Question

A) Assume that you are titrating 60.0 mL of 0.0500 M ammonia (Kb = 1.8 × 10^–5) with 0.100 M hydrochloric acid.   

How much HCl (in mL) is required to reach a titration equivalence point?

B)

Assume that you are titrating 60.0 mL of 0.0500 M ammonia (Kb = 1.8 × 10^–5) with

0.100 M hydrochloric acid.

Setting up I.C.E charts for NH₃ before the titration, and when the titration reaches the equivalence point.  Based on the I.C.E. Chart and find pH of the solutions.

[Note: You will have two I.C.E. charts and 2 pH calculations]

C) Assume that you are titrating 60.0mL of 0.05 M Ammonia (Kb = 1.8x10^-5) with 0.1 M Hydrochloric Acid.

Fill in the following table and explain your answers with calculation. (I really need a thorough table and calculations here, I understand almost nothing of this, please help.)

This is all the info I have for the whole question

Volume(mL) of HCl added	Total volume(mL)	[NH3]	[NH4+]	{H3O+](Fill this in only after equivalence point is reached)	pOH	pH
0 mL
15 mL
(What is equivalence point?)
40 mL

Answer 1