A 25.00mL sample of 0.300 M HClO(aq), hypochlorous acid, is titrated with 30.00mL of 0.250M LiOH. For hypochlorous acid, Ka= 2.9 x10-8 a. Label each as a strong or weak acid;strong or weak base; acidic, basic or neutral salt:LiOH HClOLiClO
b. Write the net ionic neutralization reaction for this titration mixture.
c. Calculate the initial moles of HClO and LiOH and set up a change table for the reactionwritten in part b.(Show these calculations below or attach work!)
d. Based on the substances present after neutralization, can the Henderson-Hasselbach equation be used? Explain!
e. Write the hydrolysisreaction for the hypochloriteion, ClO-.
f. Show the calculations for the following:[ClO-] = Kb= [OH-] =
g. What is the pH of this titration mixture?