Chemistry: Molecular Nature of Matter and Change, 6th Edition (Silberberg)

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1			Which, if any, of the following will not form a basic solution when dissolved in water?
			A)	NaOH
			B)	Ca(OH)2
			C)	CH3OH
			D)	N(CH3)3
			E)	All of the above will form basic aqueous solutions.
2			When 10.0 mL of a solution of a strong acid at pH = 2.50 is mixed with 10.0 mL of a strong acid at pH = 6.50, what is the pH of the resulting solution?
			A)	5.50
			B)	8.50
			C)	3.80
			D)	4.50
			E)	2.80
3			What is the pH of a 675 mL aqueous solution containing 0.036 mol of NaOH?
			A)	3.41
			B)	10.58
			C)	12.73
			D)	1.27
			E)	13.00
4			Which of the following pairs of species is not a conjugate acid-base pair?
			A)	HCl and H+
			B)	HSO4- and SO42-
			C)	H2SO4 and HSO4-
			D)	H2O and OH-
			E)	NH3 and NH2-
5			For which one of the following reactions is the equilibrium constant Kc > 1? Need a Hint?
			A)	CH3COOH + H2O → CH3COO- + H3O+
			B)	CH3COOH + OH- → CH3COO- + H2O
			C)	NH4+ + H2 → NH3 + H2O+
			D)	Cl- + H2O → HCl + OH-
			E)	HSO4- + H3O+ → H2SO4 + H2O
6			Calculate Ka for a monoprotic acid whose 0.30 M solution has a pH of 2.32. HA + H2O → H3O+ + A-
			A)	4.8 x 10-3
			B)	2.3 x 10-5
			C)	7.6 x 10-5
			D)	6.9 x 10-6
			E)	none of the above
7			Calculate the pH of a 0.450 M solution of NH4Cl (Kb for NH3 is 1.8 x 10-5).
			A)	4.45
			B)	2.52
			C)	5.60
			D)	4.80
			E)	9.60
8			Ascorbic acid is a diprotic acid, H2As, where As2- is the ascorbate ion. What is the ascorbate ion concentration in a 0.1 mol/L solution of H2As? (Ka1 = 8.0 x 10-5, Ka2 = 3.0 x 10-12)
			A)	3.0 x 10-12 mol/L
			B)	8.0 x 10-5 mol/L
			C)	5.5 x 10-7 mol/L
			D)	3.0 x 10-6 mol/L
			E)	1.7 x 10-6 mol/L
9			A 0.20 M NH3 solution is 1.7 % ionized. Calculate the H+ concentration. NH3 + H2O → NH4+ + OH-
			A)	2.9 x 10-12 M
			B)	3.4 x 10-3 M
			C)	2.9 x 10-14 M
			D)	0.17 M
			E)	0.20 M
10			An acid HA has a Ka of 10-7. What is the pH of a 0.1 M solution of its conjugate base?
			A)	5.0
			B)	7.0
			C)	8.0
			D)	10.0
			E)	13.0
11			Consider each of the following pairs of acids. Which statement is correct?
			A)	HClO is a stronger acid than HClO3.
			B)	H2SO3 is a stronger acid than H2SO4.
			C)	NH3 is a stronger acid than H2O.
			D)	HBr is a stronger acid than H2S.
			E)	CCl3COOH is a stronger acid than CF3COOH.
12			Consider each of the following pairs of acids. Which statement is correct?
			A)	HClO2 is a stronger acid than HClO4.
			B)	H2SO4 is a stronger acid than H2SeO4.
			C)	H2O is a stronger acid than HF.
			D)	H2S is a stronger acid than H2Se.
			E)	HS- is a stronger acid than H2S.
13			Which of the following statements about acids and bases is incorrect?
			A)	The strongest acid that can exist in water is H3O+.
			B)	All strong acids in water are leveled to the same strength.
			C)	Any base which is stronger than OH- will react with water to produce OH-.
			D)	The relative strength of strong acids can be measured by using a solvent which is a weaker base than water.
			E)	The oxide ion is a weaker base than OH-.
14			Consider the reaction CH3NH2 + H2O → CH3NH3+ + OH- where CH3NH2 is methylamine and CH3NH3+ is the methylammonium ion. Select the correct description of this reaction in terms of Lewis acid-base theory.
			A)	Methylamine serves as a Lewis acid in the forward reaction and methylammonium ion serves as a Lewis base in the reverse reaction.
			B)	Water serves as a Lewis base in the forward reaction and the hydroxide ion serves as a Lewis base in the reverse reaction.
			C)	Methylamine serves as a Lewis base in the forward reaction and hydroxide ion serves as a Lewis acid in the reverse reaction.
			D)	Water serves as a Lewis acid in the forward reaction and methylammonium ion serves as a Lewis base in the reverse reaction.
			E)	Methylamine serves as a Lewis base in the forward reaction and hydroxide ion serves as a Lewis base in the reverse reaction.
15			Which of the following is most likely to act as a Lewis acid?
			A)	NH3
			B)	F-
			C)	H2O
			D)	BF3-
			E)	Zn2+