What is the pH ( 3 significant digits) of a 0.01 M solution of sulfuric acid? Hint is that the first ionization constant is "large", and the second is finite, and the [H+] donated by the second equilibrium depends upon the amount of [H+] already donated by the first ionization. What is the answer please.
k2 is 1.2 x 10^-2.. please solve whole problem.. Im soo confused!
If you do your ICE table for the second reaction, you get this (and assume the first H goes to completion)
k2=[H][SO4]/[HSO4]
.012=(.01+x)(x)/(.01-x)
Solve for x, and calculate pH where H is .01+x