PS3 - 2 Br 2 (expressed as moles of Hg 2+ 2 per liter) in...

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CHEMISTRY 15 Fall 2009 "#$%&’( )’* +, -$./0 )*#’.1*2 3.4 50*/6/*7 8$’99/0/’.*: (due on Thursday, Oct. 1. If needed, the Ksp values can be found in Appendix F of your text) 1. Calculate the ionic strength of (a) 0.0002 M Al(NO 3 ) 3 (b) 0.02 M CuSO 4 (c) 0.01 M CuCl 2 + 0.05 M (NH 4 ) 2 SO 4 + 0.02 M Al(NO 3 ) 3 2. The ionic strength of a pure AlCl 3 solution is 0.0012. Calculate the molar concentration of AlCl 3 in this solution. [Ans: 2 ! 10 -4 M] 3. Find the activity coefficient of each ion at the indicated ionic strength. If necessary, you will find the values of the hydrated ion diameters in Chapter 10 of the text. (a) SO 2- 4 ( ! = 0.01 M) (b) Sc 3+ ( ! = 0.005 M) (c) Eu 3+ ( ! = 0.1 M) (d) (CH 3 CH 2 ) 3 NH + ( ! = 0.05 M) 4. Calculate the solubility of Hg
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Unformatted text preview: 2 Br 2 (expressed as moles of Hg 2+ 2 per liter) in (a) 3.3 ! 10-4 M Mg(NO 3 ) 2 (b) 3.3 ! 10-3 M Mg(NO 3 ) 2 (c) 3.3 ! 10-2 M Mg(NO 3 ) 2 5. An excess of the sparingly-soluble salt barium sulphate (BaSO 4 ) is added to 250 mL of distilled water in a beaker, then stirred until the mixture comes to equilibrium. (a) Calculate the concentration of Ba 2+ ( "# ) in the beaker at equilibrium. [Ans: 1 ! 10-5 M] (b) You then add 1.7 g solid sodium chloride to the beaker, stirring until all the NaCl is dissolved and the system comes to equilibrium again. Calculate the new concentration of Ba 2+ in the beaker at equilibrium. [Ans: 3 10E-5 M]...
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This note was uploaded on 02/04/2010 for the course CHEM 15 taught by Professor Staff during the Fall '08 term at University of California, Berkeley.

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