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

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1			According to the solubility rules, which of the following compounds will be soluble in water?
			A)	PbCl2
			B)	AgBr
			C)	BaSO4
			D)	Ca3(PO4)2
			E)	(NH4)3PO4
2			Which of the following compounds is a nonelectrolyte?
			A)	CH3COOH (acetic acid)
			B)	NaCl
			C)	KOH
			D)	C2H5OH (ethanol)
			E)	NH3
3			Which of the following compounds is insoluble in water?
			A)	CuSO4
			B)	PbCl2
			C)	Pb(C2H3O2)2
			D)	HCl
			E)	NH3
4			When aqueous solutions of Ba(OH)2 and H2SO4 are mixed, a reaction occurs. What ions, if any, are the spectator ions in this reaction?
			A)	Ba2+ and OH-
			B)	H+ and SO42-
			C)	Ba2+ and SO42-
			D)	H+ and OH-
			E)	There are no spectator ions since all of them react.
5			The correct net ionic equation for the process which occurs when aqueous solutions of the electrolytes AgNO3 and Na2S are mixed is:
			A)	NO3-(aq) + Na+(aq) → NaNO3(s)
			B)	2Ag+(aq) + S2-(aq) → Ag2S(s)
			C)	Ag+(aq) + S-(aq) → AgS(s)
			D)	Ag+(aq) + NO3-(aq) → AgNO3(s)
			E)	no reaction occurs
6			Aqueous copper(II) nitrate reacts with potassium iodide to yield solid copper(I) iodide, aqueous potassium nitrate, and solid iodine. The balanced net ionic equation for the reaction is:
			A)	2Cu2+(aq) + 4I-(aq) → 2CuI(s) + I2(s)
			B)	K+(aq) + 3I-(aq) → KI(s) + I2(s)
			C)	Cu2+(aq) + I-(aq) → CuI(s) + I2(s)
			D)	K+(aq) + NO3-(aq) → KNO3(s)
			E)	None of the above.
7			The net ionic equation for the reaction between aqueous solutions of HCl and NH3 is
			A)	HCl(aq) + NH3(aq) → NH4Cl(aq)
			B)	H+(aq) + NH3(aq) → NH4+(aq)
			C)	H+(aq) + OH-(aq) → H2O(l)
			D)	H+(aq) + Cl-(aq) + NH3(aq) → NH4Cl(aq)
			E)	H+(aq) + Cl-(aq) + NH3(aq) → NH4+(aq) + Cl-(aq)
8			During a titration, the following data were collected. A 25 mL portion of an unknown acid solution was titrated with 1.0 M NaOH. It required 65 mL of the base to neutralize the sample. How many moles of acid are present in 3.0 liters of this unknown solution?
			A)	2.6 moles
			B)	0.9 moles
			C)	8.7 moles
			D)	7.8 moles
			E)	5.6 moles
9			What volume of a 0.100 M solution of HCl is required to neutralize a solution prepared by dissolving 10.0 g of KOH in 250 ml of H2O?
			A)	0.178 L
			B)	0.25 L
			C)	0.71 L
			D)	1.78 L
			E)	178 L
10			What are the products when aqueous solutions of HCl and Na2CO3 react?
			A)	NaCl and HCO3
			B)	NaCl, H2O and CO2
			C)	NaCl and HCO3-
			D)	NaH and Cl2CO3
			E)	None of the above
11			In a reaction in which the SO32- ion is converted into S2O42-, the sulfur
			A)	is oxidized.
			B)	is reduced.
			C)	is the oxidizing agent.
			D)	disproportionates.
			E)	does not undergo a redox process.
12			The oxidation state of vanadium in Rb4Na[HV10O28] is:
			A)	-6
			B)	+8
			C)	-5
			D)	+3
			E)	+5
13			Equation: 3Cu(s) + 8HNO3(aq) → 2NO(g) + 3Cu(NO3)2(aq) + 4H2O(l) In the above reaction, the element oxidized is ______, the reducing agent is ______ and the number of electrons transferred from reducing to oxidizing agent in the equation, as written, is ______.
			A)	Cu, Cu, 6
			B)	Cu, N, 6
			C)	N, Cu, 6
			D)	Cu, Cu, 2
			E)	N, N, 3
14			What is the total number of electrons transferred when the equation below is balanced? Equation: I2 + ClO3- + H2O → IO3- + Cl- + H+ (in acid)
			A)	5
			B)	6
			C)	12
			D)	24
			E)	30
15			Which of the following is a halogen displacement reaction?
			A)	Fe2O3(s) + 2Al(s) → 2Fe(s) + Al2O3(s)
			B)	2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
			C)	CaBr2(aq) + H2SO4(aq) → CaSO4(s) + 2HBr(g)
			D)	2P(s) + 3Cl2(g) → 2PCl3(g)
			E)	none of the above