Acids and Bases Multiple Choice Test
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Click in the appropriate box for each question, then click "Done" at the bottom.
10 marks for each correct answer. Hints cost 5 marks each.



1. Ammonia is a base because:
When dissolved in water, OH- ions are produced
The nitrogen can donate a lone pair to an acid
The nitrogen can accept a proton from an acid
None of the above     
All of the above
2. In an acid-base reaction:
Water will always act as a base, capturing a proton from the acid
Water will always act as an acid, giving up a proton to the base
A proton will be transferred from the acid to the base
A proton will be transferred from the base to the acid
Water is always a product of the reaction

3. HClO2(aq) is a stronger acid than HClO(aq) because:

The H atom in HClO2 is bound to the Cl atom
The Cl atom in HClO2 is more electronegative than that in HClO
The extra oxygen atom "pushes" the H atom off of the HClO2 molecule
The extra oxygen atom pulls bonding electrons towards itself, weakening the O-H bond in HClO2
None of the above

4. HBr is a stronger acid than HCl because:
The Br atom is more electronegative than the Cl atom, making the H-Br bond weaker
The Cl atom is more electronegative than the Br atom making the H-Cl bond stronger
The Br atom is larger
Br- ions are more soluble than Cl- ions 
None of the above

5. Perchloric acid, HClO4, is a strong acid. Which of the following statements is true?
Solutions of HClO4 will contain insignificant quantities of undissociated HClO4 molecules
The perchlorate ion, ClO4-, is a weak base
Ka of perchloric acid is large
In an aqueous solution of HClO4, [H3O+][OH-] = Kw
All of the above
6.  Dimethyl amine, (CH3)2NH, is a weak base. Which of the following is true?
Upon addition of a strong acid to aa aqueous solution of dimethylamine, a salt will be produced
The proton from an acid will be attracted to the lone pair on the N atom of the base
(CH3)2NH2+ is a strong acid
Aqueous solutions of dimethylamine will contain very little (CH3)2NH2+ 
All of the above
7.  For the polyprotic acid H3PO4 dissolved in water:
Ka1 < Ka2 < Ka3
The predominant species in solution is PO4-3
The predominant species in solution is HPO4-2
The solution is acidic mostly due to the hydrolysis of H2PO4-
None of the above

8. If NaNO2(s) is added to an aqueous solution of the weak acid HNO2: 
The pH rises
The pH falls
The pH is unaffected

9. Assume you have a basic buffer system composed of ammonia and ammonium chloride.
The Henderson-Hasselbach equation is pH = pKa - log{[acid]/[base]}. Here, the acid and 
base are:
H3O+ and OH-
H3O+ and H2O
NH3 and NH4+
NH4+ and NH3
NH4+ and OH-

10. CaF2 is a sparingly soluble salt. HF is a weak acid. If the pH of a solution of CaF2 is 
lowered, the solubility of CaF2 will:
Increase
Decrease
Not change