C is...Ch. 12 - Prob. 12.118PAE
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
- . K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.arrow_forwardYou are designing a process to remove carbonate ions from an aqueous system by precipitation. If the effectiveness of the process is the only concern (meaning there are no environmental or other issues involved), which of the following metal ions would be the best choice: Ca2+,Fe2+,Pb2+,orAg2+ ? Explain your answer. Salt Ksp CaCO3 4.8109 FeCO3 3.51011 PbCO3 1.51013 Ag2CO3 8.21012arrow_forwardA solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?arrow_forward
- Some lithium chloride, LiCl, is dissolved in 100 mL of water in one beaker, and some Li2SO4 is dissolved in 100 mL of water in another beaker. Both are at 10 C, and both are saturated solutions; some solid remains undissolved in each beaker. Describe what you would observe as the temperature is raised. The following data are available to you from a handbook of chemistry:arrow_forwardSuppos constants for the two reactions XeF(g) + H2O(g) = XeOF4(g) + 2 HF(g) XeO4(g) + XeF,(g) 2 XeOF4(g) + XeO3F2(g) Give the equilibrium constant for the reaction XeO4(g) + 2 HF(g) = XeO3F2(g) + H2O(g)arrow_forwardCalcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C.arrow_forward
- The solubility of sodium bicarbonate in water is 11.1 g N aHCO 3/100 g H 2O at 30°C and 16.4 g N aHCO 3/100 g H 2O at 60°C. If a saturated solution of Na HCO 3 at 60°C is cooled and comes to equilibrium at 30°C, what percentage of the dissolved salt crystallizes?arrow_forwardA mixture of 0.60 mol Cl2(g) and 0.40 mol F2(g) was allowed to come to equilibrium in a 1000-mL flask. If 2x represents the molar concentration of CIF(g) at equilibrium, which expression represents the equilibrium constant? C2(g) +F2(g) 2 2CIF(g) (2x)2 (0.60 – x) · (0.40 – x) x2 (A) (B) (0.60 — х) - (0.40- х) 2x 2r2 (D) (0.60 – x) · (0.40 – x) (0.60 – x) · (0.40 – x) O A В O carrow_forwardDetermine the concentrations at equilibrium of the important species when 10.0 g ethanol (MW 46.07 g/mol) are placed with 25.0 g of oxygen (MW 32.00 g/mol) in a 1.00 L container at 100.°C. C2H5OH(I) + 302(g) 2CO2(g) + 3H20(1) Kc = 168. M1 %3Darrow_forward
- The apparent solubility products of AgCN and PbF2 at 25°C are 6.0x10-1/ and 3.3×10¬8, respectively. Calculate the solubility (g/100. g of solution) of these compounds. (Assume each solution has a density of 0.99705 g·cm-3.) 4.0 solubility of A9CN g/100. g of solution solubility of PBF2 4.0 g/100. g of solutionarrow_forwardTiny samples of aqueous solutions are sketched below, as if under a microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) The two substances in each sample can interconvert. That is, each kind of molecule can turn into the other. The equilibrium constant K for each interconversion equilibrium is shown below the sketch. Decide whether each solution is at equilibrium. Coo yes 000 8 At equilibrium? yes 1 K = = = = 8 9 no K=9 At equilibrium? O no At equilibrium? O yes K= 4 yes no 3 K= 2 At equilibrium? no Xarrow_forward9 Maps YouTube Grades for Kianna... 101 Chem101 Pratt O 3.65 O 5.66 x 103 O 13.3 O -0.0376 Question 9 At 1000 K, the equilibrium constant for the reaction 2No (g) + 02 (g) =Cl, (g) + H,O is Ko = 0.013. Calculate K, for the reverse reaction, 2HCI (g) + 02 (g) =Cl, (g) + H2O (g) O 0.99 O 1.6 x 10-4 O 1.1 O 7 O 0.013 Question 10 Consider the following equilibrium. 2 SO2 (g) + O2 (g) =2 SO3 (g) The equilibrium cannot be established when is/are placed in aarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- 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 LearningIntroductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher: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
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY