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Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is an important compound in industry and agriculture. Calculate...

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Chemistry

Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is animportant compound in industry and agriculture.

Calculate the pH for each of the following points in thetitration of 50.0 mL of a 1.5 M H3PO3(aq) with 1.5 M KOH(aq).

pKa1= 1.30

pKa2= 6.70

(a) before addition of any KOH =_____number

(b) after addition of 25.0 mL of KOH = ______number

(c) after addition of 50.0 mL of KOH = ______number

(d) after addition of 75.0 mL of KOH =_______number

(e) after addition of 100.0 mL of KOH=______number

please explain how you got each! thanks so much

also this might help: For part (a), you only need to considerthe first ionization because Ka1 >> Ka2. Use pKa1 to find thevalue of Ka1, then solve for x.

Answer & Explanation Solved by verified expert
3.8 Ratings (440 Votes)
a before adding base Since pka1 pka2 the pH of the acid is calculated as a weak monoprotic acid that is pH 12pKa1 12 log concentration 12 x13 12 log15 05619 b When base is added the reaction is H3PO3 KOH KH2PO3 H2O 50x15 x2 25x15 0 0    See Answer
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