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# AssignmentFive - Suppose you were not able to discount the...

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Take-Home Assignment #5 Please turn in neatly worked solutions for the following problems. Answers are due by 4:00 PM on Wednesday, September 19 th . The intention of these problems is to provide additional experience in solving equilibrium problems by focusing on verifying assumptions and activity effects. Thermodynamic equilibrium constants (i.e. for μ = 0) for all reactions may be found in the Appendices to the textbook. 1. In class we examined a more rigorous solution for the solubility of AgCl in distilled water. In our original approach to the problem we only included the K sp expression. Based on the result of that calculation explain why the following species can be safely ignored: AgCl 2 , AgCl 3 2– , and AgCl 4 3– . After providing a written explanation, show by suitable calculations that this reasoning is correct. Note that the actual solubility of AgCl must include the contribution from AgCl (aq) . What is the actual solubility of AgCl in distilled water? 2.
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Unformatted text preview: Suppose you were not able to discount the importance of AgX 2 – when calculating the solubility of AgX in distilled water, where X is a singly charged anion. Show how you would carry out the calculation in this situation by (a) writing an equation that can be solved for the [Ag + ] and writing an equation for the solubility of AgX that is a function of [Ag + ]. In your solution, assume the following reactions: AgX (s) ↔ Ag + + X – K sp Ag + + X – ↔ AgX (aq) K 1 AgX (a) + X – ↔ AgX 2 – K 2 3. Calculate the ionic strength of the following solutions that contain the same molar concentration of chloride ion: 0.30 M NaCl, 0.15 M CaCl 2 , and 0.10 M AlCl 3 . 4. Calculate the concentration solubility product ( K sp c ) for Zn 2 [Fe(CN) 6 ] in a solution of 0.010 M Mg(NO 3 ) 2 . 5. Calculate the solubility of Zn 2 [Fe(CN) 6 ] in 0.010 M Mg(NO 3 ) 2 and compare to its solubility in distilled water (see problem 1 of take-home assignment 4)....
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