Homework Help: College Chemistry

Posted by MiShell on Tuesday, April 13, 2010 at 6:39pm.

Consider the titration of 29.00 mL of aqueous ammonia with 18.70 mL of 0.1250 M HCl (aq). Kb for NH3 (aq) is 1.8 x 10^-5.

A.) What is the formula of the solute at the equivalence point?

B.) What is the balanced equation for the ionization of the cation of the solute?

C.) What is the molarity of the solute at the equivalence point?

D.) What is the pH at the equivalence point?

College Chemistry - DrBob222, Tuesday, April 13, 2010 at 8:34pm
You must recognize what is going on in the titration. The equation is
NH3.H2O + HCl ==> NH4Cl + H2O

Obviously NH4Cl is what you have at the equivalence point.
Hydrolyze NH4Cl to determine the pH of th solute.
NH4^+ + H2O ==> H3O^+ + NH3
Set up the ICE chart, and plug all into Ka for the hydrolysis. Ka = (Kw/Kb) =
(NH3)(H3O^+)/(NH4^+)

molarity of solute is moles/L.
Post your work if you get stuck.
College Chemistry - MiShell, Tuesday, April 13, 2010 at 9:09pm
I understand the ICE chart, but I'm unsure where you get the values to put in the chart?

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