□ H₂O(1) OK*(aq) ClO3 (aq) Aluminium sulfate is used as a flocculating agent in the treatment of waste water. a) Write the dissocation equation for the dissociation of aluminum sulfate. b) Determine the concentration of aluminium ions and sulfate ions in a 0.250 mol/L solution of aluminium sulfate. You MUST show your work to receive full marks. ▼ B I <>X Q EE U s X₂ x²

□ H₂O(1) OK*(aq) ClO3 (aq) Aluminium sulfate is used as a flocculating agent in the treatment of waste water. a) Write the dissocation equation for the dissociation of aluminum sulfate. b) Determine the concentration of aluminium ions and sulfate ions in a 0.250 mol/L solution of aluminium sulfate. You MUST show your work to receive full marks. ▼ B I <>X Q EE U s X₂ x²

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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The following data apply to the unbalanced equation A(g)B(g) (a) On the basis of the data, balance the equation (simplest whole-number coefficients). (b) Has the system reached equilibrium? Explain.
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The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.
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?
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Will a precipitate form if 750.00 mL of a 4.0 x 10-3 mol/L solution of Cerium (III) nitrate, Ce(NO3)3(aq), is mixed in a beaker with 300.00 mL of a 2.0 x 10-2 mol/L solution of potassium iodate, KIO3(aq)?The Ksp for Cerium (III) iodiate, Ce(IO3)3 (s), is 1.9 x 10-10. Justify your answer. n:
a) What is the equilibrium constant for HF(aq) ⇌ H+ (aq) + F– (aq)?, b) is it Homogenous or Heterogenous?
The solubility product constant of calcium sulfate, CaSO4CaSO4, is 7.10×10−57.10×10−5. Its molar mass is 136.1 g/molg/mol. How many grams of calcium sulfate can dissolve in 49.0 LL of pure water?
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If the equilibrium constant for a reaction A + B <=> 2C is measured as Keq = 1.318. What would the value be for the same reaction if written as 2C <=> A + B. Keq' = ____. 3 sig. fig.
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq) + I2(aq) ⇌ KI3(aq) give the same expression for the reaction quotient. KI3 iscomposed of the ions K+ and I3 −.
The solubility of Ag(I) in aqueous solutions containing dif-ferent concentrations of Cl is based on the following equilibria:Ag⁺(aq)+Cl⁻(aq)⇌AgCl(s) Kₛₚ=1.8X10⁻¹⁰ Ag⁺(aq)+2Cl⁻(aq)⇌AgCl₂⁻(s) K(f)=1.8X10⁻⁵ When solid AgCl is shaken with a solution containing Cl⁻, Ag(I)is present as both Ag⁺ and AgCl₂⁻. The solubility of AgCl is thesum of the concentrations of Ag and AgCl₂.(a) Show that [Ag⁺] in solution is given by[Ag⁺]=1.8X10⁻¹⁰/[Cl⁻]and that [AgCl₂⁻] in solution is given by [AgCl₂⁻](3.2X10⁻⁵)([Cl⁻] (b) Find the [Cl⁻] at which [Ag⁺][AgCl₂⁻].(c) Explain the shape of a plot of AgCl solubility vs. [Cl⁻].(d) Find the solubility of AgCl at the [Cl⁻] of part (b), which is the minimum solubility of AgCl in the presence of Cl