Question #2c8ae

1 Answer
Dec 10, 2015

Answer:

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

Explanation:

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.