Chapter 8

How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.175 M NaOH solution?

3.50

Which of the following compounds is soluble in water? A) CaS B) MgCO3 C) Pb I2 D) SrSO4 E) None of these compounds is soluble in water.

A) CaS

Identify the oxidation state of Ca in Ca(s). Ca(s) + 2H F(aq) → Ca F2(aq) + H2(g) A) +1 B) +2 C) 0 D) -1 E) -2

C) 0

How many H+ ions can the acid, H2SeO4 , donate per molecule? A) 0 B) 1 C) 2 D) 3

C) 2

How many of the following compounds are insoluble in water? NaC2H3O2 BaSO4 SrS AlPO4 A) 0 B) 1 C) 2 D) 3 E) 4

C) 2

Identify HCl. A) strong electrolyte, weak acid B) weak electrolyte, weak acid C) strong electrolyte, strong acid D) weak electrolyte, strong acid E) nonelectrolyte

C) strong electrolyte, strong acid

Identify K OH. A) weak acid B) weak electrolyte C) strong acid D) strong electrolyte E) nonelectrolyte

D) strong electrolyte

Identify Na Cl. A) weak acid B) weak electrolyte C) strong acid D) strong electrolyte E) nonelectrolyte

D) strong electrolyte

Give the name for HNO2.

nitrous acid

Determine the oxidation state of Mn in KMnO4.

+7

How many moles of are present in 0.550 L of a 0.550 M solution of Co ?

0.303

Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250 mL

0.350

There are ________ mol of bromide ions in 0.500 L of a 0.300M solution of Al .

0.450

What is the concentration (M) of C OH in a solution prepared by dissolving 3.96 g of C OH in sufficient water to give exactly 230 mL of solution?

0.538

What is the concentration (M) of a NaCl solution prepared by dissolving 5.3 g of NaCl in sufficient water to give 115 mL of solution?

0.79

What is the concentration (M) of sodium ions in 4.57 L of a .533 M P solution?

1.60

How many grams of P are in 325 mL of a 5.50 M solution of P ?

175

How many grams of C OH must be added to water to prepare 175mL of a solution that is 1.0 M CH3OH?

5.6

Explain the difference between a strong and weak electrolyte. Give an example of each

A strong electrolyte is either an ionic compound that is soluble in water or a molecular compound that ionizes completely in water. Possible examples are NaCl or HCl. A weak electrolyte is only slightly soluble or does not ionize to any great extent in water. Possible examples are AgCl or HC2H3O2.

Identify the oxidation state of H in H F(aq). Ca(s) + 2H F(aq) → Ca F2(aq) + H2(g) A) +1 B) +2 C) 0 D) -1 E) -2

A) +1

Determine the oxidation state of P in PO33-. A) +3 B) +6 C) +2 D) 0 E) -3

A) +3

Determine the oxidation state of C in CO3-2. A) +4 B) +2 C) -2 D) -4 E) +6

A) +4

Determine the oxidation state of nitrogen in NaNO3. A) +5 B) +3 C) 0 D) +2 E) +4

A) +5

In an acid-base neutralization reaction 23.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution? A) 0. 119 M B) 0. 237 M C) 0. 475 M D) 2.11 M

A) 0. 119 M

What is the molarity of a potassium triiodide solution, KI3(aq), if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0. 300 M thiosulfate solution, K2S2O3(aq)? The chemical equation for the reaction is 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq). A) 0. 125 M B) 0. 180 M C) 0. 250 M D) 0.500 M

A) 0. 125 M

A student prepared a stock solution by dissolving 15.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution? A) 0. 411 M B) 0. 534 M C) 1.87 M D) 2.43 M

A) 0. 411 M

How many grams of CaCl2 are formed when 25.00 mL of 0.00237 M Ca(OH)2 reacts with excess Cl2 gas? 2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l) A) 0.00 329 g B) 0.00 658 g C) 0.0 132 g D) 0.0 304 g

A) 0.00 329 g

Which of the following solutions will have the highest electrical conductivity? A) 0.045 M Al2(SO4)3 B) 0.050 M (NH4)2CO3 C) 0.10 M NaBr D) 0.10 M KI E) 0.10 M KF

A) 0.045 M Al2(SO4)3

What is the concentration of magnesium ions in a 0.125 M Mg SO4 solution? A) 0.125 M B) 0.0625 M C) 0.375 M D) 0.250 M E) 0.160 M

A) 0.125 M

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)? A) 0.20 M B) 0.40 M C) 0.10 M D) 0.36 M E) 0.25 M

A) 0.20 M

When 7.80 mL of 0.500 M AgNO3 is added to 6.25 mL of 0.300 M NH4Cl, how many grams of AgCl are formed? AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq) A) 0.269 g B) 0.553 g C) 0.822 g D) 1.61 g

A) 0.269 g

What is the molarity of a NaOH solution if 39.1 mL of a 0.112 M solution is required to neutralize a 25.0-mL sample of the NaOH solution? A) 0.350 B) 0.0716 C) 0.143 D) 54.7 E) 0.175

A) 0.350

A beaker contains 0.50 mol of potassium bromide in 600 mL of water. An additional 600 mL of water is added. The number of moles of potassium bromide in the beaker is A) 0.50 mol. B) 0.83 mol. C) 0.25 mol. D) 1.2 mol. E) 0.42 mol

A) 0.50 mol.

A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M . What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL. A) 0.713 B) 0.613 C) 0.130 D) 0.230 E) 0.513

A) 0.713

According to the balanced equation shown below, 2.00 moles of oxalic acid, H2C2O4, reacts with ________ moles of permanganate, MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l) A) 0.800 B) 2.00 C) 4.00 D) 4.50

A) 0.800

What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution? 2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq) A) 0.838 g B) 1.72 g C) 0.859 g D) 2.56 g E) 1.70 g

A) 0.838 g

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. A) 1.50 M B) 1.18 M C) 0.130 M D) 0.768 M E) 2.30 M

A) 1.50 M

How many milliliters of 0.260 M Na2S are needed to react with 25.00 mL of 0.315 M AgNO3? Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s) A) 15.1 mL B) 30.3 mL C) 41.3 mL D) 60.6 mL

A) 15.1 mL

How many ions are present in 30.0 mL of 0.600 M H2CO3 solution? A) 3.25 × 1022 ions B) 2.17 × 1022 ions C) 1.08 × 1022 ions D) 5.42 × 1022 ions E) 3.61 × 1021 ions

A) 3.25 × 1022 ions

What is the concentration of an AlCl3 solution if 150. mL of the solution contains 550. mg of Cl- ion? A) 3.45 × 10-2 M B) 8.25 × 10-2 M C) 1.03 × 10-1 M D) 3.10 × 10-1 M

A) 3.45 × 10-2 M

How many moles of CH3CH2Cl are contained in 548 mL of 0.0788 M CH3CH2Cl solution? A) 4.32 × 10-2 mol B) 2.32 × 10-2 mol C) 6.95 × 10-2 mol D) 1.44 × 10-2 mol E) 5.26 × 10-2 mol

A) 4.32 × 10-2 mol

Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 8.00 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ________ NH3(g) + ________ O2(g) →________ NO(g) + ________ H2O(l) A) 4.88 L B) 7.38 L C) 11.5 L D) 17.3 L

A) 4.88 L

Choose the statement below that is TRUE. A) A weak acid solution consists of mostly nonionized acid molecules. B) The term "strong electrolyte" means that the substance is extremely reactive. C) A strong acid solution consists of only partially ionized acid molecules. D) The term "weak electrolyte" means that the substance is inert. E) A molecular compound that does not ionize in solution is considered a strong electrolyte

A) A weak acid solution consists of mostly nonionized acid molecules.

Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s) A) Ag B) Ni C) Cl D) O E) This is not an oxidation-reduction reaction

A) Ag

Which of the following compounds is insoluble in water? A) Ag Cl B) (NH4)3PO4 C) FeSO4 D) SrS E) All of these compounds are soluble in water

A) Ag Cl

What reagent could be used to separate Br- from N O3- when added to an aqueous solution containing both? A) AgNO3(aq) B) Ba(OH)2(aq) C) CuSO4(aq) D) NaI(aq)

A) AgNO3(aq)

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed. A) H+(aq) + OH-(aq) → H2O(l) B) 2 K+(aq) + SO42-(aq) → K2SO4(s) C) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s) D) H22+(aq) + OH-(aq) → H2(OH)2(l) E) No reaction occurs.

A) H+(aq) + OH-(aq) → H2O(l)

Identify the polyprotic acid. A) H2SO4 B) HCl C) Li I D) NaOH E) Ba(OH)2

A) H2SO4

Which of the following compounds is insoluble in water? A) Hg2Cl2 B) MgSO4 C) (NH4)2CO3 D) BaS E) All of these compounds are soluble in water.

A) Hg2Cl2

The mixing of which pair of reactants will result in a precipitation reaction? A) Mg(NO3)2(aq) + Na2CO3(aq) B) K2SO4(aq) + Cu(NO3)2(aq) C) NaClO4(aq) + (NH4)2S(aq) D) NH4Br(aq) + NH4I(aq)

A) Mg(NO3)2(aq) + Na2CO3(aq)

Which of the compounds H3PO4 , Mg(OH)2, LiOH, and H Cl, behave as bases when they are dissolved in water? A) Mg(OH)2 and LiOH B) H3PO4 and H Cl C) only H Cl D) only LiOH

A) Mg(OH)2 and LiOH

When an aqueous solution of manganese (II) nitrate is combined with an aqueous solution of ammonium sulfide, what should precipitate out? A) MnS B) Mn(SO3)2 C) Mn(SO4)2 D) Mn2SO3 E) Mn2SO4

A) MnS

Which of the following is considered a strong electrolyte? A) NH4NO3 B) C12H22O11 C) Pb I2 D) HC2H3O2 E) CH3SH

A) NH4NO3

What element is undergoing oxidation (if any) in the following reaction? Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s) A) Zn B) N C) O D) Ag E) This is not an oxidation-reduction reaction.

A) Zn

An aqueous solution of H F is named A) hydrofluoric acid. B) hydrofluorous acid. C) fluoric acid. D) fluorous acid.

A) hydrofluoric acid.

How can you tell if a reaction is an oxidation-reduction reaction?

At least one species is losing electrons while at least one other species is gaining electrons. This can be evaluated by assigning oxidation numbers to each element present and looking to see if these change from reactant to product.

Identify the oxidation state of Ca in Ca Br2(aq). Ca(s) + 2H Br(aq) → Ca Br2(aq) + H2(g) A) +1 B) +2 C) 0 D) -1 E) -2

B) +2

Determine the oxidation state of nitrogen in RbNO2. A) +5 B) +3 C) 0 D) +2 E) +4

B) +3

Determine the oxidation state of Ti in Ti(SO4)2. A) +2 B) +4 C) +6 D) 0 E) -2

B) +4

What is the oxidation number of the oxygen atom in O22-? A) -2 B) -1 C) +1 D) +2

B) -1

What is the oxidation number change for the manganese atom in the following unbalanced reduction half reaction? A) -7 B) -5 C) +5 D) +7

B) -5

What volume of a 0.540 M NaOH solution contains 12.5 g of NaOH? A) 0. 169 L B) 0. 579 L C) 1. 73 L D) 5.92 L

B) 0. 579 L

What is the concentration of FeCl3 in a solution prepared by dissolving 30.0 g of FeCl3 in enough water to make 275 mL of solution? A) 6.73 × 10-4 M B) 0. 673 M C) 1.49 M D) 1.49 × 103 M

B) 0. 673 M

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution. A) 0.0297 M B) 0.0337 M C) 0.0936 M D) 0.0107 M E) 0.0651 M

B) 0.0337 M

If 100. mL of 0.200 M Na2SO4 is added to 200. mL of 0.300 M NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive. A) 0.267 M B) 0.333 M C) 0.500 M D) 0.700 M

B) 0.333 M

How many moles of Na I are required to make 250 mL of a 3.00 M solution? A) 750 moles B) 0.750 moles C) 3 moles D) 0.250 moles

B) 0.750 moles

How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 mL of 0.140 M sucrose solution? A) 8.29 × 1022 molecules C12H22O11 B) 1.21 × 1021 molecules C12H22O11 C) 6.15 × 1022 molecules C12H22O11 D) 1.63 × 1023 molecules C12H22O11 E) 5.90 × 1024 molecules C12H22O11

B) 1.21 × 1021 molecules C12H22O11

Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 40.00 mL of 0.00150 M calcium hydroxide. ________ Ca(OH)2(aq) + ________ H3PO4(aq) → ________ Ca3(PO4)2(aq) + ________ H2O(l) A) 2.70 mL B) 13.3 mL C) 20.0 mL D) 30.0 mL

B) 13.3 mL

Which of the following is an acid-base reaction? A) C(s) + O2(g) → CO2(g) B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq) C) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq) D) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s) E) None of the above are acid base reactions.

B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)

How many sodium ions are present in 30.0 mL of 0.600 M Na2CO3 solution? A) 3.25 × 1022 ions B) 2.17 × 1022 ions C) 1.08 × 1022 ions D) 5.42 × 1022 ions E) 3.61 × 1021 ions

B) 2.17 × 1022 ions

How many milliliters of a stock solution of 12.1 M would be needed to prepare 0.500 L of 0.500 M ? A) 0.0484 B) 20.7 C) 3.03 D) 48.4 E) 0.0207

B) 20.7

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: (aq) + (aq) → (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.500 mol of to completely precipitate the lead? A) 3.55 × 10-3 mL B) 282 mL C) 141 mL D) 0.141 mL E) 0.282 mL

B) 282 mL

According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO3)2. 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) A) 7.19 g B) 3.59 g C) 1.80 g D) 5.94 g E) 1.30 g

B) 3.59 g

Determine the oxidation state of fluorine in F2. A) +5 B) +3 C) 0 D) +2 E) +4

C) 0

What is the concentration of HCl in the final solution when 65 mL of a 9.0 M HCl solution is diluted with pure water to a total volume of 0.15 L? A) 2.1 × 10-2 M B) 3.9 M C) 21 M D) 3.9 × 103 M

B) 3.9 M

A FeCl3 solution is 0.175 M. How many mL of a 0.175 M FeCl3 solution are needed to make 650. mL of a solution that is 0.300 M in Cl- ion? A) 1.11 mL B) 371 mL C) 1110 mL D) It is not possible to make a more concentrated solution from a less concentrated solution.

B) 371 mL

How many milliliters of a 0.266 M CsNO3 solution are required to make 150.0 mL of 0.075 M CsNO3 solution? A) 53.2 mL B) 42.3 mL C) 18.8 mL D) 23.6 mL E) 35.1 mL

B) 42.3 mL

What precipitate is most likely formed from a solution containing Ba+2, K+1, OH-1, and CO3-2. A) KOH B) BaCO3 C) K2CO3 D) Ba(OH)2

B) BaCO3

Which of the following is a strong electrolyte in solution? A) CdS B) FeCl3 C) CH3COOH D) NiC2O4 E) PbMnO4

B) FeCl3

Which of the compounds of H CO2H , Ba(OH)2, CsOH, and H Br, behave as acids when they are dissolved in water? A) Ba(OH)2 and CsOH B) H and H Br C) only H Br D) only CsOH

B) H and H Br

The chemical formula for sulfurous acid is A) H2S(aq). B) H2SO3(aq). C) H2SO4(aq). D) H2S2O7(aq).

B) H2SO3(aq)

Which of the following pairs of aqueous solutions will form a precipitate when mixed? A) NH4NO3 + Na2CO3 B) Hg2(NO3)2 + Li Cl C) NaCl + Li3PO4 D) AgC2H3O2 + Cu(NO3)2 E) None of the above solution pairs will produce a precipitate.

B) Hg2(NO3)2 + Li Cl

Identify the spectator ions in the following molecular equation. K Br(aq) + AgNO3(aq) → Ag Br(s) + KNO3(aq) A) Ag+ and Br B) K+ and NO3- C) K+ and Br D) Ag+ and NO3- E) There are no spectator ions in this reaction

B) K+ and NO3-

Which of the following compounds is NOT an Arrhenius acid? A) CH3CO2H B) N H3 C) HNO2 D) H2SO4

B) N H3

hen 220. mL of 1.50 × 10-4 M hydrochloric acid is added to 135 mL of 1.75 × 10-4 M Mg(OH)2, the resulting solution will be A) acidic. B) basic C) neutral. D) It is impossible to tell from the information given.

B) basic

What is the name for an aqueous solution of HIO? A) hydroiodic acid B) hypoiodous acid C) iodous acid D) iodic acid E) periodic acid

B) hypoiodous acid

Identify acetic acid. A) strong electrolyte, weak acid B) weak electrolyte, weak acid C) strong electrolyte, strong acid D) weak electrolyte, strong acid E) nonelectrolyte

B) weak electrolyte, weak acid

Determine the oxidation state of Cl in ClO3-. A) +1 B) +3 C) +5 D) +7 E) 0

C) +5

What is the oxidation number of the chromium atom in Na2CrO4 ? A) -2 B) +2 C) +6 D) +7

C) +6

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 7.00 g of K3PO4 in enough water to make 350. mL of solution? A) 0.0 236 M B) 0. 0943 M C) 0. 377 M D) 0. 754 M

C) 0. 377 M

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Sr(NO3)2 solution to 150.0 mL. A) 1.13 M B) 0.0887 M C) 0.0313 M D) 0.0199 M E) 0.0501 M

C) 0.0313 M

If 4.89 g of ZnCl2 is dissolved in enough water to give a total volume of 500 mL, what is the molarity of the solution? A) 0.217 M B) 0.0179 M C) 0.0717 M D) 1.33 M E) 0.849 M

C) 0.0717 M

Which of the following solutions will have the highest concentration of chloride ions? A) 0.10 M NaCl B) 0.10 M MgCl2 C) 0.10 M AlCl3 D) 0.05 M CaCl2 E) All of these solutions have the same concentration of chloride ions.

C) 0.10 M AlCl3

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)? A) 1.03 M B) 0.343 M C) 0.114 M D) 0.138 M E) 0.0461 M

C) 0.114 M

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: (aq) + (aq) → AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.175 M solution to completely precipitate the silver? A) 4.38 × g B) 7.49 × 10-5 g C) 0.256 g D) 0.0749 g E) 1.34 × 104 g

C) 0.256 g

Based on the balanced chemical equation shown below, determine the molarity of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required to completely react with 30.00 mL of a 0. 125 M potassium bromate, KBrO3(aq), solution. The chemical equation for the reaction is 6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l). A) 0. 0156 M B) 0. 0938 M C) 0.562 M D) 1.00 M

C) 0.562 M

A stock solution of is prepared and found to contain 12.1 M of . If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M. A) 0.242 B) 1.65 C) 0.605 D) 605 E) 242

C) 0.605

How many carbonate ions are present in 30.0 mL of 0.600 M H2CO3 solution? A) 3.25 × 1022 ions B) 2.17 × 1022 ions C) 1.08 × 1022 ions D) 5.42 × 1022 ions E) 3.61 × 1021 ions

C) 1.08 × 1022 ions

What is the molar concentration of sodium ions in a 0. 550 M Na3PO4 solution? A) 0. 183 M B) 0. 550 M C) 1.65 M D) 2.20 M

C) 1.65 M

According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl2. FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq) A) 3.97 × 10-2 moles B) 2.52 × 10-2 moles C) 1.99 × 10-2 moles D) 5.03 × 10-2 moles E) 6.49 × 10-2 moles

C) 1.99 × 10-2 moles

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is needed to completely react with 12.44 mL of 0.125 M KI3(aq), according to the following chemical equation. 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq) A) 3.11 mL B) 6.22 mL C) 12.4 mL D) 49.8 mL

C) 12.4 mL

Which of the following is a precipitation reaction? A) Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq) B) KCl(aq) + LiI(aq) → KI(aq) + LiCl(aq) C) 2 KI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 KNO3(aq) D) H Cl(aq) + LiOH(aq) → Li Cl(aq) + H2O(l) E) None of the above are precipitation reactions.

C) 2 KI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 KNO3(aq)

How many chloride ions are present in 65.5 mL of 0.210 M Al Cl3 solution? A) 4.02 × 1023 chloride ions B) 5.79 × 1024 chloride ions C) 2.48 × 1022 chloride ions D) 8.28 × 1021 chloride ions E) 1.21 × 1022 chloride ions

C) 2.48 × 1022 chloride ions

6.74 g of the monoprotic acid KHP (MW = 204.2 g/mol) is dissolved into water. The sample is titrated with a 0.703 M solution of calcium hydroxide to the equivalence point. What volume of base was used? A) 8.64 mL B) 11.8 mL C) 23.5 mL D) 47.0 mL E) 93.9 mL

C) 23.5 mL

How many milliliters of a 0.184 M RbNO3 solution contain 0.113 moles of RbNO3? A) 543 mL B) 163 mL C) 614 mL D) 885 mL E) 326 mL

C) 614 mL

How many grams of H2 gas can be produced by the reaction of 63.0 grams of Al(s) with an excess of dilute hydrochloric acid in the reaction shown below? 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g) A) 3.13 g B) 4.71 g C) 7.06 g D) 14.1 g

C) 7.06 g

What volume of 1.46 M CrBr2 solution is required to react with 50.0 mL of 0.210 M Na2CO3 solution? CrBr2(aq) + Na2CO3(aq) → CrCO3(s) + 2NaBr(aq) A) 139 mL B) 45.3 mL C) 7.19 mL D) 1.68 mL E) 34.6 mL

C) 7.19 mL

How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l) A) 0. 0158 mL B) 0.101 mL C) 9.86 mL D) 63.4 mL

C) 9.86 mL

What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) A) O B) H C) C D) both C and H E) None of the elements is undergoing oxidation.

C) C

Which of the following pairs of aqueous solutions will form a precipitate when mixed? A) K2CO3 + Na Br B) Na2 SO4 + LiOH C) CaS + Na2SO4 D) None of these solution pairs will produce a precipitate. E) All of these solution pairs will produce a precipitate

C) CaS + Na2SO4

Which one of the following compounds behaves as an acid when dissolved in water? A) CaO B) C2H6 C) H F D) NaOH

C) H F

The mixing of which pair of reactants will result in a precipitation reaction? A) CsI(aq) + NaOH(aq) B) HCl(aq) + Ca(OH)2(aq) C) K2SO4(aq) + Ba (NO3)2(aq) D) NaNO3(aq) + NH4Cl(aq)

C) K2SO4(aq) + Ba (NO3)2(aq)

Which of the following is NOT a strong electrolyte? A) LiOH B) CaCl2 C) MgCO3 D) NaC2H3O2 E) Na2SO4

C) MgCO3

What element is undergoing oxidation (if any) in the following reaction? 2 MnO4-(aq) + 3 NO2-(aq) + H2O(l) → 2 MnO2(s) + 3 NO3-(aq) + 2 OH-(aq) A) Mn B) O C) N D) H E) This is not an oxidation-reduction reaction

C) N

Which pair of compounds is soluble in water? A) Hg2Cl2 and Hg2Br2 B) NiS and Li2S C) NH 4 I and Ni(NO3)2 D) Li NO3 and CuCO3

C) NH 4 I and Ni(NO3)2

Which one of the following compounds is soluble in water? A) Ca3(PO4)2 B) HgS C) Ni(NO3)2 D) MgCO3

C) Ni(NO3)2

Which one of the following compounds is insoluble in water? A) K2SO4 B) NaNO3 C) Pb SO4 D) Rb2CO3

C) Pb SO4

Which of the following pairs of aqueous solutions will form a precipitate when mixed? A) KOH + Li2S B) (NH4)2SO4 + LiCl C) Sr(C2H3O2)2 + Li2SO4 D) KNO3 + LiOH E) None of the above solution pairs will produce a precipitate

C) Sr(C2H3O2)2 + Li2SO4

When dissolved in water, RbOH behaves as A) an acid that forms Rb+ and OH- ions. B) an acid that forms RbO- and H+ ions. C) a base that forms Rb+ and OH- ions. D) a base that forms RbO- and H+ ions.

C) a base that forms Rb+ and OH- ions.

Determine the oxidation state of nitrogen in NO. A) +5 B) +3 C) 0 D) +2 E) +4

D) +2

Determine the oxidation state of S in K2SO4. A) -4 B) +2 C) +4 D) +6 E) -2

D) +6

What is the oxidation number of the sulfur atom in Li2SO4 ? A) -2 B) +2 C) +4 D) +6

D) +6

A student dissolved 5.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO3- ion are there in the final solution? A) 0.0 247 g B) 0.0 493 g C) 0.0 678 g D) 0. 136 g

D) 0. 136 g

If 42.389 g of Fe3Br2 is dissolved in enough water to give a total volume of 750 mL, what is the molarity of the solution? A) 0.327 M B) 0.0971 M C) 0.0327 M D) 0.173M E) 0.436 M

D) 0.173M

Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 1023 atoms of Fe according to the following reaction. 2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq) A) 0.374 g B) 1.33 g C) 1.14 g D) 0.187 g E) 1.51 g

D) 0.187 g

What is the concentration of nitrate ions in a 0.125 M Ba(NO3)2 solution? A) 0.125 M B) 0.0625 M C) 0.375 M D) 0.250 M E) 0.160 M

D) 0.250 M

Pure acetic acid ( ) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 15.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL. A) 1.89 × 103 M B) 31.5 M C) 0.0315 M D) 0.525 M E) 5.25 × 10-4 M

D) 0.525 M

What is the concentration of NO3- ions in a solution prepared by dissolving 15.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution? A) 0. 152 M B) 0. 305 M C) 0. 403 M D) 0.609 M

D) 0.609 M

How many sodium ions are present in 125.0 mL of 0.750 M Na3PO4 solution? A) 4.31 × 1021 ions B) 5.66 × 1022 ions C) 3.08 × 1024 ions D) 1.69 × 1023 ions E) 7.53 × 1022 ions

D) 1.69 × 1023 ions

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO3 and HI are mixed. A) 2 H+(aq) + SO32-(aq) → H2SO3(s) B) Mg2+(aq) + 2 I-(aq) → MgI2(s) C) 2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq)→ H2SO3(s) + MgI2(aq) D) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g) E) No reaction occurs.

D) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g)

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed. A) Li+(aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq) B) Li+(aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq) C) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) E) No reaction occurs.

D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)

Calculate the number of grams of solute in 250.0 mL of 0.179 M KOH. A) 78.4 B) 0.798 C) 2.51 ×103 D) 2.51 E) 7.98 × 10-4

D) 2.51

How many liters of a 0.0550 M Li F solution contain 0.163 moles of Li F? A) 3.37 L B) 1.48 L C) 8.97 L D) 2.96 L E) 1.12 L

D) 2.96 L

How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 2.75 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq) A) 50.9 mL B) 86.0 mL C) 102 mL D) 204 mL

D) 204 mL

How many of the following compounds are soluble in water? Cu(OH)2 LiNO3 NH4I Na2S A) 0 B) 1 C) 2 D) 3 E) 4

D) 3

How many grams of NaCl are required to make 300.0 mL of a 2.500 M solution? A) 58.40 g B) 175.3 g C) 14.60 g D) 43.83 g

D) 43.83 g

What volume (in mL) of 0.0887 M Mg Br2 solution is needed to make 275.0 mL of 0.0224 M Mg Br2 solution? A) 72.3 mL B) 91.8 mL C) 10.9 mL D) 69.4 mL E) 14.4 mL

D) 69.4 mL

Based on the balanced chemical equation shown below, determine the mass percent of Fe3+ in a sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride, SnCl2(aq), solution is required to completely react with the Fe3+ present in the ore sample. The chemical equation for the reaction is 2 Fe3+(aq) + Sn2+(aq) → 2 Fe2+(aq) + Sn4+(aq). A) 11.59% B) 18.13% C) 36.26% D) 72.52%

D) 72.52%

How many aluminum ions are present in 65.5 mL of 0.210 M Al I3 solution? A) 4.02 × 1023 aluminum ions B) 5.79 × 1024 aluminum ions C) 2.48 × 1022 aluminum ions D) 8.28 × 1021 aluminum ions E) 1.21 × 1022 aluminum ions

D) 8.28 × 1021 aluminum ions

According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) A) 97.4 mL B) 116 mL C) 43.0 mL D) 86.1 mL E) 58.1 mL

D) 86.1 mL

What element is undergoing reduction (if any) in the following reaction? Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s) A) Zn B) N C) O D) Ag E) This is not an oxidation-reduction reaction

D) Ag

All of the following compounds are soluble EXCEPT A) Ba(OH)2. B) Pb(NO3)2. C) ZnCl2. D) AgBr. E) Cu(C2H3O2)2.

D) AgBr.

Which of the following compounds is an Arrhenius base? A) C6H12O6 B) HOCl C) H2SO4 D) C3H7NH2

D) C3H7NH2

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed. A) K+(aq) + NO3-(aq) → KNO3(s) B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq) C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) D) Fe2+(aq) + S2-(aq) → FeS(s) E) No reaction occurs

D) Fe2+(aq) + S2-(aq) → FeS(s)

Which of the following pairs of aqueous solutions will form a precipitate when mixed? A) H F+ LiOH B) Li2S + H F C) K2CO3 + HNO3 D) MgCl2 + KOH E) All of these solution pairs will produce a precipitate.

D) MgCl2 + KOH

Which of the following is a gas-evolution reaction? A) 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) B) 2 H2(g) + O2(g) → 2 H2O(g) C) LiCl(aq) + NaNO3(aq) → LiNO3(aq) + NaCl(g) D) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l) E) None of the above are gas-evolution reactions.

D) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l)

Which of the following compounds is an Arrhenius base? A) CH3OH B) CH3CO2H C) HOCl D) SrOH

D) SrOH

Determine the name for H FO3. A) hydro fluoric acid B) hydro fluorus acid C) fluorate acid D) fluoric acid E) per fluoric acid

D) fluoric acid

Determine the oxidation state of nitrogen in NO2. A) +5 B) +3 C) 0 D) +2 E) +4

E) +4

Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M KCl to 250.0 mL. A) 0.160 M B) 0.0320 M C) 2.50 M D) 0.00800 M E) 0.0160 M

E) 0.0160 M

A solution is prepared by mixing 20.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution? A) 0.180 B) 8.33 C) 1.50 D) 0.0400 E) 0.120

E) 0.120

How many milliliters of 0.188 M solution are needed to neutralize 50.00 mL of 0.0789 M NaOH? A) 0.742 B) 8.39 × 10-3 C) 119 D) 0.0477 E) 21.0

E) 21.0

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? Hint: You will want to write a balanced reaction. A) 581 mL B) 173 mL C) 345 mL D) 139 mL E) 278 mL

E) 278 mL

How many moles of Na F are contained in 258.6 mL of 0.0296 M Na F solution? A) 1.31 × 10-3 mol B) 8.74 × 10-3 mol C) 1.14 × 10-3 mol D) 3.67 × 10-3 mol E) 7.65 × 10-3 mol

E) 7.65 × 10-3 mol

Which of the following compounds will undergo a gas-evolving reaction in an aqueous solution? A) CH3COOH B) HF C) HCl D) H2SO4 E) H2CO3

E) H2CO3

Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s) A) O B) H C) C D) Fe E) Li

E) Li

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed. A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s) B) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s) C) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s) D) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3(s) E) No reaction occurs.

E) No reaction occurs

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed. A) 2 H+(aq) + CO32-(aq) → H2CO3(s) B) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq) C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g) D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq) E) No reaction occurs.

E) No reaction occurs

What element is undergoing oxidation (if any) in the following reaction? 2 HCl(aq) + Ca(OH)2(aq) → 2 H2O(l) + 2 CaCl2(aq) A) H B) Cl C) Ca D) O E) This is not an oxidation-reduction reaction

E) This is not an oxidation-reduction reaction

Determine the name for aqueous H Br. A) bromic acid B) bromous acid C) hydro bromous acid D) hydrogen bromate E) hydro bromic acid

E) hydro bromic acid

Identify sugar. A) strong electrolyte, weak acid B) weak electrolyte, weak acid C) strong electrolyte, strong acid D) weak electrolyte, strong acid E) nonelectrolyte

E) nonelectrolyte

How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days. Why?

The concentration would slowly increase as water from the solution evaporated. This is because the amount of NaCl in the flask would remain constant while the amount of water decreases.