1. In combination with molybdenum, the cobalt(II) sulfide is used as a catalyst in the industrial process called hydrodesulfurization, which is used on a large scale in refineries. The solubility of cobalt(II) sulfide (CoS) in water is 0.38 g/L at 18°C, and its molecular weight is 91.0 g/mol. Calculate the solubility product constant for cobalt(II) sulfide at 18°C.

1. In combination with molybdenum, the cobalt(II) sulfide is used as a catalyst in the industrial process called hydrodesulfurization, which is used on a large scale in refineries. The solubility of cobalt(II) sulfide (CoS) in water is 0.38 g/L at 18°C, and its molecular weight is 91.0 g/mol. Calculate the solubility product constant for cobalt(II) sulfide at 18°C.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.26PAE: The following data were collected for the reaction, H2(g) + L(g) ** - HI(g), at equilibrium at 25°C:...

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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)
Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr2O72 , and the yellow chromate ion, CrO42 . (See the following photos.) The equilibrium reaction between the two ions is Cr2O72(aq)+H2O(l)2CrO42(aq)+2H+(aq) Explain why orange dichromate solutions turn yellow when sodium hydroxide is added.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Calculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.
Given HFH+(aq)+F(aq)Ka=6.9104HF(aq)+F(aq)H2(aq)K=2.7 calculate K for the reaction 2HF(aq)H+(aq)+HF2(aq)
Phosphate 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=6.2108
Sodium tripolyphosphate (Na5P3O10) is used in many synthetic detergents. Its major effect is to soften the water by complexing Mg2+ and Ca2+ ions. It also increases the efficiency of surfactants, or wetting agents that lower a liquids surface tension. The K value for the formation of MgP3O103 is 4.0 108 The reaction isMg2+(aq)+P3O105(aq)MgP3O103(aq). Calculate the concentration of Mg2+ in a solution that was originally 50. ppm Mg2+ (50. mg/L of solution) after 40. g Na5P3O10 is added to 1.0 L of the solution.
The following data were collected for the reaction, H2(g) + L(g) ** - HI(g), at equilibrium at 25°C: [HJ = 0.10 mol L-1, [IJ = 0.20 mol L"\ [HI] = 4.0 mol L’1 Calculate the equilibrium constant for the reaction at this temperature.
A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.
The preparation of cis-platin [Pt(NH 3) 2CI 2], an anticancer drug, uses an equilibrium reaction: K 2PECI 4(aq) + 2NH 3(aq) = 2 KCI(aq) + Pt(NH 3) 2CI 2(aq). Which of the following conditions would lead to an increase in the amount of Pt(NH 3) 2CI 2 formed? The use of a low concentration of NH3 The addition of a large concentration of KCI The use of a large concentration of NH3 The use of a stoichiometric ration of K2PTCI4 and NH3
Cyanide ion is toxic because it forms stable complexes with Fe3* in iron-containing proteins important in energy production. To study this effect, a biochemist prepares one liter of a solution that contains 0.025 mol Fe3+ and 0.80 mol CN. What is the final molar concentration of Fe3+ in the solution? K, of Fe(CN)g3- is 4.0 x 1043.
A saturated solution of Mg3(PO4)2 has a concentration of 0.939 mg per liter. Calculate the solubility product constant for Mg3(PO4)2.

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