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Answer 1 · 2015-12-10T07:25:41

#[H^+]=7.58xx10^(-6)M#

We console this question using Henderson-Hasselbalch equation:

#pH=pK_a+log(([C_2H_3O_2^-])/([HC_2H_3O_2]))#

#pK_a=-logK_a=-log(1.8xx10^(-5))=4.74#

#=>pH=4.74+log((0.48)/(0.2))=5.12#

Now we can calculate the concentration of #H^+# by:

#[H^+]=10^(-pH)=10^(-5.12)=7.58xx10^(-6)M#

Here is a video that explains Henderson-Hasselbalch equation:
Acid - Base Equilibria | Buffer Solution.