|MadSci Network: Chemistry|
The "educator?" Do you know the story "The Emperor's New Clothes?" Assuming unit chemical activities (dilute solution), pH is the negative common logarithm of the hydrogen ion concentration (the "p" means "negative common logarithm of"). There is neither mystery nor romance to it. It is merely a concentration of a species in solution. 1a) You look up the pKa of HOCl. You now know the Ka. You write the hydrolysis equation OCl- + H20 <--> HOCl + OH- You write the equilibrium expression from the equation You plug in the known concentrations and the HOCl ionization constant. You solve for the unknown [H+] (or [OH-]; they're related) You take -log[H+] to get the pH. It is no different from figuring out the pH of an acetate buffer. 1b) Same idea, You look up the disproprotionation (or conproportionation) constant of Cl2 + H2O <--> HOCl + HCl (or the equation in base; whatever). 2) You could do something daring, going beyond cracking your textbook, like looking it up in another text (library). Or confront your instructor and have it (no gender attribute - politically correct) actually teach something - as in successfully conveying useful information. (Ammonia is the least of your worries in millimolar solution. Worry about H2Se outgassing.) Ammonia cannot outgas as the neutral molecule if it is protonated as the ion. Under what conditions does that obtain? -- Uncle Al Schwartz UncleAl0@ix.netcom.com ("zero" before @) http://pw2.netcom.com/~uncleal0/uncleal.htm http://www.ultra.net.au/~wisby/uncleal.htm http://www.guyy.demon.co.uk/uncleal/uncleal.htm (Toxic URLs! Unsafe for children, Democrats, and most mammals) "Quis custodiet ipsos custodes?" The Net!
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