Deck 4: Chemical Reactions and Solutions Stoichiometry

Question 1

A 6.70-g sample consisting of a mixture of silver nitrate and sodium nitrate is dissolved in water. This aqueous mixture then reacts with aqueous barium chloride to form 3.60 g of silver chloride. Calculate the percent by mass of silver nitrate in the first mixture.

A) 63.7%
B) 45.3%
C) 42.7%
D) 43.8%
E) 78.0%

Answer 1

63.7%

Question 2

A 230.-mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the solution is 1.10 M. What volume of solvent has evaporated from the 0.275 M solution? (Assume volumes are additive.)

A) 288 mL
B) 172 mL
C) 63.3 mL
D)230. mL
E) 58.0 mL

Answer 2

172 mL

Question 3

You dissolve 15.71 g of NH4NO3 in 150.0 mL of solution (call this solution A). You take 20.0 mL of solution A and add water until the total volume is 75.0 mL (call this solution B). You take 15.0 mL of solution B and add 25.0 mL of water to it (call this solution C). You mix 10.0 mL of solution B and 10.0 mL of solution C (call this solution D). What is the concentration of ammonium nitrate in solution D?

A) 0.240 M
B) 0.190 M
C) 0.131 M
D) 0.279 M
E) none of these

Answer 3

A

Question 4

What volume of 0.504 M barium nitrate solution is needed to prepare 218.0 mL of a solution that is 0.244 M in nitrate?

A) 4.50 *10² mL
B) 5.28 * 10¹ mL
C) 3.52 * 10¹ mL
D) 1.06 *10² mL
E) 2.11 *10² mL

Question 5

1.00 mL of a 3.50 *10^-4 M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming solution A. 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. How many grams of oleic acid are in 5.00 mL of solution B? (molar mass for oleic acid = 282 g/mol)

A) 9.87 *10^-6 g
B)4.94 * 10^-5 g
C)4.94 * 10^-4 g
D)1.97* 10^-6 g
E)7.00 *10^-6 g

Question 6

To calculate the concentration in molarity of a salt solution, you need to know

A) the molar mass of the salt and the total volume of the solution.
B) the mass of the salt added, the molar mass of the salt, the volume of water added, and the total volume of the solution.
C) the mass of the salt added to the solution and the volume of water added to the solution.
D) the mass of the salt added, the molar mass of the salt, and the total volume of the solution.
E) the mass of the salt added to the solution and the total volume of the solution.

Question 7

What volume of 2.0 M HCl can be prepared from 2.00 L of 9.00 M HCl?

A) 444 mL
B) 4.50 L
C) 2.25 L
D) 9.00 L
E) none of these

Question 8

A 51.24-g sample of Ba(OH)₂ is dissolved in enough water to make 1.20 L of solution. How many milliliters of this solution must be diluted with water in order to make 1.00 L of 0.100 molar Ba(OH)₂?

A) 278 mL
B) 333 mL
C)400. mL
D) 249 mL
E) 1.20 *10³ mL

Question 9

A 16.2-g sample of HF is dissolved in water to give 2.6 *10² mL of solution. The concentration of the solution is

A) 6.2 M
B) 0.21 M
C) 4.2 M
D) 0.81 M
E) 3.1 M

Question 10

Mixing 40.0 mL of a 4.00 M sodium chloride solution with 20.0 mL of a 5.00 M calcium chloride solution results in a solution with a chloride ion concentration of

A) 4.33 M.
B) 6.00 M.
C) 4.50 M.
D) 7.00 M.
E) none of these

Question 11

Nonelectrolytes are insoluble in water.

Question 12

What volume of 12.0 M HCl is required to prepare 16.0 L of 0.250 M hydrochloric acid?

A) 768 mL
B) 333 mL
C) 585 mL
D)130. mL
E) none of these

Question 13

The concentration of a 300.0-mL sample of a calcium chloride solution is 0.256 M. What is the mass of the solute?

A) 8.52 g
B) 5.80 g
C) 2.70 g
D) 95 g
E) 28.4 g

Question 14

What volume of 6.60 M potassium hydroxide is required to prepare 53.6 mL of 0.450 M KOH?

A) 786 mL
B) 0.0554 mL
C) 3.65 mL
D) 6.31 mL
E) 1.35 mL

Question 15

If a student needs to make a 0.10 M solution of NaHCO₃, how many milliliters of solution can be made using a 0.35-g sample of NaHCO₃?

A) 4.2 mL
B) 1.0 * 10² mL
C) 35 mL
D) 3.5 mL
E) 42 mL

Question 16

How much water must be added to 20.0 mL of a 9.50 M sulfuric acid solution to make a 0.480 M solution? (Assume volumes are additive.)

A) 81.0 mL
B) 376 mL
C) 396 mL
D) 101 mL
E) none of these

Question 17

How many grams of Na₂SO₄ are required to make 150.0 mL of a 0.180 M sodium sulfate solution?

A) 3.40 g
B) 3.84 g
C) 3.21 g
D) 2.78 g
E) none of these

Question 18

Consider five solutions that all have the same mass of solute in 100.0 mL of solution. Which has the highest concentration as measured in molarity?

A) Na₂SO₄
B) NaF
C) KCl
D) CaCl₂
E) NaCl

Question 19

You have 120.0 mL of a 0.245 M solution of NaCl sitting in a beaker. After several days you test the solution and find that it has a concentration of 0.348 M. How much water must have evaporated? (Assume volumes are additive.)

A) 84.5 mL
B) 35.5 mL
C)120. mL
D) 204 mL
E) 119 mL

Question 20

Which of the following solutions contains the greatest total ion concentration?

A) One mole of sodium phosphate dissolved in 1.0 L of solution.
B) One mole of potassium hydroxide dissolved in 1.0 L of solution.
C) One mole of iron(II) nitrate dissolved in 1.0 L of solution.
D) One mole of potassium chloride dissolved in 1.0 L of solution.
E) At least two of these solutions have an equal number of ions, and these contain the greatest total ion concentration.

Question 21

Reacting 42.8 mL of 0.320 M AgNO₃ with 55.8 mL of 0.580 M K₂CrO₄ results in what mass of solid formed?

A) 3.27 g
B) 7.25 g
C) 2.27 g
D) 3.07 g
E) 10.74 g

Question 22

If all of the chloride in a 5.000-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO₃, what is the percentage of chloride in the sample?

A) 1.425%
B) 20.22%
C) 50.55%
D) 10.10%
E) none of these

Question 23

A solution contains the ions Ag⁺, Pb²⁺, and Ni²⁺. Dilute solutions of NaCl, Na₂SO₄, and Na₂S are available to separate the positive ions from each other. In order to effect separation, the solutions should be added in which order?

A) Na₂S, NaCl, Na₂SO₄
B) Na₂SO₄, NaCl, Na₂S
C) Na₂SO₄, Na₂S, NaCl
D) NaCl, Na₂S, Na₂SO₄
E) NaCl, Na₂SO₄, Na₂S

Question 24

Select the unbalanced net ionic equation for the reaction between aqueous lead nitrate and aqueous potassium iodide.

A) Pb(NO₃)₂(aq) + KI(aq) $\rightarrow$ PbI₂(s) + KNO₃(aq)
B) Pb²⁺(aq) + I^-(aq) $\rightarrow$ PbI₂(s)
C) Pb²⁺(aq) + NO₃^-(aq) + K⁺(aq) + I^-(aq) $\rightarrow$ PbI₂(s) + K⁺(aq) + NO₃^-(aq)
D) Pb²⁺(aq) + NO₃^-(aq) + K⁺(aq) + I^-(aq) $\rightarrow$ Pb²⁺(aq) + I^-(aq) + K⁺(aq) + NO₃^-(aq)
E) none of these

Question 25

Lead(II) nitrate reacts with sodium chloride in aqueous solution to form a precipitate. What is the net ionic equation for this reaction?

A) Na⁺(aq) + Cl^2-(aq) $\rightarrow$ Na₂Cl(s)
B) Na⁺(aq) + NO₃^-(aq) $\rightarrow$ NaNO₃(s)
C) Pb²⁺(aq) + 2NO₃^-(aq) $\rightarrow$ Pb(NO₃)₂(s)
D) Na⁺(aq) + Cl^-(aq) $\rightarrow$ NaCl(s)
E) Pb²⁺(aq) + 2Cl^-(aq) $\rightarrow$ PbCl₂(s)

Question 26

An aqueous solution of barium nitrate reacts with an aqueous solution of sodium sulfate. Identify the solid and indicate its coefficient in the balanced equation.

A) BaSO_{4 ,} 1
B) NaNO_{3 ,} 1
C) BaSO_{2 ,} 2
D) NaNO_{3 ,} 2
E) none of these

Question 27

You dissolve a 1.28-g sample of NaCl in a total volume of 125.0 mL of solution. Your lab partner has 1.50 M aqueous NaCl and wants to make a solution with the same concentration and volume as yours. How much of the solution does your lab partner need to use?

A) 1.83 mL
B) 14.6 mL
C) 125 mL
D) 107 mL
E) none of these

Question 28

When NH₃(aq) is added to Cu²⁺(aq), a precipitate initially forms. What is its formula?

A) CuO
B) Cu(NH₃)
C) Cu(OH)₂
D) Cu(NO₃)₂
E)

Question 29

A 4.000-g sample of the metal nitrate M(NO₃)₂ was dissolved in water and treated with excess aqueous sodium sulfate. The sulfate salt that formed weighed 3.318 g. Determine the identity of the metal.

A) Pb
B) Ca
C) Ba
D) K
E) none of these

Question 30

Which one of the following basic solutions will not neutralize 25.0 mL of a 1.0 M sulfuric acid solution?

A) 100.0 mL of 0.50 M NaOH
B) 25.0 mL of 1.0 M NaOH
C) 50.0 mL of 1.0 M NaOH
D) 25.0 mL of 2.0 M KOH
E) All of these will neutralize 25.0 mL of a 1.0 M sulfuric acid solution.

Question 31

Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?

A) Ni²⁺, SO₄^2-
B) Al³⁺, S^2-
C) Mn²⁺, OH^-
D) Co²⁺, PO₄^3-
E) Ag⁺, Cl^-

Question 32

Magnesium metal reacts with hydrochloric acid to form aqueous magnesium chloride and hydrogen gas. When 3.65 g of magnesium is added to 50.0 mL of 3.00 M hydrochloric acid, what mass of hydrogen is produced, assuming a complete reaction?

A) 0.302 g
B) 0.246 g
C) 0.151 g
D) 0.123 g
E) none of these

Question 33

An aqueous solution of silver nitrate is added to an aqueous solution of potassium chromate, and this reaction produces a solid. What is the formula for the solid?

A) AgCrO₄
B) KNO₃
C) AgK
D) K₂NO₃
E) Ag₂CrO₄

Question 34

Consider the reaction between 50.0 mL of 0.200 M sodium hydroxide and 75.0 mL of 0.100 M HCl. Which of the following statements is correct?

A) The NaOH is the limiting reactant.
B) After the reaction, the concentration of Na⁺ is greater than the concentration of OH^-.
C) After the reaction, the concentration of Na⁺ is equal to the concentration of Cl^-.
D) After the reaction, the concentration of Na⁺ is still 0.200 M because Na⁺ is a spectator ion.
E) None of these are correct.

Question 35

A mixture contained no fluorine compound except methyl fluoroacetate, FCH₂COOCH₃ (molar mass = 92.1 g/mol. When chemically treated, all the fluorine was converted to CaF₂ (molar mass = 78.1 g/mol). The mass of CaF₂ obtained was 12.1 g. Find the mass of methyl fluoroacetate in the original mixture.

A) 28.5 g
B) 92.0 g
C) 14.3 g
D) 24.2 g
E) 12.1 g

Question 36

When aqueous sodium hydroxide is added to aqueous nitric acid, what is the balanced molecular equation for the reaction that takes place?

A) 2NaOH(aq) + H₂NO₃(aq) $\rightarrow$ Na₂NO₃(aq) + 2H₂O(l)
B) NaOH(aq) + HNO₃(aq) $\rightarrow$ NaNO₃(aq) + H₂O(l)
C) NaOH(aq) + HNO₂(aq) $\rightarrow$ NaNO₂(aq) + H₂O(l)
D) Na(OH)₂(aq) + H₂NO₃(aq) $\rightarrow$ Na₂NO₃(aq) + 2H₂O(l)
E) NaOH(aq) + HNO₄(aq) $\rightarrow$ NaNO₄(aq) + H₂O(l)

Question 37

What is the net ionic equation for the reaction of aqueous sodium hydroxide with aqueous nitric acid?

A) Na⁺(aq) + OH^-(aq) + H⁺(aq) + NO₃^-(aq) $\rightarrow$ NaOH(s) + HNO₃(l)
B) H⁺(aq) + OH^-(aq) $\rightarrow$ H₂O(l)
C) Na⁺(aq) + OH^-(aq) $\rightarrow$ NaOH(s)
D) Na⁺(aq) + OH^-(aq) + H⁺(aq) + NO₃^-(aq) $\rightarrow$ Na⁺(aq) + NO₃^-(aq) + H₂O(l)
E) none of these

Question 38

High concentrations of aqueous solutions of sodium sulfide and nickel(II) nitrate are mixed together. Which statement is correct?

A) Both NaNO₃ and NiS precipitate from solution.
B) No precipitate forms.
C) NiS will precipitate from solution.
D) NaNO₃ will precipitate from solution.
E) No reaction will occur.

Question 39

You mix 50.0 mL of 2.00 M lead(II) nitrate with 50.0 mL of 2.00 M sodium chloride. What mass of lead(II) chloride should you form?

A) 12.1 g
B) 13.9 g
C) 27.8 g
D) 24.3 g
E) none of these

Question 40

When 0.2 M sodium hydroxide and 0.2 M barium nitrate are mixed, a precipitate is formed. What is the net ionic equation for the formation of this precipitate?

A) Na⁺(aq) + NO₃^-(aq) $\rightarrow$ NaNO₃(s)
B) Na⁺(aq) + OH^-(aq) $\rightarrow$ NaOH(s)
C) Ba²⁺(aq) + 2NO₃^-(aq) $\rightarrow$ Ba(NO₃) ₂(s)
D) Ba²⁺(aq) + 2OH^-(aq) $\rightarrow$ Ba(OH)₂(s)
E) none of these

Question 41

A 0.350-g sample of an acid, HX, requires 25.4 mL of a 0.140 M NaOH solution for complete reaction. Calculate the molar mass of the acid.

A) 98.4 g/mol
B) 121.3 g/mol
C) 42.3 g/mol
D) 68.4 g/mol
E) none of these

Question 42

In which state of the following compounds does nitrogen have the most positive oxidation state?

A) NaNO₂
B) N₂O
C) HNO₃
D) NO₂
E) NH₄Cl

Question 43

What volume of 0.25 M HNO₃ is necessary to react exactly with 7.4 g of Ca(OH)₂?

A) 8.0 * 10² mL
B) 1.2 *10² mL
C) 4.0 *10² mL
D) 2.5* 10² mL
E) 2.0 *10² mL

Question 44

Calculate the concentration of NaOH if 26.2 mL reacts exactly with 24.4 mL of 0.311 M HCl.

A) 0.145 M
B) 0.334 M
C) 0.290 M
D) 0.579 M
E) 0.311 M

Question 45

What are the oxidation numbers of carbon in CO₂ and CO₃^2-, respectively?

A) +2, +6
B) +4, +4
C) -4, -4
D) +4, +6
E) -4, -6

Question 46

What is the oxidation state of chromium in K₂Cr₂O₇?

A) +4
B) -3
C) +2
D) -5
E) +6

Question 47

In the following reaction, which species is the reducing agent?
3Cu + 6H⁺ + 2HNO₃ $\rightarrow$ 3Cu²⁺ + 2NO + 4H₂O

A) N in HNO₃
B) Cu
C) H⁺
D) N in NO
E) Cu²⁺

Question 48

A 0.382-g sample of an unknown triprotic acid is titrated to the third equivalence point using 32.6 mL of 0.239 M NaOH. Calculate the molar mass of the acid.

A) 7.79 g/mol
B) 1.47 *10² g/mol
C) 16.3 g/mol
D) 52.1 g/mol
E) 49.0 g/mol

Question 49

In the reaction Zn(s) + Cu(NO₃)₂(aq) $\rightarrow$ Zn(NO₃)₂(aq) + Cu(s), identify the oxidizing agent.

A) Cu
B) Cu(NO₃)₂
C) O₃
D) Zn
E) Zn(NO₃)₂

Question 50

The following reaction occurs in aqueous acid solution: NO₃^- + I^- $\rightarrow$ IO₃^- + NO₂
What is the oxidation state of iodine in IO₃^-?

A) (+5)
B) 0
C) (-3)
D) (-5)
E) (+3)

Question 51

In the reaction Zn + H₂SO₄ $\rightarrow$ ZnSO₄ + H₂, which element, if any, is oxidized?

A) zinc
B) hydrogen
C) oxygen
D) sulfur
E) none of these

Question 52

You have separate aqueous solutions of NaOH and Ca(OH)₂ with the same concentrations. You wish to neutralize an aqueous solution of HCl. Which basic solution would require more volume to neutralize the acid?

A) You need to know the volume and concentration of the HCl solution to answer this question.
B) You need to know the concentrations of the basic solutions to answer this question.
C) the NaOH solution
D) You need to know the concentrations of the acid and bases and the volume of the acid to answer this question.
E) the Ca(OH)₂ solution

Question 53

A student weighs out 0.568 g of KHP (molar mass = 204 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid with one acidic proton.

A) 0.943 M
B) 3.15 M
C) 0.0757 M
D) 0.100 M
E) none of these

Question 54

Which of the following is not an oxidation-reduction reaction?

A) A reaction in which a metal reacts with a nonmetal
B) A combustion reaction
C) A precipitation reaction
D) A metal reacting with an acid
E) All of these are oxidation-reduction reactions

Question 55

Which of the following reactions does not involve oxidation-reduction?

A) LiOH + HCl $\rightarrow$ H₂O + LiCl
B) Mg + 2HI $\rightarrow$ MgI₂ + H₂
C) 2Na + 2H₂O $\rightarrow$ 2NaOH + H₂
D) MnO₂ + 4HI $\rightarrow$ I₂ + 2H₂O + MnI₂
E) CH₄ + 2O₂ $\rightarrow$ 2H₂O + CO₂

Question 56

When aqueous solutions of silver nitrate and potassium chromate are mixed, the blood-red precipitate silver chromate is formed. If 10.0 mL of 0.25 M aqueous silver nitrate is mixed with 15.0 mL of 0.14 M aqueous potassium chromate, what is the total concentration of ions in the solution after the precipitate is formed?

A) 0.14 M
B) 0.39 M
C) 0.30 M
D) 0.50 M
E) 0.25 M

Question 57

Which of the following statements is(are) true? Oxidation and reduction
I.Cannot occur independently of each other.
II.Accompany all chemical changes.
III.Describe the loss and gain of electron(s), respectively.
IV.Result in a change in the oxidation states of the species involved.

A) I only
B) II only
C) III only
D) IV only
E) I, III, and IV

Question 58

Sulfamic acid, HSO₃NH₂ (molar mass = 97.1 g/mol), is a strong monoprotic acid that can be used to standardize a strong base: HSO₃NH₂(aq) + KOH(aq) $\rightarrow$ KSO₂NH₂(aq) + H₂O(l)
A 0)179-g sample of HSO₃NH₂ required 19.4 mL of an aqueous solution of KOH for complete reaction. What is the molarity of the KOH solution?

A) 9.25 M
B) 0.194 M
C) 9.50 *0^-5 M
D) 0.0950 M
E) none of these

Question 59

You are titrating a solution of sodium hydroxide of unknown concentration with a solution of phosphoric acid that has a concentration of 0.300 M. Starting with 29.0 mL of the sodium hydroxide solution, you use 16.8 mL of the acid to titrate the base to completion. Calculate the concentration of the sodium hydroxide solution.

A) 0.518 M
B) 0.174 M
C) 0.0579 M
D) 0.521 M
E) 0.348 M

Question 60

What volume of 0.350 M KOH is required to react completely with 24.0 mL of 0.650 M H₃PO₄?

A) 52.0 mL
B) 156 mL
C) 26.0 mL
D) 104 mL
E) none of these

Question 61

In the balanced equation for the following redox equation, what is the sum of the coefficients? Fe³⁺ + I^- $\rightarrow$ Fe²⁺ + I₂

A) 7
B) 4
C) 6
D) 8
E) 5

Question 62

Which of the following is(are) oxidation-reduction reactions?
I.PCl₃ + Cl₂ $\rightarrow$ PCl₅
II.Cu + 2AgNO₃ $\rightarrow$ Cu(NO₃)₂ + 2Ag
III.CO₂ + 2LiOH $\rightarrow$ Li₂CO₃ + H₂O
IV.FeCl₂ + 2NaOH $\rightarrow$ Fe(OH)₂ + 2NaCl

A) I, II, III, and IV
B) I and II only
C) I, II, and III only
D) IV only
E) III only

Question 63

When the following reaction is balanced in acidic solution, what is the coefficient of water? Zn(s) + NO₃^-(aq) $\rightarrow$ Zn²⁺(aq) + NH₄⁺(aq)

A) 2
B) 3
C) 1
D) 4
E) none of these

Question 64

For the reaction of sodium bromide with chlorine gas to form sodium chloride and bromine, what are the appropriate half-reactions? (ox = oxidation and re = reduction)

A) ox: 2Br^- $\rightarrow$ Br₂ + 2e^-; re: Cl₂ + 2e^- $\rightarrow$ 2Cl^-
B) ox: Br + 2e^- $\rightarrow$ Br^2-; re: 2Cl^- $\rightarrow$ Cl₂ + 2e^-
C) ox: Cl₂ + 2e^- $\rightarrow$ 2Cl^-; re: 2Br^- $\rightarrow$ Br₂ + 2e^-
D) ox: 2Na⁺ + 2e^- $\rightarrow$ 2Na; re: 2Cl^- $\rightarrow$ Cl₂ + 2e^-
E) ox: Cl + e^- $\rightarrow$ Cl^-; re: Br $\rightarrow$ Br^- + e^-

Question 65

For the redox reaction 2Fe²⁺ + Cl₂ $\rightarrow$ 2Fe³⁺ + 2Cl^-, which of the following are the correct half-reactions?
I.Cl₂ + 2e^- $\rightarrow$ 2Cl^-
II.Cl $\rightarrow$ Cl^- + e^-
III.Cl₂ $\rightarrow$ 2Cl^- + 2e^-
IV.Fe²⁺ $\rightarrow$ Fe³⁺ + e^-
V.Fe²⁺ + e^- $\rightarrow$ Fe³⁺

A) I and V
B) I and IV
C) III and IV
D) II and IV
E) II and V

Question 66

The equation 2C₂H₆ + 7O₂ $\rightarrow$ 4CO₂ + 6H₂O is an oxidation-reduction reaction.

A) True; the carbon is oxidized and the hydrogen is reduced.
B) True; the carbon is reduced and the oxygen is oxidized.
C) False
D) True; the oxygen is reduced and the hydrogen is oxidized.
E) True; the carbon is oxidized and oxygen is reduced.

Question 67

The following unbalanced reaction occurs in basic media: Fe²⁺ + Cr₂O₇^2- $\rightarrow$ Fe³⁺ + Cr³⁺
The coefficient for water in the balanced equation is __________, and water appears on the __________ side of the equation.

A) 14, left
B) 14, right
C) 7, right
D) 7, left
E) none of these

Question 68

With what volume of 2.5 M HF will 6.4 g of calcium hydroxide react completely, according to the reaction 2HF + Ca(OH)₂ $\rightarrow$ CaF₂ + 2H₂O?

A) 1.6*10¹ mL
B) 2.6 * 10¹ mL
C) 1.6 *10² mL
D) 6.9 *10¹ mL
E) 3.5 * 10¹ mL

Question 69

Identify each of the following unbalanced reactions using the following choices:

-H₂SO₄ + Ba(OH)₂ $\rightarrow$ BaSO₄ + H₂O

A)Precipitation reaction
B)Acid-base reaction
C)Oxidation-reduction reaction
D)Combustion reaction
E)More than one of answers a-d apply.

Question 70

When the equation Cl₂ $\rightarrow$ Cl^- + ClO₃^- (basic solution) is balanced using the smallest whole-number coefficients, what is the coefficient of OH^-?

A) 1
B) 2
C) 3
D) 4
E) 6

Question 71

The ion MnO₄^- is often used to analyze for the Fe²⁺ content of an aqueous solution by using the reaction MnO₄^- + Fe²⁺ $\rightarrow$ Fe³⁺ + Mn²⁺
In acidic solution. A 54.4-mL sample of a solution containing Fe²⁺ requires 33.3 mL of a 0.022 M KMnO₄ solution for complete reaction. What is the concentration of the Fe²⁺ in the original solution?

A) 6.7 *10^-2 M
B) 1.3 * 10^-2 M
C) 3.6 *10^-1 M
D) 4.0 * 10^-2 M
E) 2.7 *10^-3 M

Question 72

The following reaction occurs in aqueous acid solution: NO₃^- + I^- $\rightarrow$ IO₃^- + NO₂
In the balanced equation, what is the coefficient of NO₃^-?

A) 2
B) 3
C) 4
D) 5
E) 6

Question 73

Balance the reaction below in acidic aqueous solution, using the oxidation number method. In the balanced equation, what is the coefficient of Fe²⁺? ClO₂^- + Fe²⁺ $\rightarrow$ Cl^- + Fe³⁺

A) 5
B) 4
C) 8
D) 1
E) 7

Question 74

In the reaction 3Cu(s) + 8HNO₃(aq) $\rightarrow$ 3Cu(NO₃)₂(aq) + 4H₂O(l) + 2NO(g)
6.3 g of Cu and 100.0 mL of 1.0 M HNO₃ are combined. Which of the following statements is true?

A) Cu and HNO₃ react in a 1:1 mole ratio.
B) Cu is the limiting reagent, and 0.062 mol HNO₃ does not react.
C) 0.080 mol H₂O is produced
D) HNO₃ is the limiting reagent, and 0.062 mol Cu does not react.
E) Cu and HNO₃ are present in stoichiometric amounts; neither is in excess.

Question 75

Selecting from the following, indicate which reagents would be mixed to produce Cu(OH)₂.

Question 76

The following reaction occurs in aqueous acid solution: NO₃^- + I^- $\rightarrow$ IO₃^- + NO₂
In the balanced equation, what is the coefficient of water?

A) 3
B) 2
C) 4
D) 1
E) 5

Question 77

Balance the reaction below in acidic solution. IO₃^- + I^- $\rightarrow$ I₂
What volume of 0.352 M HCl is needed to produce 2.48 *10^-3 mol of iodine, I₂, with an excess of KIO₃ and KI?

A) 14.1 mL
B) 4.96 mL
C) 7.05 mL
D) 2.48 mL
E) none of these

Question 78

Write the balanced molecular equation for the reaction between aqueous solutions of lithium phosphate and sodium hydroxide.

Question 79

The following equation describes the oxidation of ethanol to acetic acid by potassium permanganate: 3C₂H₅OH + 4KMnO₄ $\rightarrow$ 3HC₂H₃O₂ + 4MnO₂ + 4KOH + H₂O
5)0 g of ethanol and an excess of aqueous KMnO₄ are reacted, and 5.9 g HC₂H₃O₂ results. What is the percent yield?

A) 5.9 g HC₂H₃O₂ is impossible because it represents more than a 100% yield.
B) 91%
C) 100%
D) 67%
E)30.%

Question 80

In the reaction 2MnO₄^- + 5H₂O₂ + 6H⁺ $\rightarrow$ 2Mn²⁺ + 8H₂O + 5O₂
What volume of 0.150 M KMnO₄ solution is needed to titrate 75.0 mL of a 0.150 M H₂O₂ solution?

A) 75.0 mL
B) 30.0 mL
C) 45.0 mL
D) 15.0 mL
E) none of these