4. An experiment similar to the one described in this module was performed to determine the solubility and solubility product constant of lead(ll) chloride (gmm = 278.10). The equilibrium involved is PbCl2(s) Pb2+ (aq)+2 CI¯(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO, solution. The solid AgCl was filtered from solution, dried, and weighed. The following data were obtained for three samples of the filtered, saturated solution. determination 1 temperature of solution, °C volume of PbCl2 solution analyzed, mL mass of dry AgCI, g 20.2 20.4 20.1 25.00 22.00 20.10 0.2543 0.2276 0.2051 Calculate the following: number of moles of: AgCl(s) Cl- (aq) Pb2*(aq) (CI"] in PbCl2 solution, M [Pb2+1 in PbCl2 solution, M Ksp average Ksp solubility of P6C12, in g per 100 mL chemistry handbook value for solubility at 20°, g per 100 mL

4. An experiment similar to the one described in this module was performed to determine the solubility and solubility product constant of lead(ll) chloride (gmm = 278.10). The equilibrium involved is PbCl2(s) Pb2+ (aq)+2 CI¯(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO, solution. The solid AgCl was filtered from solution, dried, and weighed. The following data were obtained for three samples of the filtered, saturated solution. determination 1 temperature of solution, °C volume of PbCl2 solution analyzed, mL mass of dry AgCI, g 20.2 20.4 20.1 25.00 22.00 20.10 0.2543 0.2276 0.2051 Calculate the following: number of moles of: AgCl(s) Cl- (aq) Pb2*(aq) (CI"] in PbCl2 solution, M [Pb2+1 in PbCl2 solution, M Ksp average Ksp solubility of P6C12, in g per 100 mL chemistry handbook value for solubility at 20°, g per 100 mL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4.0 mL of 0.20 M HCI is added to 4.0 mL of 0.30 M Pb(NO3)2 to produce a precipitate of PbCl21s)- Water in the amount of 9.0 mL is added to dissolve the precipitate. Based on this data, what is the Ksp of PBCI2(s}? Express answer as a decimal value.
A highly acidic (pH< 0.5) industrial wastewater has an initial AlP" concentration of 10 ppm. An engineer decides that strong base should be added to the wastewater in order to raise the pH so that most of the aluminum will precipitate and be removed from solution. The pertinent solubility reaction from Appendix A of our text is: Al(OH)3 (s) → Al* + 30H¯ with pK, = 32.9 a. What is the lowest pH needed to precipitate all but 50 ppb of the aluminum from the wastewater? Assume equilibrium conditions can be achieved. b. Suppose the engineer decides that the pH should be raised to 7. What equilibrium concentration of aluminum would be left in solution? Report your answer in ppb and moles per liter.
1. In this experiment we measured K, for borax Na,B,O,(OH), 8H,0(s)=2Na*(aq)+B,0,(OH),² (aq)+8H,0(1) write down K, for this reaction in terms of reactants/product sp concentrations We measured the concentration of the borate by titrating it with HCl to make boric acid B,O,(OH), (a) + 2 HCI( aq) + 3 H,O(I) → 4 H,BO, + 2CI (ag) the pH at the equivalence point is pH = 4. 2. What indicator did we use, and what color was the indicator at the equivalence point? 3. At 48.2°C, 5.00ml of the saturated solution of bo ax was titrated with 0.235M HCI. It took 23.00 mL of the a id to reach the equivalence point. 1. What is the molarity of the tetra-borate anion in t e solution? 2. What is Kn for borax at this temperature?
[PBCI,] complex K; = 2.5 x 1015 For the aqueous at 25 °C. Suppose equal volumes of 0.0030M Pb(NO,) solution and 0.38M KCl solution are mixed. Calculate the equilibrium molarity of aqueous Pb- 2+ ion. Round your answer to 2 significant digits. ?
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The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M, [C]=0.0230 M, and [AC5]=0.100 M. Determine the formation constant, Kf, of AC5. Kf = 155367729.8 The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.152 M. What is the Ksp of AB? Ksp = ?
a solution contains 0.0036 M Zn^+2 and 0.044 M Fe^+2. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. at what concentration of sulfide ion will a precipitate begin to form? what is the identity of the precipitate? Ksp(Zns)=2.0x10^-25, Ksp(FeS)=6.3x10^-18. a)1.4x10^-16 M, FeS b)1.4x10^-16 M, ZnS c)5.6x10^-24 M, ZnS d)5.6x10^-24 M, FeS e) No precipitate will form at any concentration of sulfide ion.