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

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1			Which of the following is not a characteristic property of bases?
			A)	taste bitter
			B)	turn litmus from pink to blue
			C)	neutralize acids
			D)	react with carbonates to produce carbon dioxide gas
			E)	feel slippery
2			Calculate the hydroxide ion concentration of a solution if its pH is 6.389.
			A)	1.00 x 10-14 mol/L
			B)	4.08 x 10-7 mol/L
			C)	9.92 x 10-7 mol/L
			D)	2.45 x 10-8 mol/L
			E)	none of the above
3			What is the hydronium ion concentration in a solution with a pH of 2.80?
			A)	6.3 x 102 mol/L
			B)	1.6 x 10-3 mol/L
			C)	6.3 x 10-2 mol/L
			D)	4.8 x 10-8 mol/L
			E)	5.0 x 10-7 mol/L
4			Consider the reaction of the base, ammonia (NH3), with water. The conjugate acid of NH3 is
			A)	H3O+
			B)	NH4+
			C)	NH2-
			D)	OH-
			E)	NH2+
5			Which of the following is a correct description of the natural direction of a Brønsted-Lowry acid-base reaction?
			A)	weaker acid + weaker base → stronger acid + stronger base
			B)	weaker acid + stronger base → stronger acid + weaker base
			C)	stronger acid + weaker base → weaker acid + stronger base
			D)	stronger acid + stronger base → weaker acid + weaker base
			E)	None of the above statements is always correct.
6			Calculate the acid-dissociation constant (Ka) for a weak acid (HA) if a 0.50 M HA solution has a hydronium ion concentration of 3.0 x 10-4M.
			A)	6.0 x 10-4
			B)	5.0 x 10-6
			C)	9.0 x 10-8
			D)	6.0 x 10-6
			E)	1.8 x 10-7
7			What is the pH of a 0.20 M CH3COOH (acetic acid) solution? (Ka = 1.8 x 10-5)
			A)	5.4
			B)	2.7
			C)	5.7
			D)	2.0
			E)	4.0
8			Calculate the [HS-] of a 0.33 mol/L solution of H2S (Ka1 = 9.0 x 10-8; Ka2 = 1.0 x 10-17).
			A)	3.0 x 10-8 mol/L
			B)	9.0 x 10-8 mol/L
			C)	1.7 x 10-4 mol/L
			D)	3.0 x 10-4 mol/L
			E)	8.1 x 10-15 mol/L
9			In a 0.100 M HF solution, the percent dissociation is determined to be 9.5%. Calculate the Ka for HF based on this data.
			A)	9.5 x 10-2
			B)	1.0 x 10-3
			C)	3.1 x 10-3
			D)	7.6 x 10-4
			E)	9.5 x 10-4
10			What is the pH of a solution prepared from 0.250 mol of NH3 dissolved in sufficient water to make 1.00 L of solution? (Kb = 1.8 x 10-5)
			A)	2.12
			B)	2.67
			C)	8.92
			D)	11.33
			E)	13.40
11			Which, if any, of the following is not a strong acid in water?
			A)	HF
			B)	HBr
			C)	HCl
			D)	HI
			E)	All four are strong acids in water.
12			Which of the following substances when dissolved in water will form an acid aqueous solution?
			A)	KI
			B)	Ba(OH)2
			C)	CH3COONa
			D)	NH4Cl
			E)	NaF
13			Which of the following substances when dissolved in water will form a basic aqueous solution?
			A)	KBr
			B)	CH3CO2Na
			C)	BaCl2
			D)	NO2
			E)	(CH3)3NHCl
14			Which, if any, of the following is an example of the leveling effect?
			A)	The concentrations of H+ and OH- in pure water are equal.
			B)	The number of strong acids equals the number of strong bases.
			C)	The number of strong acids equals the number of weak acids.
			D)	In water, no acid stronger than H3O+ can exist.
			E)	None of the above is an example of the leveling effect.
15			Which of the following reactions illustrate Al(OH)3 acting as a Lewis acid?
			A)	Al(OH)3 → Al3+ + 3OH-
			B)	Al(OH)3 + OH- → Al(OH)2O- + H2O
			C)	Al(OH)3 + OH- → Al(OH)4-
			D)	Al(OH)3 + 3H+ → Al3+ + 3H2O
			E)	Al3+ + 3OH- → Al(OH)3