CHEM 1212 – Principles of Chemistry II

CHEM 1212 – Principles of Chemistry II, Spring 2008
Ch. 16 Homework Assignment (10 points) – Due date 3/3/08
Calculate the following:
pH and pOH of a 0.05 M H2SO4 solution
[H+] and [OH-] for a 1.5 M NaOH solution
For each of the following aqueous reactions, identify the acid, the base, the
conjugate acid and the conjugate base:
(a) HNO3 + H2O
HClO4 + CH3NH2
[Cu(H2O)6]2+ + H2O
NO3- + H3O+
ClO4- + CH3NH3+
[Cu(H2O)5OH]+ + H3O+
Consider the acid HA.
Write the acid dissociation reaction for HA.
If HA is a strong acid, where will the equilibrium position be?
Will Ka be small or large if HA is a strong acid?
Would you expect the conjugate base of HA to be a stronger or weaker base
than water?
If HA is a strong acid, what will be the major species present at equilibrium?
Provide definitions of each of the following:
Lewis Acid / Lewis Base
Lowry Bronsted Acid / Lowry Bronsted Base
Arrhenius Acid / Arrhenius Base
What would happen to the pH of a sample of water if each of the following salts
were dissolved in it? Provide simple explanations for each answer.
A 0.75 M solution of hydrofluoric acid (HF – Ka = 6.8 x10-4) is made up for a
particular experiment in a General Chemistry lab, but the person making it up
forgot to check the pH before he left the lab. What is the pH of this solution?