Science
ChemistryChemistry for Engineering Students12.110 In Exercise 12.109, what do you predict would happen to an aqueous copper(ll) iodate equilibrium if sulfide ion, S 2 - , were added? The K s p of CuS is 8.7 × 10 − 36 . 12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar solubility in water and its K s p .

12.110 In Exercise 12.109, what do you predict would happen to an aqueous copper(ll) iodate equilibrium if sulfide ion, S 2 - , were added? The K s p of CuS is 8.7 × 10 − 36 . 12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar solubility in water and its K s p .

BuyFind

Chemistry for Engineering Students

4th Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781337398909
BuyFind

Chemistry for Engineering Students

4th Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781337398909

Solutions

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Textbook Problem

12.110 In Exercise 12.109, what do you predict would happen to an aqueous copper(ll) iodate equilibrium if sulfide ion, S2-, were added? The Kspof CuS is 8.7 × 10 − 36 .

12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar solubility in water and its Ksp.

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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 - write the equilibrium constant expression for any...Ch. 12 - calculate equilibrium constants from experimental...Ch. 12 - Calculate equilibrium composition from initial...Ch. 12 - calculate molar solubility from Kspor vice versa.Ch. 12 - write equilibrium constants for the dissociation...Ch. 12 - Use LeChatelier’s principle to explain the...Ch. 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 - 12.3 WTiat fraction of the annual release of...Ch. 12 - 12.4 In what geographical region of the country...Ch. 12 - 12.5 In Chapter 11, we discussed several factors...Ch. 12 - With what chemical in concrete does CO2 actually...Ch. 12 - A student finds a piece of old concrete that has...Ch. 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 - In the following equilibrium in lake water, which...Ch. 12 - Write equilibrium (mass action) expressions for...Ch. 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 - For the equilibria given below, determine each of...Ch. 12 - (a) In Exercise 12.21, if A, = 2.1 X IO10 and K2=...Ch. 12 - 12.23 An engineer is considering the use of...Ch. 12 - 12.24 Using the equations HAsO4’“(aq) *^AsO4J_(aq)...Ch. 12 - 12.25 In Exercise 12.24, which reaction has the...Ch. 12 - The following data were collected for the...Ch. 12 - The following data were collected for a system at...Ch. 12 - The equilibrium constant for the reaction, 3 H;(g)...Ch. 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 - 12.32 The equilibrium constant of the reaction of...Ch. 12 - 12.33 The following reaction establishes...Ch. 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 - In each of the reactions below, tell how the...Ch. 12 - 12.44 How would a temperature increase affect each...Ch. 12 - The following equilibrium is established in a...Ch. 12 - Write the K_, expression for each of the following...Ch. 12 - 12.47 Write an equilibrium equation and a A.,(,...Ch. 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 - 12.51 Calculate the solubility’ of ZnCO, in (a)...Ch. 12 - Because barium sulfate is opaque to X-rays, it is...Ch. 12 - The ore cinnabar (HgS) is an important source of...Ch. 12 - Calculate the As(l of the following compounds,...Ch. 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 - A student is studying a solution of the sparingly...Ch. 12 - 12.61 Write the formula of the conjugate base of...Ch. 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 - 12.65 Write chemical equations and equilibrium...Ch. 12 - 12.66 Write chemical equations and equilibrium...Ch. 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 - 12.72 The ionization constant of a very weak acid,...Ch. 12 - Morphine, an opiate derived from the opium poppy...Ch. 12 - Consider the titration of 50.0 mL of 0.250 M HNO}...Ch. 12 - Cyanic acid (HOCN) is a weak acid with AL, = 3.5 X...Ch. 12 - In a particular experiment, the equilibrium...Ch. 12 - For the reaction, PCl5(g) «=* PCl?(g) + Cl2(g),...Ch. 12 - 12.78 Use values from Appendix E at the back of...Ch. 12 - A group of students working on chemistry homework...Ch. 12 - 12.80 W hat is meant by the term crack...Ch. 12 - 12.81 Ductile materials, like metal wires, are...Ch. 12 - If bendable concrete were widely available, would...Ch. 12 - The monomer of polyvinyl alcohol was described in...Ch. 12 - At a particular temperature, iodine vapor, L, is...Ch. 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 - 12.89 For each of the following, are products or...Ch. 12 - In each of the reactions, how does the equilibrium...Ch. 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 - Consider two flasks. Both contain equal volumes of...Ch. 12 - Two weak acids, A and B, are each titrated with...Ch. 12 - Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300...Ch. 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 - 12.107 To prepare community wastewater to be...Ch. 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 - 12.112 You find a bottle in the laboratory. You...Ch. 12 - 12.113 You find a bottle of acid in the laboratory...Ch. 12 - 12.114 You need to find the equilibrium constant...Ch. 12 - 12.115 A mixture of 1.00 mole of PCl3 ; and 2.00...Ch. 12 - 12.116 Sulfur dioxide can be generated by the...Ch. 12 - 12.117 The vapor pressure of water at 80.0 °C is...Ch. 12 - 12.118 Although ammonia is made in enormous...

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