Posted by chem on Saturday, February 28, 2009 at 11:56pm.
Ammonia,is a weak base with a Kb value of 1.8x10^-5 .What is the pH of a 0.22M ammonia solution?
sorry the 2nd question is the right one
NH3 + HOH ==> NH4^+ + OH^-
Kb = (NH^+)(OH^-)/(NH3)
Do an ICE chart and plug into the expression for Kb. I get pOH = about 2.7 and pH = about 11.3 but you need to go through and not estimate as I did.
ok thanks alot...
the PartB asks for:
What is the percent ionization of ammonia at this concentration?
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