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
Videos
Textbook Question
Chapter 12, Problem 12.50PAE
In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water?
The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
11.
The structural formulae of two amino acids are shown below.
||
НООС - СH-CH, - CH-С -ОН
NH2
Glutamic acid (glu)
When glutamic acid dissolve in aqueous sodium hydroxide, monosodium glutamate
(MSG) is formed, which is used as a flavor enhancer. Write an equation for the formation
of MSG. Predict whether a solution of glutamic acid is acidic, basic or neutral. Explain
your answer.
1. Copper oxides are a product of the oxidation of copper that often form on the inside of copper pipes transporting water and serves to protect the pipes against corrosion. They are toxic. At a pH above 8, these oxides are virtually insoluble in water. As the pH of the water flowing drops below 7, the solubility of these oxides increases, and the layer begins to dissolve. Based on this knowledge, and the data collected in your lab, what implications does this have on toxic metal pollutants or other pollutants in our drinking supply when the water flowing is acidic? Would this problem become better or worse if the water flowing through the pipes was hot?
2. The chemical obtained from red cabbage that acts as a pH indicator is a pigment called anthocyanin. Based on your results, do you think anthocyanin is a useful indicator? Why or why not?
A 1.00 liter solution contains 0.58 moles hypochlorous acid and 0.45 moles sodium hypochlorite .
If 0.22 moles of nitric 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 nitric acid.)
VA. The number of moles of HCIO will remain the same.
vB. The number of moles of CIO" will decrease.
vC. The equilibrium concentration of H30+ will increase.
D. The pH will remain the same.
vE. The ratio of [HCIO] / [CIO¯] will remain the same.
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
- A 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a What is the hydroxide-ion concentration of this solution? b 0.075 mol of MgCl2 is added to the above solution. Assume that there is no volume change. After Mg(OH)2 has precipitated, what is the molar concentration of magnesium ion? What percent of the Mg2+ is removed from solution?arrow_forwardIf 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?arrow_forwardWhich of the following pictures best represents an unsaturated solution of sodium chloride, NaCl? In these pictures, the dark gray spheres represent Na+ ions and the green spheres represent chloride ions. For clarity, water molecules are not shown.arrow_forward
- 1,2-Dichloroethane is a volatile organic compound that was once added to gasoline along with the heavy metal lead. At many former gasoline storage sites, the unsaturated soil and groundwater are still contaminated with 1,2-dichloroethane. One of the concerns with volatile organic compounds in the unsaturated zone of soil is that they can diffuse into buildings and contaminate the air. Calculate the concentration of 1,2- dichloroethane in air that will result in a carcinogenic risk of 104, based on a breathing rate of 11.3 m/d, exposure for 10 hours per day, and an inhalation PF of 9.1x102 kg•d/mg. Express your answer in µg/m³. А. Calculate the concentration of 1,2-dichloroethane in groundwater that will result in a hazard quotient of 1, based on drinking 2 L of water per day for a lifetime and an oral RfD of 0.012 mg/(kg d). Express your answer in ppb. В.arrow_forwardIn which of the following aqueous solutions would you expect AgF to have the lowest solubility? pure water 0.023 M NaF 0.030 M LiF 0.015 M KF 0.0075 M AgNO3arrow_forwardOnly about 0.16 mg of AgBr(s) will dissolve in 1.0 L of water (this volume of solid is smaller than the head of a pin). In a solution of ammonia that contains 0.10 mol ammonia per liter of water, there are about 555 watermolecules for every molecule of ammonia. However, more than 400 times as much AgBr (68 mg) will dissolve in this solution as in plain water. Explain how such a tiny change in the composition of the solution can have such a largeeffect on the solubility of AgBrarrow_forward
- Which salt would you expect to dissolve more readily in acidic solution? Barium sulfate or barium fluoride . Explain .arrow_forwardwhere silver chloride dissolves more and where it dissolves less: a) in 0.5 liters of clean water b) in 0.8 liters of 0.5M NaCl salt solution or c) in 0.8 liters of 0.2M AgNO3 silver nitrate solution?arrow_forward1) Describe how you would prepare a 500.00 mL portion of 0.25M calcium hydroxide solution starting with solid calcium hydroxide. (b) What is the pH of the solution? 2) Acetone has a vapor pressure of 183.0 mm Hg at 40 °C and a heat of vaporization of 30.8 kJ/mol. What is the vapor pressure of acetone at 25 °C? 3) (a) Calculate the molality (m) of a solution containing 75.0 gm of glycol (C2H&O2) in 250.0 gm of water. (b) What is the mass percent of glycol in this solution?arrow_forward
- It takes 38.85 mL of an NaOH solution to neutralize 1.036 g of potassium acid phthalate. What is the molarity of the NaOh solution? The molar mass of KHP is 204.22 g/mole.arrow_forwardA 0.800 M solution of NH3 is prepared and is in equilibrium with its ions. Is the assumption valid (using the 5% rule)? Ammonia has a Kb of 1.75x10¬5.arrow_forwardIn which of the following aqueous solutions would you expect AgF to have the highest solubility? 0.00750 M LİF 0.023 M NaF 0.015 M KF 0.030 M AgNO3 AgF will have the same solubility in all solutions.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
General 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: 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 for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
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
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
General Chemistry | Acids & Bases; Author: Ninja Nerd;https://www.youtube.com/watch?v=AOr_5tbgfQ0;License: Standard YouTube License, CC-BY