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1		If an acid HA has Ka = 10-5, what is the pH of a mixture of 0.1 mole of the acid and 0.1 mole of its conjugate base in 1.0 liter of water?
			A)	5
			B)	9
			C)	3
			D)	4
			E)	6
2		A solution contains equimolar amounts of NaH2PO4 and Na2HPO4. What is its pH? (for H3PO4, the Ka values are, respectively, 7.5 x 10-3; 6.2 x 10-8; 4.8 x 10-13)
			A)	3
			B)	5
			C)	7
			D)	9
			E)	13
3		What is the optimum pH of a sodium formate/formic acid buffer? (Ka = 1.7 x 10-4)
			A)	7.0
			B)	6.2
			C)	3.8
			D)	3.0
			E)	1.7
4		A buffer is prepared by mixing 100 mL of 0.500 M HCl and 200 mL of 0.500 M sodium acetate. The Ka for acetic acid is 1.8 x 10-5. Calculate the pH of the buffer.
			A)	4.44
			B)	4.74
			C)	5.05
			D)	5.45
			E)	6.13
5		A sample of vinegar (dilute acetic acid) weighing 5.056 g is titrated with 30.25 mL of 0.1022 M NaOH. What is the weight percent of acetic acid (CH3COOH) in the sample?
			A)	3.025%
			B)	3.669%
			C)	3.710%
			D)	4.221%
			E)	4.302%
6		An acid with a Ka of 1 x 10-8 is titrated with NaOH, both solutions being 0.020 M. What should the Ka of the indicator be, in order to obtain the best end point?
			A)	10-4
			B)	10-6
			C)	10-7
			D)	10-8
			E)	10-10
7		Consider the titration of 0.1000 M HBr with 0.1000 M KOH. Calculate the pH after 55.00 mL of the base has been added to 50.00 mL of the HBr solution.
			A)	6.62
			B)	7.35
			C)	8.90
			D)	11.68
			E)	12.50
8		Consider the titration of 0.1000 M NH3 (Kb = 1.76 x 10-5) with 0.1000 M HNO3. The pH at the equivalence point is
			A)	between 2.0 and 4.0
			B)	between 4.5 and 6.5
			C)	approximately 7.0
			D)	between 7.5 and 9.5
			E)	between 11.0 and 13.0
9		Which one of the following gases is not involved in producing acidic precipitation?
			A)	SO2
			B)	SO3
			C)	NO
			D)	N2O
			E)	NO2
10		What is the solubility product constant expression (Ksp) for PbCl2?
			A)	[Pb2+](2)[Cl-]
			B)	[Pb2+] [Cl-]/2
			C)	[Pb2+][Cl-]2/[PbCl2]
			D)	[Pb2+] [Cl-]/[PbCl2]
			E)	[Pb2+][Cl-]2
11		The molar solubility of PbCl2 is 3.9 x 10-2 mol/L. What is the Ksp of PbCl2?
			A)	5.9 x 10-5
			B)	4.1 x 10-5
			C)	1.5 x 10-3
			D)	2.4 x 10-4
			E)	3.9 x 10-2
12		Calculate the pH of a saturated solution of Mg(OH)2 (Ksp for Mg(OH)2 = 1.2 x 10-11)
			A)	3.5
			B)	10.2
			C)	10.5
			D)	11.0
			E)	11.3
13		Calculate the concentration of calcium ions in a saturated calcium phosphate solution. (Ksp for Ca3(PO4)2 = 1.3 X 10-26)
			A)	1.2 x 10-5 mol/L
			B)	2.0 x 10-5 mol/L
			C)	6.6 x 10-6 mol/L
			D)	7.8 x 10-6 mol/L
			E)	8.3 x 10-6 mol/L
14		Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (Ksp for Ag2CO3 = 8.1 x 10-12)
			A)	8.1 x 10-12 M
			B)	2.8 x 10-6 M
			C)	1.4 x 10-6 M
			D)	1.4 x 10-8 M
			E)	2.0 x 10-4 M
15		Calculate the concentration of uncomplexed silver ions in a solution that contains 0.10 M Ag(NH3)2+ and 1.0 M NH3. (Kf for Ag(NH3)2+ = 1.5 x 107)
			A)	6.7 x 10-8 M
			B)	6.7 x 10-9 M
			C)	1.5 x 10-7 M
			D)	0.15 M
			E)	8.2 x 10-5 M