and PbOH 2 Type c salt ions Cl Type d PbCl Make sure to write the equilibrium

And pboh 2 type c salt ions cl type d pbcl make sure

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+ , and Pb(OH) 0 2 Type c : salt ions: Cl - Type d : PbCl + (Make sure to write the equilibrium equation for this d- species. [See last equation in the Table below, corresponding to K 4 ]. Since we have 9 unknowns at equilibrium, we will need a total of 9 equations. 2
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Step-2 : Write the relevant equilibrium equations and constants H 2 O ↔ H + + OH - K w = {H + }{OH - } = 10 -14.0 Eq.1. CH 3 COOH CH 3 COO - + H+ ¿ C H 3 COO ¿ ¿ ¿ K 1 = ¿ Eq.2. Pb 2+ + OH - Pb(OH)+ 2 + ¿ Pb ¿ ¿ ¿ { Pb ( OH ) + ¿ } ¿ K 2 = ¿ Eq.3. Pb(OH) + + OH - Pb(OH) 2 0 + ¿ }{ OH ¿ } { Pb ( OH ) ¿ K 3 = { Pb ( OH ) 2 0 } ¿ Eq.4. Pb 2+ + Cl - PbCl + 2 + ¿ Pb ¿ ¿ ¿ { PbCl + ¿ } ¿ K 4 = ¿ Eq.5 . 3
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Step-3 : Write a mass balance (MB) on each ion type other than H + and OH - . Define an ion type as any ion or molecule in its most dissociated form (e.g. Na + , Cl - , Cu 2+ , NH 3 0 ). In contrast, neutrally charged compounds and ions that can still undergo dissociation ( CuCO 3 0 , NH 4 + , HCO 3 - , etc.) are not ion types . Additionally, OH - and H + are not included here as they appear separately as type species . Finally, the number of ions for a given system is equal to the number of weak acid/base systems (i.e. groups of type b species ) plus the number of type c species Ion Types initialconditions ( c i n iA ) = equilibriumconditions ( c i n iA ) Where A is an ion type, c i is the conc. which contains ion type A, and n A = number of A groups in each molecule of species i Eq # CH 3 COO - (3*10 -3 )(2) = {CH 3 COO - }(1) + {CH 3 COOH}(1) 6
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  • Fall '08
  • CHADIK
  • Chemistry, #, Electric charge, 0.02 m, 0.020 M, 0.013 m

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