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Consider the titration of50.0 mL of 0.217 M hydrazoic acid (HN3, Ka=2.6 x 10^-5) with 0.183M
NaOH. The pH of the soluion before any NaOH is added is____
The answer is 2.62
I cant figure out what to do after you get the moles
Solution
Concentration of acid = 0.217M
[H+] = sqrt (Ka* C)
[H+] = 2.37 * 10 ^ -3
so pH = -log([H+]) = 2.624

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Consider the titration of50.0 mL of 0.217 M hydrazoic acid (HN3, Ka=.pdf

  • 1. Consider the titration of50.0 mL of 0.217 M hydrazoic acid (HN3, Ka=2.6 x 10^-5) with 0.183M NaOH. The pH of the soluion before any NaOH is added is____ The answer is 2.62 I cant figure out what to do after you get the moles Solution Concentration of acid = 0.217M [H+] = sqrt (Ka* C) [H+] = 2.37 * 10 ^ -3 so pH = -log([H+]) = 2.624