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Find the pH during the titration of 20.00 mL of 0.1590 M nitrous acid, HNO2 (Ka...

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Chemistry

Find the pH during the titration of 20.00 mL of 0.1590 M nitrousacid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.1590 M NaOH solution after thefollowing additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL(d) 19.00 mL (e) 19.95 mL (f) 20.00 mL (g) 20.05 mL (h) 25.00mL

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4.2 Ratings (632 Votes)
a We have only nitrous acid we make our ICE table and establish dissociation equation HNO2 NO2 H3O HNO2 NO2 H3O I 0159 0 0 C x x x E 0159 x x x We use constant of acid definition Ka NO2 H3O HNO2 71 x 104 x2 0159 x Isolation for x x H 00103 M pH logH 19872 b When adding 10 mL we have 001 L 0159 molL 000159 moles of NaOH 002 L 0159 molL 000318 moles of HNO2 Half the moles will    See Answer
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