A 20.00-mL sample of a 0.100 M solution of butanoic acid, CH3CH2CH2COOH (Ka = 1.54 x 10-5), is titrated with 0.100 M KOH

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A 20.00-mL sample of a 0.100 M solution of butanoic
acid, CH3CH2CH2COOH (Ka = 1.54 x 10-5), is titrated with 0.100 M
KOH solution. Answer the following questions (1 thru
8):
Calculate the volume of KOH (in mL) required to reach
the equivalence point?
Calculate the pH before adding any KOH
Calculate the pH after addition of 10.00 mL of
KOH
Calculate the pH at the equivalence
Calculate the pH at the half equivalence point.
Show that the titration is at the half equivalence
point
Calculate the pH after addition of 25.00 mL of
KOH
Use the calculated pH values, obtained from questions 1
thru 7, to carefully draw the resulting titration curve. Clearly
label the axes.
Choose an appropriate indicator for this
titration.
Please do what you can for this problem. Please Show ICE tables
and net ionic equations.