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a. Calculate the pH of a 7.71×10-3 M solution of H2SO4

(Ka = 0.0120 for HSO4-)

b. Calculate [OH-] of a 5.45×10-1 M aqueous solution of pyridine (C5H5N, Kb = 1.7×10-9).

c. Calculate the pH of the above solution.

Oct 23rd, 2017

Question a)

Please you have to solve this equation:

0.012 = y^2 / (0.00771 - y)

where y is the concentration of [H+], please keep in mind that since H2SO4 is a strong acid, then your chemical reaction is:

H2SO4 = H+   +   SO4-.

After a simple computation, I get:

y=[H+] = 0.0053= 5.3*10^(-3)

so we have_

pH = -Log(5.3*10^(-3))= 2.28

Feb 13th, 2015

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