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This is a buffer solution.
Buffer solution always contains mixture od two compounds; salt and weak acid (or base).Two wise men prepared a special formula for such calculations.
Quote from: AWK on November 19, 2016, 03:12:06 PMBuffer solution always contains mixture od two compounds; salt and weak acid (or base).Two wise men prepared a special formula for such calculations.yes...But usually is:Salt : NH4Clweak base : NH3So I have a buffer solution of NH4+/NH3 and a strong base Cl- that doesn't hydrolizeBUT I have,in this case , a buffer solution of a chemical compound "A" (NH3/NH4+) and a weak base CH3COO- that reacts with water (hydrolize) So how can I calculate pH considering also the protonation of CH3COO- in my buffer solution?Thanks!
For buffer solution a working ratio Bronsted acid/conjugated Bronsted base is from 1/10 to 10/1.Your data fails in this range.
@ AWK:QuoteFor buffer solution a working ratio Bronsted acid/conjugated Bronsted base is from 1/10 to 10/1.Your data fails in this range. assuming that with the excess of ammonia given, the acetic acid becomes more or less completely deprotonized, the resulting ratio of NH3/NH4+ should be like ~ (10-2 - 10-3) / 10-3 = 9 : 1 , which is well within named range