Question

How would I get the Ice of the titration of 40.00ml of 0.100M H2NNH2(aq) having a Kb of 3.0x10^-6 by 0.100M HClO4(aq)?

Trying to plot a pH curve. I know the combination of acid base is strong acid weak base

Answer 1

millimoles H2NNH2 = mL x M = 40.00 x 0.100M = 4.000 mmoles.
mmoles HClO4 = mL x 0.1M = ??. You don't list any of the volumes.
Here is how the ICE chart would look.

....H2NNH2 + HClO4 ==> H2NNH3^+ + ClO4^-
begin..4.000...0........0...........0
add...........?mmols.................
change.-?mmoles.-?mmoles.+mmoles.
equil..4-?.......0......+mmoles

Then use the Kb expression for zero mL HClO4. Use the Henderson-Hasselbalch equation for all HClO4 volumes after the beginning and before the equivalence point. Use the hydrolysis of the salt at the equivalence point and use excess HClO4 for all volumes after the equivalence point. The curve should look like one of these (or the reverse of one of these).
http://www.chemguide.co.uk/physical/acidbaseeqia/phcurves.html