Chapter 4 Worksheet

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MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) According to the following balanced reaction, how many moles of NO are formed from 8.44moles of NO2 if there is plenty of water present?

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

A) 25.3 moles NOB) 1.83 moles NOC) 5.63 moles NOD) 2.81 moles NOE) 8.44 moles NO

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2) According to the following balanced reaction, how many moles of KO are required to exactlyreact with 5.44 moles of H2O?

4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g)

A) 8.33 moles H2OB) 10.9 moles H2OC) 16.7 moles H2OD) 2.72 moles H2OE) 4.87 moles H2O

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3) How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to thefollowing reaction? The molar mass of KNO3 is 101.11 g/mol.

4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

A) 0.724 mol O2B) 0.290 mol O2C) 0.580 mol O2D) 18.5 mol O2E) 1.73 mol O2

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4) Two samples of potassium iodide are decomposed into their constituent elements. The firstsample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4kg of potassium, how many kg of iodine were produced?A) 79.4 kg B) 13.3 kg C) 22.5 kg D) 92.4 kg E) 44.4 kg

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5) A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the onlyproduct, what mass of ammonia is formed?A) 1.10 g B) 17.01 g C) 3.02 g D) 14.01 g E) 23.07 g

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6) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 8.000 moles ofC8H18 with 4.000 moles of O2.

2 C8H18 + 25 O2 → 16 CO2 + 18 H2OA) 20.00% B) 50.00% C) 25.00% D) 12.50%

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7) Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 reactwith excess Al according to the following reaction.

Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)A) 81.93 % B) 57.30 % C) 20.02 % D) 28.65 % E) 61.03 %

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8) Which of the following solutions will have the highest concentration of chloride ions?A) 0.10 M AlCl3B) 0.10 M MgCl2C) 0.05 M CaCl2D) 0.10 M NaClE) All of these solutions have the same concentration of chloride ions.

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9) How many milliliters of a 0.184 M NaNO3 solution contain 0.113 moles of NaNO3?A) 885 mL B) 326 mL C) 163 mL D) 614 mL E) 543 mL

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10) How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?A) 8.74 × 10-3 molB) 1.14 × 10-3 molC) 1.31 × 10-3 molD) 3.67 × 10-3 molE) 7.65 × 10-3 mol

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

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

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

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14) How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3mL of 0.140 M sucrose solution?A) 1.63 × 1023 molecules C12H22O11B) 5.90 × 1024 molecules C12H22O11C) 8.29 × 1022 molecules C12H22O11D) 1.21 × 1021 molecules C12H22O11E) 6.15 × 1022 molecules C12H22O11

14)

15) According to the following reaction, what volume of 0.244 M KCl solution is required to reactexactly 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) 86.1 mL C) 43.0 mL D) 58.1 mL E) 116 mL

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16) According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KClsolution? Assume that there is excess Pb(NO3)2.

2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)

A) 3.59 g B) 1.80 g C) 1.30 g D) 5.94 g E) 7.19 g

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17) Identify HCl.A) strong electrolyte, strong acidB) weak electrolyte, strong acidC) weak electrolyte, weak acidD) strong electrolyte, weak acidE) nonelectrolyte

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18) Identify sugar.A) weak electrolyte, weak acidB) nonelectrolyteC) strong electrolyte, weak acidD) strong electrolyte, strong acidE) weak electrolyte, strong acid

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19) How many of the following compounds are soluble in water?

Cu(OH)2 LiNO3 NH4Br K2S

A) 1 B) 2 C) 4 D) 3 E) 0

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20) Which of the following compounds is soluble in water?A) CaSB) BaSO4C) PbCl2D) MgCO3E) None of these compounds is soluble in water.

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21) Which of the following compounds is insoluble in water?A) Hg2I2B) BaSC) MgSO4D) (NH4)2CO3E) All of these compounds are soluble in water.

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22) Which of the following is a precipitation reaction?A) HCl(aq) + KOH(aq) → KCl(aq) + H2O(l)B) Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq)C) 2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq)D) NaCl(aq) + LiI(aq) → NaI(aq) + LiCl(aq)E) None of the above are precipitation reactions.

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23) Which of the following pairs of aqueous solutions will form a precipitate when mixed?A) K2CO3 + HNO3B) HCl + LiOHC) MgCl2 + KOHD) Li2S + HClE) All of these solution pairs will produce a precipitate.

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24) Which of the following pairs of aqueous solutions will form a precipitate when mixed?A) Na2 SO4 + KOHB) K2CO3 + NaClC) CaS + Na2SO4D) None of these solution pairs will produce a precipitate.E) All of these solution pairs will produce a precipitate.

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25) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions ofH2SO4 and KOH are mixed.

A) H22+(aq) + OH-(aq) → H2(OH)2(l)

B) 2 K+(aq) + SO42-(aq) → K2SO4(s)

C) H+(aq) + OH-(aq) → H2O(l)

D) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s)E) No reaction occurs.

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

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

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

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29) What element is undergoing oxidation (if any) in the following reaction?

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

A) OB) CC) HD) both C and HE) None of the elements is undergoing oxidation.

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30) What element is undergoing reduction (if any) in the following reaction?

Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)

A) NB) OC) AgD) ZnE) This is not an oxidation-reduction reaction.

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31) Identify the oxidation state of H in HCl(aq).

Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)A) +1 B) 0 C) +2 D) -1 E) -2

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32) Balance the chemical equation given below, and determine the number of milliliters of 0.00300 Mphosphoric acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide.

________ Ca(OH)2(aq) + ________ H3PO4(aq) → ________ Ca3(PO4)2(aq) + ________H2O(l)

A) 33.8 mL B) 15.0 mL C) 3.04 mL D) 22.5 mL

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33) According to the balanced equation shown below, 4.00 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) 9.00 B) 4.00 C) 8.00 D) 1.60

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34) Which one of the following compounds is soluble in water?A) CoS B) Cu3(PO4)2 C) ZnCO3 D) Pb(NO3)2

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35) Which one of the following compounds is insoluble in water?A) K2CO3 B) NaNO3 C) Ca Cl2 D) Pb Cl2

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36) The mixing of which pair of reactants will result in a precipitation reaction?A) NaNO3(aq) + NH4Cl(aq) B) CsI(aq) + NaOH(aq)C) HCl(aq) + Ca(OH)2(aq) D) K2SO4(aq) + Hg2(NO3)2(aq)

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37) Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:

Pb2+ (aq) + 2I- (aq) → PbI2 (s)

Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. Howmany milliliters of 3.550 M HI(aq) must be added to a solution containing 0.700 mol ofPb(NO3)2 (aq) to completely precipitate the lead?A) 0.197 mLB) 197 mLC) 0.394 mLD) 394 mLE) 2.54 × 10-3 mL

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38) What reagent could not be used to separate Br- from CO32- when added to an aqueous solutioncontaining both?A) AgNO3 (aq) B) Fe(NO3)2(aq) C) Cu(NO3)2 (aq) D) Ca(NO3)2 (aq)

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

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Answer KeyTestname: UNTITLED3

1) D2) B3) A4) A5) B6) C7) A8) A9) D10) E11) C12) B13) B14) D15) B16) A17) A18) B19) D20) A21) A22) C23) C24) C25) C26) C27) B28) A29) B30) C31) A32) B33) D34) D35) D36) D37) D38) A39) E

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