More Titration Problems for practice

	Nancy J. Mullins, Ph.D.
	© 2003

Steps to the problem

	1. Write the net ionic equation for the reaction.1
	2. Dilute the substances to represent the effect of changing volume on concentrations
	3. Allow the limiting reagent to be consumed 100%2
	4.  Examine what remains:
		Xs H3O+? pH determined from this concentration.3
		Xs OH-? pH=14+log[OH-]
		Xs Weak acid? Write the Ka reaction to find [H3O+]
		Xs Weak Base? Write the Ka reaction to find [OH-]
		Xs Buffer? Use the Henderson-Hasselbalch equation.

1.For the titration of 25mL of 3M NH₃ with 2.5M HCl:

	A. What is the net ionic equation?
	B. What is the endpoint?
	C. What is the pH at 0 mL
	D. What is the pH at 5 mL?
	E. What is the pH at 10 mL?
	F. what is the pH at the endpoint?
	G. What is the pH at 35 mL?
	H. Select an appropriate indicator

2. For the titration of 25mL of 3M NaCN with 5M HCl:

	A. What is the net ionic equation?
	B. What is the endpoint?
	C. What is the pH at 0 mL
	D. What is the pH at 5 mL?
	E. What is the pH at 10 mL?
	F. what is the pH at the endpoint?
	G. What is the pH at 35 mL?
	H. Select an appropriate indicator

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