GT chemistry – review guide for acids, bases and equilibrium
NH3 + H+  NH4+
Arhenius – yes or no? Why?
Brønsted – yes or no? Why?
Lewis? yes or no? Why?
NH3 + H2O  NH4+ + OHArhenius – yes or no? Why?
Brønsted – yes or no? Why?
Lewis? yes or no? Why?
HCH3COO + H2O  H3O+ + CH3COOArhenius – yes or no? Why?
Brønsted – yes or no? Why?
Lewis? yes or no? Why?
NH4+ + CH3COO-  NH3 + HCH3COO
Arhenius – yes or no? Why?
Brønsted – yes or no? Why?
Lewis? yes or no? Why?
For each acid, name the acid. Then write out an equation that shows the dissociation of the
acid. Label the conjugate base. Some acids may have more than dissociation and therefore
more multiple conjugate bases.
HCl
HCH3COO
H3PO4
H2CO3
HNO3
HNO2
Give a mathematical definition for each of the following:
pH
pOH
Ka
pKa
Complete the following table
pH
[H30+]
pOH
[OH-]
Acid, base or
neutral?
2.1
6.8 X 10-8
2.1
6.8 X 10-8
neutral
What is the pH of a 3.5 X 10-3 HCl solution?
If 25.2 ml of a base is required to titrate 42.5 ml of a 3.00 M acid solution to equivalance,
what was the molarity of the base?
If the pKa of acetic acid is 4.76, what is the pH of a 0.01 M acetic acid solution?
Magesium Hydroxide has a Ksp of 1.5 X 10-11, and fully dissociates according to the
following reaction:
Mg(0H)2  Mg2+ + 2OHGiven this Ksp, find the hydroxide ion concentration [OH-] resulting from a 1.0 M Mg(OH)2
solution.
What is the pOH of this solution?
What is the pH of this solution?
Consider the following equation:
H2 (g) + I2 (g)  2 HI(g)
Calculate Keq if at 300oK the concentrations are [H2] = 0.40 M
[I2] = 0.45 M ; [HI] = 0.30 M
In the above scenario, what direction would equilibrium shift if pressure were increased?
Explain why.
The production of ammonia from Nitrogen and Hydrogen gases is carried out under high
heat and high pressure. Here is the reaction:
N2(g) + 3H2(g)  2NH3(g) + heat
Keq for this reaction is 1.4 X 10-4. If one had of 0.602 mol/L N2 and 0.420 mol/L of H2, how
many mol/L of ammonia would be present?
Using what you know about gasses and Le Chatelier’s principle, why must pressure be
constantly applied to maintain production of ammonia?
In the production of ammonia, increasing the total pressure (by decreasing volume) would
have what effect on equilibrium?
If additional heat were applied, what direction would equilibrium shift?
I have discovered a ridiculous compound with a formula of A3B2. If a saturated solution of
this stuff had a molar concentration of 4.6 X 10-2, what is the Ksp for my compound?