Explain the ph of the solution when half of the base

Reference no: EM13517994

Comsider the titration of a 25 mL of a 0.100 M solution of a weak acid HA, pKa = 7.5, with a 0.200M solution of a strong base.

a) how many mL of base must be added to reach the equivalnce point?

b) what is the pH of the solution when half of the base in part a has been added?

c) what is the pH of the solution at the equivalnce point?

d) if phenol solution = 0.167 M calculate the pH of it when Ka = 1.0 x 10^-10.

e) what is the concentration of hydroxide ions, [OH^-], when 100.0 mL of 0.400 M NaOH have been added to 100.0 mL of a 0.100 M H2SO4?

Reference no: EM13517994

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