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#1. Calculate the pH for each of the following cases in the titration of 50.0 mL...

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Chemistry

#1. Calculate the pH for each of the following cases in thetitration of 50.0 mL of 0.200 M HClO(aq) with 0.200 M KOH(aq). Theionization constant of HClO is Ka = 4.0×10–8.

(a) Before addition of any KOH

(b) After addition of 25.0 mL of KOH

(c) After addition of 30.0 mL of KOH

(d) After addition of 50.0 mL of KOH

(e) After addition of 60.0 mL of KOH

#2 Calculate the pH for each of the following cases in thetitration of 25.0 mL of 0.200 M pyridine, C5H5N(aq) with 0.200 MHBr(aq). The ionization constant for pyridine is Kb =1.7×10–9.

(a) Before addition of any HBr

(b) After addition of 12.5 mL of HBr

(c) After addition of 20.0 mL of HBr

(d) After addition of 25.0 mL of HBr

(e) After addition of 29.0 mL of HBr

Answer & Explanation Solved by verified expert
3.8 Ratings (692 Votes)
Unfortunately this is a lengthy problem because it is not possible to use one method and plug in different values except for the second and third b and c volumes Equation HClO KOH KClO H2O 1 mol HClO reacts with 1 mol KOH to produce 1 mol KClO plus water You will notice that throughout most of the problem you have a solution containing a weak acid HClO and the conjugate base of that acid from the salt KClO This is a buffer solution a Before any addition of KOH What you are asked to do is calculate the pH of the acid solution You do this by using the Ka equation Ka H acid 40108 H 0200 H 40108 0200 H 80109 H 80109 H 8944105 M pH log H pH log8944105 pH 405 b After addition of 250mL of KOH This produces a mixture of    See Answer
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